Quizlet Chemistry Comp, Electrolysis (IGCSE), Electrolysis - IGCSE, Chemistry - Electrolysis, Electrolysis, Oxidation, Oxidation Numbers, Balancing oxidation-reduction equations, Redox Reactions, Redox Reaction, Balancing Chemical Equations, Balancin...
Adrenal genital syndrome
* virilism= congenital adrenal. Is secondary male characteristics
Carbon oxi#
+2,+4,-4
Apparatus used in a titration
- Pipette (to measure alkali) - Burette (to measure acid) - conical flask - retort stand - funnel - indicator
Acid reactions with ammonia
- acid + ammonia --> ammonium salt sulfuric acid + ammonia --> ammonium sulphate
How to test for carbonate ions
- add an acid (hydrochloric acid) - you can see if a gas is carbon dioxide by bubbling it through limewater - if the gas is carbon dioxide, it turns cloudy - if the limewater turns cloudy, then carbonate ions are present
CaS + H2O + CO2 -> Ca(HCO3)2 + H2S
...
CaS + H2O -> Ca(HS)2 + Ca(OH)2
...
size of needle for female
1-3
pH + pOH =
14
PH₃ + O₂ → P₄O₁₀ + H₂O
4PH₃ + 8O₂ → P₄O₁₀ + 6H₂O
In drinks, citrus, pop, etc.
Acid
What colour precipitate does Cu2+ produce when tested?
Blue precipitate
31. H2C2O4 + 2 H2O ⇄ 2 H3O+ + C2O42− Oxalic acid, H2C2O4, is a diprotic acid with K1 = 5 x 10−2 and K2 = 5 x 10−5. Which of the following is equal to the equilibrium constant for the reaction represented above? (A) 5 x 10−2 (B) 5 x 10−5 (C) 2.5 x 10−6 (D) 5 x 10−7 (E) 2.5 x 10−8
C
56. A 0.20-molar solution of a weak monoprotic acid, HA, has a pH of 3.00. The ionization constant of this acid is... (A) 5.0 x 10−7 (B) 2.0 x 10−7 (C) 5.0 x 10−6 (D) 5.0 x 10−3 (E) 2.0 x 10−3
C
Questions 9-12 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of substances. Assume all concentrations are 1 M. (A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 9. The solution with the lowest Ph
C
Cr (+2 charge)
Chromium (II)
All of the following species can function as Brönsted-Lowry bases in solution EXCEPT... (A) H2O (B) NH3 (C) S2− (D) NH4+ (E) HCO3−
D
what is the most heat resistant VIRUS in the worl
HBV; can be transmitted through sex or feces, food, water
Conjugate acid of Cl-
HCl
At the cathode...
Ions gain electrons.
What is an electrolyte?
Liquids that are good conductors of electricity
non-electrolytes are ......
Liquids that do not conduct electricity
MnO₂ + HCl → MnCl₂ + Cl₂ + H₂O
MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O
Ni (+2 charge)
Nickel
N₂ + F₂ → NF₃
N₂ + 3F₂ → 2NF₃
Concentrated sulfuric acid change
Pungent gas is produced
Sb₂S₃ + HCl → H₃SbCl₆ + H₂S
Sb₂S₃ + 12HCl → 2H₃SbCl₆ + 3H₂S
Scandium
Sc
Groin: the gonads
Secrete sex steroids. Male: androgens, female: estrogen + progrsterone
If a substance gives up the electrons readily it is known as a...?
Strong reducing agent
Electrolysis
The breaking down of an ionic compound when molten or in an aqueous solution by the passage of electricity.
SCN (-1 charge)
Thiocyanate
True or False The number of electrons lost must equal the number of electrons gained.
True
NAD+ and NADH
When it got reduced to NADH, the postive + went away NADH gained hydrogen ions and electrons
Oxidation of any free element is...?
Zero
Zn (+2 charge)
Zinc
__Mg + __Cl₂ --> __MgCl₂
balanced
__MgO + __SO₃ --> __MgSO₄
balanced
__PCl₃ + __Cl₂ --> __PCl₅
balanced
Kb is what constant? ____ _________
base dissociation
A pH of 14 is strongly
basic
In any aqueous solution, when [H+] increases, [OH-] _____
decreases
When [H+] ______, [OH-] increases
decreases
In NADH, NAD+'s reduced form.. it is carrying
hydrogen ions and electrons.. potential energy
miss follicle
incorrect angle, increased pain and bruising, red scabs, % of infection increases
How to make insoluble salts
ion
erythema
redness
concordant
results that agree (very close together)
(NH₄)₂Cr₂O₇ → Cr₂O₃ + H₂O + N₂
(NH₄)₂Cr₂O₇ → Cr₂O₃ + 4H₂O + N₂
(NH4)2BeF4 -> BeF2 + NH3 + HF
...
K3[Fe(SCN)6] + Na2Cr2O7 + H2SO4 -> Fe(NO3)3 + Cr2(SO4)3 + CO2 + H2O + Na2SO4 + KNO3
...
K4Fe(CN)6 + KMnO4 + H2SO4 -> KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 + H2O
...
K4[Fe(SCN)6] + K2Cr2O7 + H2SO4 -> Fe2(SO4)3 + Cr2(SO4)3 + CO2 + H2O + K2SO4 + KNO3
...
S + N₂O → SO₂ + N₂
1 S + 2 N₂O → 1 SO₂ + 2 N₂
SO₂ + H₂O → H₂SO₃
1 SO₂ + 1 H₂O → 1 H₂SO₃
SO₃ + H₂O → H₂SO₄
1 SO₃ + 1 H₂O → 1 H₂SO₄
SiC + Cl₂ → SiCl₄ + C
1 SiC + 2 Cl₂ → 1 SiCl₄ + 1 C
Method to make copper sulfate (crystals) with copper oxide and sulphuric acid
1) Add copper oxide and hot sulfuric acid to a beaker 2) Add copper oxide (i.e 3 spatulas) until it stops reacting with the acid/stops releasing carbon dioxide (fizzing) - this will tell us when all the acid has been used (saturated solution) CuO + H2SO4 --> CuSO4 + H2O 3) Filter the reaction mixture using a funnel with filter paper inside to remove excess copper carbonate. Once the process is over, pure copper sulfate solution is left in the flask 4) Leave to evaporate by putting the pure copper sulfate solution in an evaporating basin which is heated strongly by a Bunsen burner until half of the water has evaporated. Remaining water left to evaporate over a number of hours to form copper sulfate crystals
How to test for sulfate ions
1) Add dilute hydrochloric acid to the substance - this will remove any cabronates/sulfites which may react with the barium ions to form white precipitate. This can result to confusion in our results 2) Add barium chloride solution (containing barium ions) 3) If any sulfate ions are present, white precipitate will form which will be a positive result
__N₂ + __O₂ --> __NO
1, 1, 2
size of needle for male
4-5
Bitter taste
Base
sulfur dioxide
SO2
Sulphuric acid forms
Sulfate salts
SO3 (-2 charge)
Sulfite
Punngent gas produced
Sulfur dioxide
Hydrochloric acid forms
chlorine salts
What does respiration mean?
exchange of gases.. Respiration is when oxygen from the air move into the cells and the C02 in the cells moves out.
Are humans efficient at harvesting energy?
no. we must strip electron's energy off very slowly, making us inefficient at it.
K2Cr207
potassium dichromate
Base
- any substance that has a pH greater than 7 - if a base dissolves in water, it is called an alkali
titre
- the concentration of a solution determined by the titration - the minimum volume of a solution needed to reach the end point in a titration.
(NH4)2Cr2O7 -> NH3 + H2O + Cr2O3 + O2
...
(NH4)3AsS4 + HCl -> As2S5 + H2S + NH4Cl
...
Ag2S + KCN -> KAg(CN)2 + K2S
...
AgNO3 + FeCl3 -> Fe(NO3)3 + AgCl
...
Al + FeO -> Al2O3 + Fe
...
Al + HCl -> AlCl3 + H2
...
Al + KOH + H2O -> KAlO2 + H2
...
Al + NH4ClO4 -> Al2O3 + AlCl3 + NO + H2O
...
Al + NaOH + H2O -> NaAl(OH)4 + H2
...
Al + O2 -> Al2O3
...
Al(NO3)3 + Na2CO3 -> Al2(CO3)3 + NaNO3
...
Al(OH)3 + H2SO4 -> Al2(SO4)3 + H2O
...
Be(OH)2 + NH4HF2 -> (NH4)2BeF4 + H2O
...
Bi(NO3)3 + H2S -> Bi2S3 + HNO3
...
C + SiO2 + Cl2 -> SiCl4 + CO
...
C10H16 + Cl2 -> C + HCl
...
C2H2 + O2 -> CO2 + H2O
...
C2H3Cl + O2 -> CO2 + H2O + HCl
...
C2H5OH + O2 -> CO + H2O
...
C2H5OH + O2 -> CO2 + H2O
...
C3H8 + O2 -> CO2 + H2O
...
C4H10 + O2 -> CO2 + H2O
...
C6H6 + O2 -> CO2 + H2O
...
Ca3(PO4)2 + SiO2 + C -> CaSiO3 + P4 + CO
...
Ca3(PO4)2 + SiO2 -> CaSiO3 + P2O5
...
Ca3(PO4)2 + SiO2 -> P4O10 + CaSiO3
...
Ca3P2 + H2O -> Ca(OH)2 + PH3
...
Ca5F(PO4)3 + H2SO4 -> Ca(H2PO4)2 + CaSO4 + HF
...
CaCN2 + H2O -> CaCO3 + NH3
...
CaHPO4⋅2H2O + NaOH + H2O -> Na2HPO4⋅12H2O + Ca(OH)2
...
CaS2 + O2 -> CaS2O3
...
Cr(OH)3 + H2SO4 -> Cr2(SO4)3 + H2O
...
Cu + CO2 + O2 + H2O -> CuCO3⋅Cu(OH)2
...
Fe + O2 -> Fe2O3
...
FeCl3 + Ca(OH)2 -> CaCl2 + Fe(OH)3
...
FeCl3 + NH4OH -> Fe(OH)3 + NH4Cl
...
FeO + H3PO4 -> Fe3(PO4)2 + H2O
...
FeS + O2 -> Fe2O3 + SO2
...
FeS2 + O2 -> Fe2O3 + SO2
...
FeSO4 + K3[Fe(CN)6] -> Fe3[Fe(CN)6]2 + K2SO4
...
H2S + Cl2 -> S8 + HCl
...
H2SO4 + Al(OH)3 -> Al2(SO4)3 + H2O
...
H2SO4 + HI -> H2S + I2 + H2O
...
H2SO4 + NaHCO3 -> Na2SO4 + CO2 + H2O
...
I2 + HNO3 -> HIO3 + NO2 + H2
...
K2CO3 + C + N2 -> KCN + CO
...
K2MnO4 + H2SO4 -> KMnO4 + MnO2 + K2SO4 + H2O
...
K3AsO4 + H2S -> As2S5 + KOH + H2O
...
KO2 + CO2 -> K2CO3 + O2
...
KOH + AlCl3 -> KCl + Al(OH)3
...
Mg3N2 + H2O -> Mg(OH)2 + NH3
...
MgNH4AsO4 + 6H2O -> Mg2As2O7 + NH3 + H2O
...
MgNH4PO4 -> Mg2P2O7 + NH3 + H2O
...
MnO2 + HCl -> MnCl2 + H2O + Cl2
...
Na3AsO3 + H2S -> As2S3 + NaOH
...
NaCl + H2SO4 -> Na2SO4 + HCl
...
NaOH + Cl2 -> NaCl + NaClO + H2O
...
NaOH + Zn(NO3)2 -> NaNO3 + Zn(OH)2
...
NiS + O2 -> NiO + SO2
...
P4 + H2O -> H3PO4 + H2
...
P4 + O2 -> P2O5
...
P4O10 + H2O -> H3PO4
...
P4O10 + HCl -> POCl3 + HPO3
...
P4O6 + H2O -> H3PO3
...
P4O6 -> P4 + P2O4
...
PCl3 + H2O -> H3PO3 + HCl
...
Si + S8 -> Si2S4
...
Si2H3 + O2 -> SiO2 + H2O
...
SiCl4 + H2O -> H4SiO4 + HCl
...
SiH4 + O2 -> SiO2 + H2O
...
SiO2 + HF -> SiF4 + H2O
...
Sn(OH)2 + NaOH -> Na2SnO2 + H2O
...
Sn(OH)4 + NaOH -> Na2SnO3 + H2O
...
TiCl4 + Mg -> MgCl2 + Ti
...
U3O8 + HNO3 -> UO2(NO3)2 + NO2 + H2O
...
(CuOH)₂CO₃ → CuO + CO₂ + H₂O
1 (CuOH)₂CO₃ → 2 CuO + 1 CO₂ + 1 H₂O
Al(OH)₃ + NaOH → NaAlO₂ + H₂O
1 Al(OH)₃ + 1 NaOH → 1 NaAlO₂ + 2 H₂O
CaCO₃ → CaO + CO₂
1 CaCO₃ → 1 CaO + 1 CO₂
CaC₂ + N₂ → CaCN₂ + C
1 CaC₂ + 1 N₂ → 1 CaCN₂ + 1 C
NaH₂PO₄ → NaPO₃ + H₂O
1 NaH₂PO₄ → 1 NaPO₃ + 1 H₂O
NaPO₃ + CuO → NaCuPO₄
1 NaPO₃ + 1 CuO → 1 NaCuPO₄
[Cr(N₂H₄CO)₆]₄[Cr(CN)₆]₃ + KMnO₄ + H₂SO₄ → K₂Cr₂O₇ + MnSO₄ + CO₂ + KNO₃ + K₂SO₄ + H₂O ***This is the mother of all chemical equations***
10 [Cr(N₂H₄CO)₆]₄[Cr(CN)₆]₃ + 1176 KMnO₄ + 1399 H₂SO₄ → 35K₂Cr₂O₇ + 1176 MnSO₄ + 420 CO₂ + 660 KNO₃ + 223 K₂SO₄ + 1879 H₂O
# of buffer systems crucial in maintaining human blood pH within a narrow range (pH 7.35-7.45)
2
CO + O₂ → CO₂
2 CO + 1 O₂ → 2 CO₂
ClO₂ + H₂O → HClO₂ + HClO₃
2 ClO₂ + 1 H₂O → 1 HClO₂ + 1 HClO₃
Cu(CN)₂ → CuCN + C₂N₂
2 Cu(CN)₂ → 2 CuCN + 1 C₂N₂
Al + HCl → AlCl₃ + H₂
2Al + 6HCl → 2AlCl₃ + 3H₂
Na₃PO₄ + CaCl₂ → NaCl + Ca₃(PO₄)₂
2Na₃PO₄ + 3CaCl₂ → 6NaCl + Ca₃(PO₄)₂
What are electrodes?
A graphite (inert) or metal strip that conducts electricity.
Any change in oxidation number of an atom indicates what?
A redox reaction has taken place
Slippery feel
Acid
Said that acids are hydrogen-containing compounds that ionize to yield hydrogen ions (H+) in aqueous solutions.
Arrhenius
Said that bases are compounds that ionize to yield hydroxide ions (OH-) in aqueous solution
Arrhenius
Three types of acids and bases: (hint: in alphabetical order)
Arrhenius, Bronsted-Lowry, Lewis
Why is alkali not measured using the burette
As alkali can damage glass wear
A 1-molar solution of which of the following salts has the highest pH? (A) NaNO3 (B) Na2CO3 (C) NH4Cl (D) NaHSO4 (E) Na2SO4
B
Nitric acid change
Brown gas produced
Iron(III) salts
Brown or orange
What colour precipitate does Fe3+ produce when tested?
Brown precipitate
Conjugate base of CH₃COOH
CH3COO-
Cn (-1 charge)
Cyanide
Acids that contain two ionizable hydrogens
Diprotic
Iron(III) salts
Fe3+
Negative ions
Form at the anode.
Alpha £
Glucagon
Glucagon=
Hormone
At the anode...
Ions lose electrons.
C2O4 (-2 charge)
Oxalate
The anode is the ........
Positive electrode
Anode
Positive electrode.
P₄ + O₂ → P₂O₃
P₄ + 3O₂ → 2P₂O₃
RIG
Reduction is gain of electrons
Ag (+1 charge)
Silver
Cortisol
Steroid hormone secreted by the adrenal glands in response to tissue damage
Sn (+2 charge)
Tin (II)
reversible reaction
a chemical reaction in which the products re-form the original reactants
name 2 metals less reactive than hydrogen
copper and silver
According to Lewis, a substance can accept or donate a pair of electrons to form a ____ bond
covalent
What forms at the cathode?
either a metal or hydrogen
Name the buffer system involving etha--
ethanoic acid-ethanoate ion
True or false: all salts are neutral
false
a method of balancing redox reactions by balancing the oxidation and reduction half-reactions
half-reaction method
Strong acids have ___ Ka values
large
If it is an oxidation, I will...
loose an electron
concentration formula
moles/volume
what is spread viral
mumps, rubella, chicken pox, polio
7
neutral
Acidified potassium manganate
purple to colourless
The solution of known concentration is called the
standard solution
___ acids are completely ionized in aqueous solutions
strong
Example of diprotic acid (name)
sulfuric acid
what are molten ionic compounds broken into
their elements (metal and non metal)
inert substance is ........
unreactive
Example of amphoteric substance (common name)
water
adrenal glands
(Suprarrenales) sit on top of kidneys
Neutralisation (1st acid equation)
- A reaction of an acid with a base, forming a salt and water - acid + alkali ---> salt + water - H+ + OH- ---> H2O - example: hydrochloric acid + sodium hydroxide --> sodium chloride + water
H in NaH
-1
Hydrogen's oxidation number?
1+ when combined with nonmetals 1- when combines with metals
1dm3 =
1000cm3
HAsO₂ → As₂O₃ + H₂O
2 HAsO₂ → 1 As₂O₃ + 1 H₂O
HAsO₃ → As₂O₅ + H₂O
2 HAsO₃ → 1 As₂O₅ + 1 H₂O
MgCl2 Oxidation Number
2+(2 x -1)=0
__NaOH + __CO₂ --> __Na₂CO₃ + __H₂O
2, 1, 1, 1
AgNO₃ + Cu → Cu(NO₃)₂ + Ag
2AgNO₃ + Cu → Cu(NO₃)₂ + 2Ag
HgO → Hg + O₂
2HgO → 2Hg + O₂
what is the half equation for the reaction at the positive electrode in the electrolysis of bauxite
2O²- ---> O² + 4e-
AgBr + GaPO₄ → Ag₃PO₄ + GaBr₃
3AgBr + GaPO₄ → Ag₃PO₄ + GaBr₃
How do we lose potential energy?
Because we do respiration in steps, every time we will lose energy. We lose the potential energy by losing heat in our bodies.
Be₂C + H₂O → Be(OH)₂ + CH₄
Be₂C + 2H₂O → 2Be(OH)₂ + CH₄
Conjugate acid of CH₃COO-
CH₃COOH
C₃H₈ + O₂ → CO₂ + H₂O
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
C₅H₁₂ + O₂ → CO₂ + H₂O
C₅H₁₂ + 8O₂ → 5CO₂ + 6H₂O
What two ions form when water dissociates?
H+ and OH-
oxidation number
Indicates the oxidation state of an element in its free state or in a compound
Beta B
Insulin
Hydrogen -1
NaH(+1,-1)
Formula for sodium hydroxide
NaOH
What colour precipitate does Fe2+ produce when tested?
Pale green precipitate
S + HNO₃ → H₂SO₄ + NO₂ + H₂O
S + 6HNO₃ → H₂SO₄ + 6NO₂ + 2H₂O
SO₂ + Li₂Se → SSe₂ + Li₂O
SO₂ + 2Li₂Se → SSe₂ + 2Li₂O
Pancreas
Sits behind the stomach, hormonal cells. Secretes hormones & glucagon
A pH of 0 is strongly
acidic
______ is a solution in which the pH remains relatively constant when small amounts of acid or base are added
buffer
calculating moles (2)
concentration x volume
H2PO4 (-1 charge)
dihydrogen phosphate
insertion= when over insertion can cause..
good in HF can cause petechiae
electron acceptor?
oxidizing agent
Cesium Oxidation Number
+1
Group 1 metals oxidation number in their compounds
+1
H in H20
+1
H in NH3
+1
K in K2SO4 oxi #
+1
Na in NaCl oxi #
+1
What is the unusual oxidation number of oxygen in a compound?
+1
Thallium oxi#s
+1,+3
Hydrogen in its compounds
+1,-1 in ionic hydrides
Beryllium oxidation number
+2
Ca in CaO
+2
Group II metals oxi#in their compounds
+2
Magnesium Oxidation Number!
+2
Mg in MgCl2
+2
Radium oxi #
+2
Scrontium oxi #
+2
Hg oxidation number
+2,+1
Actinium oxi#
+3
Aluminium oxi#
+3
Scandium oxidation number
+3
Cr oxidation number
+3, +6
C in NaHCO3
+4
SnCL4 (Sn)
+4
Silicon oxi#
+4,-4
(S) SO4 -2
+6
K2Cr2O7
+6
KMnO4.Mn oxidation
+7
Rule 4 for MnO4-
+7
Neutralisation of dilute acids with bases - metal carbonate (2nd acid equation)
- Acid + metal carbonate --> salt + water + carbon dioxide - 2HCL + Na2CO3 --> 2NaCl + H2O + CO2 hydrochloric acid + sodium carbonate --> Sodium chloride + water + carbon dioxide - H2SO4 + Cu2CO3 --> Cu2SO4 + H2O + CO2 sulfuric acid + copper carbonate ---> Copper sulphate + water + carbon dioxide
formula for copper sulfate crystals
- Copper carbonate + sulfuric acid ---> copper sulphate + water + carbon dioxide CuCO3 + H2SO4(aq) ---> CuSO4(aq) + H2O + CO2
Alkali composition
- Dissolve in water and split up forming hydroxide ions (ionise) - Strong alkalis fully ionise in water - Weak alkalis only partially ionise in water - Ammonia is an alkali (NH3)
Naming salts
- First part of name comes form the metal in the alkali base - Second part comes from the acid - NaOH + HCl ---> NaCl + H2O - Sodium hydroxide + hydrochloric acid --> sodium chloride + water
Neutralisation of strong acids and bases
- HCl + KOH ---> KCl + H2O hydrochloric acid + potassium hydroxide --> potassium chloride + water - H2SO4 + NaOH --> Na2SO4 + H2O sulfuric acid + sodium hydroxide --> sodium sulfate + water
Acid reactions with metals (4rd acid equation)
- acid + metal --> salt + hydrogen hydrochloric acid + magnesium --> magnesium chloride + hydrogen - cannot see salt produced as it has been dissolved in the acid observations with magnesium: effervescence - hydrogen gas produced quickly, reacts immediately with acid observation with zinc: slight fizzing, hydrogen gas rises towards the surface as more acid is added, slow reaction observations with iron: slow reaction with acid: tiny bubbles of hydrogen gas rising towards the surface of the acid (very small fizz), very slow reaction, observation: no reaction
Acid composition
- contains hydrogen ions - acids splits up to form a hydrogen ion and another ion in water (ionise). HCl (aq) ---> H+ (aq) + Cl- - Hydrogen ions gives acids their characteristics - Strong acids fully ionise in water to release H+ ions (hydrochloric acid, sulphuric acid, nitric acid). pH is usually from 0-2 - Weak acids (ethnic, critic, carbonic) only partially ionise to release H+ ions
Transition metals
- elements that form a bridge between elements on the left and right sides of the periodic table - high melting/boilng points - malleable - high density - good electrical + thermal conductivity - form coloured compounds - good catalysts
SnCl4 (Cl)
-1
Group VII element
-1in halides sometimes positive for Cl,Br and I
O in CO2
-2
O in Na2O
-2
Oxygen in its compounds
-2,except in peroxides and superoxides
The [H+] of a basic solution is less than 1 x 10^?M
-7
The [H+] of an acidic solution is greater than 1 x 10^? M
-7
(NH4)2Cr2O7 -> Cr2O3 + N2 + H2O
...
Al2(SO4)3 + Ca(OH)2 -> CaSO4 + Al(OH)3
...
Al2O3 + C + N2 -> AlN + CO
...
Al4C3 + H2O -> CH4 + Al(OH)3
...
AlCl3 + AgNO3 -> AgCl + Al(NO3)3
...
As + NaOH -> Na3AsO3 + H2
...
As2O5 + H2O -> H3AsO4
...
Au + HCl + HNO3 -> AuCl3 + NO + H2O
...
Au + KCN + O2 + H2O -> K[Au(CN)2] + KOH
...
Au2O3 -> Au + O2
...
Au2S3 + H2 -> Au + H2S
...
B2O3 + H2O -> H3BO3
...
BaCl2 + Al2(SO4)3 -> BaSO4 + AlCl3
...
C7H10N + O2 -> CO2 + H2O + NO2
...
C7H16 + O2 -> CO2 + H2O
...
C7H6O2 + O2 -> CO2 + H2O
...
CH4 + O2 -> CO2 +H2O
...
CO2 + H2O -> C6H12O6 + O2
...
Ca + AlCl3 -> CaCl2 + Al
...
Ca(NO3)2 -> CaO + NO2 + O2
...
Ca(OH)2 + P4O10 + H2O -> Ca(H2PO4)2
...
Ca10F2(PO4)6 + H2SO4 -> Ca(H2PO4)2 + CaSO4 + HF
...
Ca3(PO4)2 + C -> Ca3P2 + CO
...
Ca3(PO4)2 + H2SO4 -> CaSO4 + H3PO4
...
Ca3(PO4)2 + H3PO4 -> Ca(H2PO4)2
...
CuSO4 + KCN -> CuCN + K2SO4 + C2N2
...
Fe + H2O + O2 -> Fe2O3.H2O
...
Fe + H2O -> Fe3O4 + H2
...
Fe(OH)3 -> Fe2O3 + H2O
...
Fe2(SO4)3 + Ba(NO3)2 -> BaSO4 + Fe(NO3)3
...
Fe2(SO4)3 + KOH -> K2SO4 + Fe(OH)3
...
Fe2O3 + C -> CO + Fe
...
Fe2O3 + CO -> Fe + CO2
...
Fe2O3 + H2 -> Fe + H2O
...
Fe3O4 + H2 -> Fe + H2O
...
FeC2O4⋅2H2O + H2C2O4 + H2O2 + K2C2O4 -> K3[Fe(C2O4)3]⋅3H2O
...
H3AsO3 -> As2O3 + H2O
...
H3BO3 + Na2CO3 -> Na2B4O7 + CO2 + H2O
...
H3BO3 -> H4B6O11 + H2O
...
H3PO3 -> H3PO4 + PH3
...
H3PO4 + (NH4)2MoO4 + HNO3 -> (NH4)3PO4⋅2MoO3 + NH4NO3 + H2O
...
H3PO4 + Ca(OH)2 -> Ca(H2PO4)2 + H2O
...
H3PO4 + HCl -> PCl5 + H2O
...
HCl + HNO3 -> NOCl + Cl2 + H2O
...
HCl + K2CO3 -> KCl + H2O + CO2
...
HClO4 + P4O10 -> H3PO4 + Cl2O7
...
Hg(OH)2 + H3PO4 -> Hg3(PO4)2 + H2O
...
Hg2CrO4 -> Cr2O3 + Hg + O2
...
KBr + Al(ClO4)3 -> AlBr3 + KClO4
...
KClO3 -> KCl + O2
...
KClO3 -> KClO4 + KCl
...
KNO3 + C12H22O11 -> N2 + CO2 + H2O + K2CO3
...
MnO2 + KOH + O2 -> K2MnO4 + H2O
...
NH3 + NO -> N2 + H2O
...
NH3 + O2 -> HNO2 + H2O
...
NH3 + O2 -> NO + H2O
...
NH4Cl + Ca(OH)2 -> CaCl2 + NH3 + H2O
...
NH4VO3 -> V2O5 + NH3 + H2O
...
NO + NaOH -> NaNO2 + H2O + N2O
...
Na + H2O -> NaOH + H2
...
Na2B4O7 + HCl + H2O -> NaCl + H3BO3
...
Na2CO3 + HCl -> NaCl + H2O + CO2
...
Na2O2 + H2O -> NaOH + O2
...
Na2S2 + O2 -> Na2S2O3
...
Na2SnO3 + H2S -> SnS2 + NaOH + H2O
...
PCl5 + H2O -> H3PO4 + HCl
...
PCl5 + P2O5 -> POCl3
...
POCl3 + H2O -> H3PO4 + HCl
...
Pb + Na + C2H5Cl -> Pb(C2H5)4 + NaCl
...
Pb(NO3)2 -> PbO + NO2 + O2
...
Pb(OH)2 + NaOH -> Na2PbO2 + H2O
...
Pb3(VO4)2⋅PbCl2 + HCl -> VO2Cl + PbCl2 + H2O
...
Pb3O4 + HNO3 -> Pb(NO3)2 + PbO2 + H2O
...
S8 + O2 -> SO3
...
Sb + O2 -> Sb4O6
...
Se + NaOH -> Na2Se + Na2SeO3 + H2O
...
Si + NaOH + H2O -> Na2SiO3 + H2
...
UO2 + HF -> UF4 + H2O
...
UO2(NO3)2⋅6H2O -> UO3 + NO2 + O2 + H2O
...
V2O5 + Al -> Al2O3 + V
...
V2O5 + Ca -> CaO + V
...
V2O5 + HCl -> VOCl3 + H2O
...
VO2Cl + NH4OH -> NH4VO3 + NH4Cl + H2O
...
Zn + NaOH + H2O -> Na2Zn(OH)4 + H2
...
[Ag(NH3)2]Cl + HNO3 -> NH4NO3 + AgCl
...
Cl2 oxidation number
0
Na oxidation number
0
The pH scale ranges from __ to __
0, 14
(CN)₂ + NaOH → NaCN + NaOCN + H₂O
1 (CN)₂ + 2 NaOH → 1 NaCN + 1 NaOCN + 1 H₂O
(NH₄)₂SO₄ + CaCO₃ → (NH₄)₂CO₃ + CaSO₄
1 (NH₄)₂SO₄ + 1 CaCO₃ → 1 (NH₄)₂CO₃ + 1 CaSO₄
AgBr + Na₂S₂O₃ → Na₃[Ag(S₂O₃)₂] + NaBr
1 AgBr + 2 Na₂S₂O₃ → 1 Na₃[Ag(S₂O₃)₂] + 1 NaBr
AlN + H₂O → NH₃ + Al(OH)₃
1 AlN + 3 H₂O → 1 NH₃ + 1 Al(OH)₃
Al₂O₃ + Na₂CO₃ → NaAlO₂ + CO₂
1 Al₂O₃ + 1 Na₂CO₃ → 2 NaAlO₂ + 1 CO₂
As₂O₃ + H₂O → H₃AsO₃
1 As₂O₃ + 3 H₂O → 2 H₃AsO₃
BaCO₃ + HNO₃ → Ba(NO₃)₂ + CO₂ + H₂O
1 BaCO₃ + 2 HNO₃ → 1 Ba(NO₃)₂ + 1 CO₂ + 1 H₂O
BaO + H₂O → Ba(OH)₂
1 BaO + 1 H₂O → 1 Ba(OH)₂
BaO₂ + H₂SO₄ → BaSO₄ + H₂O₂
1 BaO₂ + 1 H₂SO₄ → 1 BaSO₄ + 1 H₂O₂
BaSO₂ + H₂SO₄ → Ba(HSO₄)₂
1 BaSO₂ + 1 H₂SO₄ → 1 Ba(HSO₄)₂
Be(OH)₂ → BeO + H₂O
1 Be(OH)₂ → 1 BeO + 1 H₂O
BeF₂ + Mg → MgF₂ + Be
1 BeF₂ + 1 Mg → 1 MgF₂ + 1 Be
BeO + C + Cl₂ → BeCl₂ + CO
1 BeO + 1 C + 1 Cl₂ → 1 BeCl₂ + 1 CO
BeSO₄ + NH₄OH → Be(OH)₂ + (NH₄)₂SO₄
1 BeSO₄ + 2 NH₄OH → 1 Be(OH)₂ + 1 (NH₄)₂SO₄
C + H₂O → CO + H₂
1 C + 1 H₂O → 1 CO + 1 H₂
CO₂ + NH₃ + H₂O → NH₄HCO₃
1 CO₂ + 1 NH₃ + H₂O → 1 NH₄HCO₃
CO₂ + NH₃ → OC(NH₂)₂ + H₂O
1 CO₂ + 2 NH₃ → 1 OC(NH₂)₂ + 1 H₂O
Ca(ClO₃)₂ → CaCl₂ + O₂
1 Ca(ClO₃)₂ → 1 CaCl₂ + 3 O₂
Ca(HCO₃)₂ → CaCO₃ + CO₂ + H₂O
1 Ca(HCO₃)₂ → 1 CaCO₃ + 1 CO₂ + 1 H₂O
Ca(OH)₂ + CO₂ → CaCO₃ + H₂O
1 Ca(OH)₂ + 1 CO₂ → 1 CaCO₃ + 1 H₂O
Ca(OH)₂ + H₃PO₄ → CaHPO₄ + H₂O
1 Ca(OH)₂ + 1 H₃PO₄ → 1 CaHPO₄ + 2 H₂O
Ca(OH)₂ + CO₂ → Ca(HCO₃)₂
1 Ca(OH)₂ + 2 CO₂ → 1 Ca(HCO₃)₂
CaCO₃ + HCl → CaCl₂ + H₂O + CO₂
1 CaCO₃ + 2 HCl → 1 CaCl₂ + 1 H₂O + 1 CO₂
CaC₂ + H₂O → C₂H₂ + Ca(OH)₂
1 CaC₂ + 2 H₂O → 1 C₂H₂ + 1 Ca(OH)₂
CaO + H₂O → Ca(OH)₂
1 CaO + 1 H₂O → 1 Ca(OH)₂
CaO + C → CaC₂ + CO
1 CaO + 3 C → 1 CaC₂ + 1 CO
CaS + H₂O → Ca(OH)₂ + H₂S
1 CaS + 2 H₂O → 1 Ca(OH)₂ + 1 H₂S
CaSO₄ → CaS + O₂
1 CaSO₄ → 1 CaS + 2 O₂
Ca₃(PO₄)₂ + H₂SO₄ → CaSO₄ + Ca(H₂PO₄)₂
1 Ca₃(PO₄)₂ + 2 H₂SO₄ → 2 CaSO₄ + 1 Ca(H₂PO₄)₂
CdSO₄ + H₂S → CdS + H₂SO₄
1 CdSO₄ + 1 H₂S → 1 CdS + 1 H₂SO₄
CuSO₄ + KCN → Cu(CN)₂ + K₂SO₄
1 CuSO₄ + 2 KCN → 1 Cu(CN)₂ + 1 K₂SO₄
FeS + H₂SO₄ → H₂S + FeSO₄
1 FeS + 1 H₂SO₄ → 1 H₂S + 1 FeSO₄
Fe₂O₃ + SiO₂ → Fe₂Si₂O₇
1 Fe₂O₃ + 2 SiO₂ → 1 Fe₂Si₂O₇
Hg₂CO₃ → Hg + HgO + CO₂
1 Hg₂CO₃ → 1 Hg + 1 HgO + 1 CO₂
H₂CO₃ → H₂O + CO₂
1 H₂CO₃ → 1 H₂O + 1 CO₂
H₂SO₃ → H₂O + SO₂
1 H₂SO₃ → 1 H₂O + 1 SO₂
H₃PO₄ + Ca(OH)₂ → CaHPO₄⋅2H₂O
1 H₃PO₄ + 1 Ca(OH)₂ → 1 CaHPO₄⋅2H₂O
H₄As₂O₇ → As₂O₅ + H₂O
1 H₄As₂O₇ → 1 As₂O₅ + 2 H₂O
K₂O + H₂O → KOH
1 K₂O + 1 H₂O → 2 KOH
Li₂O + H₂O → LiOH
1 Li₂O + 1 H₂O → 2 LiOH
MnO₂ + K₂CO₃ + KNO₃ → K₂MnO₄ + KNO₂ + CO₂
1 MnO₂ + 1 K₂CO₃ + 1 KNO₃ → 1 K₂MnO₄ + 1 KNO₂ + 1 CO₂
MnS + HCl → H₂S + MnCl₂
1 MnS + 2 HCl → 1 H₂S + 1 MnCl₂
Mn₂O₃ + Al → Al₂O₃ + Mn
1 Mn₂O₃ + 2 Al → 1 Al₂O₃ + 2 Mn
NH₃ + O₂ → HNO₃ + H₂O
1 NH₃ + 2 O₂ → 1 HNO₃ + 1 H₂O
NH₄NO₃ → N₂O + H₂O
1 NH₄NO₃ → 1 N₂O + 2 H₂O
NaCl + NH₄HCO₃ → NaHCO₃ + NH₄Cl
1 NaCl + 1 NH₄HCO₃ → 1 NaHCO₃ + 1 NH₄Cl
Na₂Cr₂O₇ + S → Cr₂O₃ + Na₂SO₄
1 Na₂Cr₂O₇ + 1 S → 1 Cr₂O₃ + 1 Na₂SO₄
Na₂O + H₂O → NaOH
1 Na₂O + 1 H₂O → 2 NaOH
Na₂SO₃ + S → Na₂S₂O₃
1 Na₂SO₃ + 1 S → 1 Na₂S₂O₃
N₂ + H₂ → NH₃
1 N₂ + 3 H₂ → 2 NH₃
N₂O₃ + H₂O → HNO₂
1 N₂O₃ + 1 H₂O → 2 HNO₂
N₂O₅ + H₂O → HNO₃
1 N₂O₅ + 1 H₂O → 2 HNO₃
PCl₅ + H₂O → POCl₃ + HCl
1 PCl₅ + 1 H₂O → 1 POCl₃ + 2 HCl
PCl₅ + KNO₂ → NOCl + POCl₃ + KCl
1 PCl₅ + 1 KNO₂ → 1 NOCl + 1 POCl₃ + 1 KCl
PbCrO₄ + HNO₃ → Pb(NO₃)₂ + H₂CrO₄
1 PbCrO₄ + 2 HNO₃ → 1 Pb(NO₃)₂ + 1 H₂CrO₄
SiO₂ + Ca(OH)₂ → CaSiO₃ + H₂O
1 SiO₂ + 1 Ca(OH)₂ → 1 CaSiO₃ + 1 H₂O
SiO₂ + Na₂CO₃ → Na₂SiO₃ + CO₂
1 SiO₂ + 1 Na₂CO₃ → 1 Na₂SiO₃ + 1 CO₂
SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + NH₄Br
1 SrBr₂ + 1 (NH₄)₂CO₃ → 1 SrCO₃ + 2 NH₄Br
UF₄ + Mg → MgF₂ + U
1 UF₄ + 2 Mg → 2 MgF₂ + 1 U
UO₃ + H₂ → UO₂ + H₂O
1 UO₃ + 1 H₂ → 1 UO₂ + 1 H₂O
Xe + F₂ → XeF₆
1 Xe + 3 F₂ → 1 XeF₆
Zn + HCl → ZnCl₂ + H₂
1 Zn + 2 HCl → 1 ZnCl₂ + 1 H₂
Zn + KOH → K₂ZnO₂ + H₂
1 Zn + 2 KOH → 1 K₂ZnO₂ + 1 H₂
Zn(OH)₂ + NaOH → Na₂ZnO₂ + H₂O
1 Zn(OH)₂ + 2 NaOH → 1 Na₂ZnO₂ + 2 H₂O
Method to make copper sulfate (crystals) with copper carbonate and sulfuric acid
1) Add copper carbonate and sulfuric acid to a beaker 2) Add copper carbonate (i.e 3 spatulas) until it stops reacting with the acid/stops releasing carbon dioxide (fizzing) - this will tell us when all the acid has been used CuCO3 + H2SO4 (aq)---> CuSO4 (aq) + H2O + CO2 3) Filter the reaction mixture using a funnel with filter paper inside to remove excess copper carbonate. Once the process is over, pure copper sulfate solution is left in the flask 4) Leave to evaporate by putting the copper chloride in an evaporating basin which is heated strongly by a Bunsen burner until half of the water has evaporated. Remaining water left to evaporate over a number of hours to form copper sulfate crystals
Give two examples of redox reactions
1) The burning of wood in a fireplace 2) The metabolization of food by your body
How to set up a titration
1) Use a pipette to transfer the sodium hydroxide (alkali + analyse) into a conical flask and record volume added 2) Add a few drops of indicator - this is to see the end point (point when the analyse has been neutralised) 3) Place the conical flask on a white file and the funnel in the burette - this ensures we can see a colour change clearly 4) Pour acid into the funnel through the burette and read off initial volume 5) Add acid in a trial run order to get a rough idea what volume is required 6) In the first run, add acid until a colour change is observed. then add the acid drip by drip. This important as to not overshoot the end-point 7) The end volume is then read off 8) Swirl the mixture during the titration as this allows both solutions to properly dissolve 9) Repeat the process until similar (concordant) volumes are obtained. Any anomalies are excluded from calculating the mean value 10) This is a type of neutralisation reaction DISCLAIMER: when forming crystals with titration, only use indicator to calculate titre of a solution. then use the titre to neutralise the acid and alkali WITHOUT the indicator
__BaCl₂ + __Na₂SO₄ --> __NaCl + __BaSO₄
1, 1, 2, 1
__Cu + __HCl --> __CuCl₂ + __H₂
1, 2, 1, 1
__Mg + __HCl --> __MgCl₂ + __H₂
1, 2, 1, 1
__Mg + __HF --> __MgF₂ + __H₂
1, 2, 1, 1
__Sn + __HF --> __SnF₂ + __H₂
1, 2, 1, 1
__CS₂ + __O₂ --> __CO₂ + __SO₂
1, 3, 1, 2
__Al₂(SO₄)₃ + __Ca(OH)₂ --> __Al(OH)₃ + __CaSO₄
1, 3, 2, 3
Fluorine's oxidation number?
1-
how is aluminium extracted from the ore bauxite (whole process)
1. electrolysis 2. aluminium oxide has a very high melting point so it's mixed with cryolite to lower the melting point. 3. the molten mixture contains free ions so it'll conduct electricity 4. the positive Al3+ ions are attracted to the negative electrode where they each pick up three electrons and turn into neutral aluminium atoms. These then sink down to the bottom of the electrolysis tank 5. the negative O2- ions are attracted to the positive electrode where they each lose two electrons. The neutral oxygen atoms will then combine to form O² molecules
For aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals =
1.0 x 10⁻¹⁴
How does the ecosystem use photosynthesis to make energy?
1.Plants take C02 in atmosphere and water through roots, uses light energy to convert it into organic molecule such as glucose. Then it releases O2 (waste product) 2. The next process is cellular respiration .. it takes the organic molecules such as carbon, hydrogen, oxygen bonded together, r groups and proteins--it takes the energy stored in these carbon hydrogen bonds/ the molecules and combines it with 02 and then breaks it all back down.
HIO₃ → I₂O₅ + H₂O
2 HIO₃ → 1 I₂O₅ + 1 H₂O
HNO₂ + O₂ → HNO₃
2 HNO₂ + 1 O₂ → 2 HNO₃
HNO₃ + P₂O₅ → N₂O₅ + HPO₃
2 HNO₃ + 1 P₂O₅ → 1 N₂O₅ + 2 HPO₃
HgO → Hg + O₂
2 HgO → 2 Hg + 1 O₂
H₂ + O₂ → H₂O
2 H₂ + 1 O₂ → 2 H₂O
H₂O₂ → H₂O + O₂
2 H₂O₂ → 2 H₂O + 1 O₂
H₃AsO₄ → As₂O₅ + H₂O
2 H₃AsO₄ → 1 As₂O₅ + 3 H₂O
H₃PO₄ → H₄P₂O₇ + H₂O
2 H₃PO₄ → 1 H₄P₂O₇ + 1 H₂O
K + Br₂ → KBr
2 K + 1 Br₂ → 2 KBr
KHSO₄ → K₂S₂O₇ + H₂O
2 KHSO₄ → 1 K₂S₂O₇ + 1 H₂O
Mg(OH)₂ → (MgOH)₂O + H₂O
2 Mg(OH)₂ → 1 (MgOH)₂O + 1 H₂O
NaHCO₃ → Na₂CO₃ + CO₂ + H₂O
2 NaHCO₃ → 1 Na₂CO₃ + 1 CO₂ + 1 H₂O
NaOH + FeSO₄ → Na₂SO₄ + Fe(OH)₂
2 NaOH + 1 FeSO₄ → 1 Na₂SO₄ + 1 Fe(OH)₂
Na₂HPO₄ → Na₄P₂O₇ + H₂O
2 Na₂HPO₄ → 1 Na₄P₂O₇ + 1 H₂O
N₂ + O₂ → N₂O
2 N₂ + 1 O₂ → 2 N₂O
__CO + __O₂ --> __CO₂
2, 1, 2
__H₂ + __O₂ -->__H₂O
2, 1, 2
__K + __I₂ --> __KI
2, 1, 2
__Mg + __O₂ --> __MgO
2, 1, 2
__Na + __F₂ --> __NaF
2, 1, 2
__SO₂ + __O₂ --> __SO₃
2, 1, 2
__LiCl + __Mg(NO₃)₂ --> __LiNO₃ + __MgCl₂
2, 1, 2, 1
__Na + __MgF₂ --> __NaF + __Mg
2, 1, 2, 1
__K + __H₂O --> __KOH + __H₂
2, 2, 2, 1
__Al + __Cl₂ --> __AlCl₃
2, 3, 2
__MgS + __O₂ --> __MgO + __SO₂
2, 3, 2, 2
__Al + __Cu(NO₃)₂ --> __Cu + __Al(NO₃)₃
2, 3, 3, 2
Oxygen's oxidation number?
2- in most compounds and ions 1- in peroxides 2+ when combined with F
Ag₂O → Ag + O₂
2Ag₂O → 4Ag + O₂
Al + H₂SO₄ → Al₂(SO₄)₃ + H₂
2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂
AlBr₃ + K₂SO₄ → KBr + Al₂(SO₄)₃
2AlBr₃ + 3K₂SO₄ → 6KBr + Al₂(SO₄)₃
CuFeS₂ + O₂ → Cu + FeO + SO₂
2CuFeS₂ + 5O₂ → 2Cu + 2FeO + 4SO₂
C₂H₂N₂O₄ + O₂ → CO₂ + H₂O + N₂
2C₂H₂N₂O₄ + O₂ → 4CO₂ + 2H₂O + 2N₂
C₂₁H₃₀O₂ + O₂ → CO₂ + H₂O
2C₂₁H₃₀O₂ + 55O₂ → 42CO₂ + 30H₂O
C₃H₈O + F₂ → CF₄ + HF + O₂
2C₃H₈O + 20F₂ → 6CF₄ + 16HF + O₂
C₄H₁₀ + O₂ → CO₂ + H₂O
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O
C₆H₆ + O₂ → CO₂ + H₂O
2C₆H₆ + 9O₂ → 12CO₂ + 6H₂O
C₇H₅N₃O₆ → N₂ + H₂O + CO + C
2C₇H₅N₃O₆ → 3N₂ + 5H₂O + 7CO + 7C
C₈H₁₈ + O₂ → CO₂ + H₂O
2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O
Fe₂O₃ + C → Fe + CO₂
2Fe₂O₃ + 3C → 4Fe + 3CO₂
what is the half equation for the reduction of hydrogen
2H+ + 2e‐ ----> H²
HCN + CuSO₄ → H₂SO₄ + Cu(CN)₂
2HCN + CuSO₄ → H₂SO₄ + Cu(CN)₂
HCl + CaCO₃ → CaCl₂ + H₂O + CO₂
2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂
H₂ + O₂ → H₂O
2H₂ + O₂ → 2H₂O
H₂O + O₂ → H₂O₂
2H₂O + O₂ → 2H₂O₂
H₂S + SO₂ → S + H₂O
2H₂S + SO₂ → 3S + 2H₂O
K + Cl₂ →KCl
2K + Cl₂ →2KCl
KClO → KCl + O₂
2KClO → 2KCl + O₂
KClO₃ → KCl + O₂
2KClO₃ → 2KCl + 3O₂
LiHCO₃ + H₂SO₄ → Li₂SO₄ + H₂O + CO₂
2LiHCO₃ + H₂SO₄ → Li₂SO₄ + 2H₂O + 2CO₂
NH₃ + CuO → Cu + N₂ + H₂O
2NH₃ + 3CuO → 3Cu + N₂ + 3H₂O
NH₃ + H₂SO₄ → (NH₄)₂SO₄
2NH₃ + H₂SO₄ → (NH₄)₂SO₄
Na + H₂O → NaOH + H₂
2Na + 2H₂O → 2NaOH + H₂
NaBr + CaF₂ → NaF + CaBr₂
2NaBr + CaF₂ → 2NaF + CaBr₂
NaBr + Cl₂ → Br₂ + NaCl
2NaBr + Cl₂ → Br₂ + 2NaCl
NaCl + F₂ → NaF + Cl₂
2NaCl + F₂ → 2NaF + Cl₂
NaF + Br₂ → NaBr + F₂
2NaF + Br₂ → 2NaBr + F₂
NaHCO₃ + H₂SO₄ → CO₂ + Na₂SO₄ + H₂O
2NaHCO₃ + H₂SO₄ → 2CO₂ + Na₂SO₄ + 2H₂O
NaHCO₃ → Na₂CO₃ + CO₂ + H₂O
2NaHCO₃ → Na₂CO₃ + CO₂ + H₂O
NaNO₃ + PbO → Pb(NO₃)₂ + Na₂O
2NaNO₃ + PbO → Pb(NO₃)₂ + Na₂O
RbNO₃ + BeF₂ → Be(NO₃)₂ + RbF
2RbNO₃ + BeF₂ → Be(NO₃)₂ + 2RbF
The information below describes a redox reaction. Ag+(aq)+Al(s)--->Ag(s)+Al3+(aq) Ag+(aq)+e---->Ag(s) Al(s)-->Al3+(aq)+3e- What is the coefficient of silver in the final, balanced equation for this reaction?
3
Mg + N₂ → Mg₃N₂
3 Mg + 1 N₂ → 1 Mg₃N₂
O₂ → O₃
3 O₂ → 2 O₃
Aluminum's oxidation number
3+
__Mg + __AlCl₃ --> __MgCl₂ +__Al
3, 2, 3, 2
AgNO₃ + FeCl₃ → Fe(NO₃)₃ + AgCl
3AgNO₃ + FeCl₃ → Fe(NO₃)₃ + 3AgCl
Cu + HNO₃ → Cu(NO₃)₂ + NO + H₂O
3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 2NO + 4H₂O
Fe₂O₃ + CO → Fe₃O₄ + CO₂
3Fe₂O₃ + CO → 2Fe₃O₄ + CO₂
Hg(OH)₂ + H₃PO₄ → Hg₃(PO₄)₂ + H₂O
3Hg(OH)₂ + 2H₃PO₄ → Hg₃(PO₄)₂ + 6H₂O
H₂SO₄ + B(OH)₃ → B₂(SO₄)₃ + H₂O
3H₂SO₄ + 2B(OH)₃ → B₂(SO₄)₃ + 6H₂O
MgO + H₃PO₄ → Mg₃(PO₄)₂ + H₂O
3MgO + 2H₃PO₄ → Mg₃(PO₄)₂ + 3H₂O
NH₄OH + H₃PO₄ → (NH₄)₃PO₄ + H₂O
3NH₄OH + H₃PO₄ → (NH₄)₃PO₄ + 3H₂O
__Al + __O₂ --> __Al₂O₃
4, 3, 2
__Fe +__O₂ --> __Fe₂O₃
4, 3, 2
Al + O₂ → Al₂O₃
4Al + 3O₂ → 2Al₂O₃
Al₂O₃ + Fe → Fe₃O₄ + Al
4Al₂O₃ + 9Fe → 3Fe₃O₄ + 8Al
Fe + O₂ →Fe₂O₃
4Fe + 3O₂ →2Fe₂O₃
what is the oxidation half equation for oxygen forming from hydroxide ions
4OH‐ ---> O² + 2H²O + 4e‐
P + O₂ → P₂O₅
4P + 5O₂ → 2P₂O₅
how long does it take tweezed hair to regrow
5-6 weeks
CO + I₂O₅ → CO₂ + I₂
5CO + I₂O₅ → 5CO₂ + I₂
virgin growth is hair that has not been touched in
6-8 months
AgI + Fe₂(CO₃)₃ → FeI₃ + Ag₂CO₃
6AgI + Fe₂(CO₃)₃ → 2FeI₃ + 3Ag₂CO₃
K + B₂O₃ → K₂O + B
6K + B₂O₃ → 3K₂O + 2B
A neutral solution has a pOH of
7
Acidic solutions have a pH lower than
7
Neutral solutions have a pH of
7
Actinium (Ac)
89
angle of inclination, hair doesnt exist at
90 or 0 degrees
55. The equilibrium constant for the reaction represented by the equation below is greater than 1.0. Which of the following gives the correct relative strengths of the acids and bases in the reaction? H2PO4− + HBO32− ⇄ HPO42− + H2BO3− Acids Bases A.H2PO4− > H2BO3− and HBO32− > HPO42− B.H2BO3− > H2PO4− and HBO32¯ > HPO42− C.H2PO4− > H2BO3− and HPO42− > HBO32− D.H2BO3− > H2PO4− and HPO42− > HBO32− E.H2PO4− = H2BO3− and HPO42− = HBO32−
A
A solution of calcium hypochlorite, a common additive to swimming-pool water, is... (A) basic because of the hydrolysis of the OCl− ion (B) basic because Ca(OH)2 is a weak and insoluble base (C) neutral if the concentration is kept below 0.1 molar (D) acidic because of the hydrolysis of the Ca2+ ions (E) acidic because the acid HOCl is formed
A
HC2H3O2(aq) + CN− (aq) ⇄ HCN(aq) + C2H3O2− (aq) The reaction represented above has an equilibrium constant equal to 3.7 x 104. Which of the following can be concluded from this information? (A) CN− (aq) is a stronger base than C2H3O2− (aq) (B) HCN(aq) is a stronger acid than HC2H3O2(aq) (C) The conjugate base of CN− (aq) is C2H3O2− (aq) (D) The equilibrium constant will increase with an increase in temperature. (E) The pH of a solution containing equimolar amounts of CN− (aq) and HC2H3O2 (aq) is 7.0
A
Questions 9-12 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of substances. Assume all concentrations are 1 M. (A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 11. A buffer at a pH > 8
A
The net ionic equation for the reaction between silver carbonate and hydrochloric acid is... (A) Ag2CO3(s) + 2 H+ + 2 Cl− 2 AgCl(s) + H2O + CO2 (g) (B) 2 Ag+ + CO32− + 2 H+ + 2 Cl− 2 AgCl(s) + H2O + CO2(g) (C) CO32− + 2 H+ H2O + CO2(g) (D) Ag+ + Cl¯ AgCl(s) (E) Ag2CO3(s) + 2 H+ 2Ag+ + H2CO3
A
Use these answers for questions 8 - 10. (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10−5 NH3 = 1.8 x 10−5 H2CO3; K1 = 4 x 10−7 H2CO3; K2 = 4 x 10−11 8. A solution prepared to be initially 1 M in NaCl and 1 M in HCl.
A
What part of the curve corresponds to the optimum buffer action for the acetic acid/acetate pair? (A) Point V (B) Point X (C) Point Z (D) Along all of section WY (E) along all of section YZ
A
Alkali
A base that dissolves in water to form a solution with a pH greater than 7
Brine is electrolysed in...
A diaphragm cell.
Define a conductor?
A material that allows heat and electricity to pass through it.
Define an insulator?
A material that does not allow heat or electrons to move through it easily.
what is an electrolyte
A molten or dissolved ionic compound that conducts electricity
An anion is ..........
A negatively charged ion
A cation is ........
A positively charged ion
In an ecosystem that uses photosynthesis, O2 release is considered what?
A waste product
Why does the breakdown of glucose not turn into ATP
ADP and phosphate is in the cell. When we break apart the glucose, the energy that is released is used to fuel the reaction of taking ADP and attaching the phosphate back to it. This is why we say it regenerates Breaking down of glucose down not turn into ATP. IT is the energy of breaking down glucose that fuels the reaction that turns ADP back into ATP.
What is ADP? what is the Pi in the ADP+Pi
ADP is adenosine diphosphate. Pi is inorganic phosphate
C2H3O2 (-1 charge)
Acetate
Can be strong or weak electrolytes in aqueous solution
Acid
React with metals to produce hydrogen gas
Acid
Tastes sour
Acid
Used as preservative (foods)
Acid
Used in fragrances and flavors
Acid
Ka is what constant? _____ ___________
Acid dissociation
What is ATP?
Adenosine triphosphate It has 3 phosphate molecule
How to insert needle
Always insert needle on the underside of the hair, parallel to the hair, under the hair, size of the hair=size of needle. Never parallel or perpendicular
what is the half equation for the reaction at the negative electrode during the electrolysis of bauxite
Al³+ + 3e- ---> Al
Al₂(SO₃)₃ + NaOH → Na₂SO₃ + Al(OH)₃
Al₂(SO₃)₃ + 6NaOH → 3Na₂SO₃ + 2Al(OH)₃
Al₄C₃ + H₂O → CH₄ + Al(OH)₃
Al₄C₃ + 12H₂O → 3CH₄ + 4Al(OH)₃
NH4 (+1 charge)
Ammonium
what is an aqueous solution
An aqueous solution is a solution in which the solvent is water.
what happens during electrolysis
An electric current is passed through an electrolyte which causes the ions to move towards the electrodes where they react and the ions get discharged
What is electroplating?
An electrolytic process in which metal ions are reduced and the metal atoms are deposited on a surface
NAD+ wants to accept electrons, right now it's acting as
An electron acceptor. This means its in a state of oxidize.. When NAD picks up hydrogens and electrons, it becomes reduced..
Salt
An ionic compound made from the neutralization of an acid with a base.
acid
Any substance that forms an aqueous solution with a pH less than 7
Rule 6 for oxidation number
Atoms in a polyatomic ion is the sum of the oxidisation numbers
54. Which of the following is the correct equilibrium expression for the hydrolysis of CO32− ? (A) K = [HCO3− ] / ( [CO32− ] [H3O+] ) (B) K = ( [HCO3−] [OH−] ) / [CO32−] (C) K = ( [CO32− ] [OH−] ) / [HCO3−] (D) K = [CO32− ] / ( [CO2] [OH−]2 ) (E) K = ( [CO32− ] [H3O+] ) / [HCO3−]
B
8. Use these answers for questions 8 - 10. (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10−5 NH3 = 1.8 x 10−5 H2CO3; K1 = 4 x 10−7 H2CO3; K2 = 4 x 10−11 10. A solution prepared to be initially 0.5 M in CH3COOH and 1 M in CH3COONa
B
A molecule or an ion is classified as a Lewis acid if it... (A) accepts a proton from water (B) accepts a pair of electrons to form a bond (C) donates a pair of electrons to form a bond (D) donates a proton to water (E) has resonance Lewis electron-dot structures
B
A pure white crystalline solid dissolves in water to yield a basic solution that liberates a gas when excess acid is added to it. On the basis of this information, the solid could be... (A) KNO3 (B) K2CO3 (C) KOH (D) KHSO4 (E) KCl
B
At 25°C, aqueous solutions with a pH of 8 have a hydroxide ion concentration, [OH−], of... (A) 1 × 10−14 M (B) 1 × 10−8 M (C) 1 × 10−6 M (D) 1M (E) 8M
B
Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar, 32.0 milliliters of 0.500-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present? (A) 1.60 M (B) 0.800 M (C) 0.640 M (D) 0.600 M (E) 0.400 M
B
Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion a solution in largest concentration, other than the K+ ion, is... (A) H2PO4− (B) HPO42− (C) PO43− (D) OH− (E) H3O+
B
Mixtures that would be considered buffers include which of the following? I. 0.10 M HCl + 0.10 M NaCl II. 0.10 M HF + 0.10 M NaF III. 0.10 M HBr + 0.10 M NaBr (A) I only (B) II only (C) III only (D) I and II (E) II and III
B
Questions 9-12 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of substances. Assume all concentrations are 1 M. (A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 12. A buffer at a pH <6
B
When dilute nitric acid was added to a solution of one of the following chemicals, a gas was evolved, This gas turned a drop of limewater, Ca(OH)2, cloudy, due to the formation of a white precipitate. The chemical was... (A) household ammonia, NH3 (B) baking soda, NaHCO3 (C) table salt, NaCl (D) epsom salts, MgSO4 . 7H2O (E) bleach, 5% NaOCl
B
When phenolphthalein is used as the indicator in a titration of an HCl solution with a solution of NaOH, the indicator undergoes a color change from clear to red at the end point of the titration. This color change occurs abruptly because... (A) phenolphthalein is a very strong acid that is capable of rapid dissociation (B) the solution being titrated undergoes a large pH change near the end point of the titration (C) phenolphthalein undergoes an irreversible reaction in basic solution (D) OH− acts as a catalyst for the decomposition of phenolphthalein (E) phenolphthalein is involved in the rate-determining step of the reaction between H3O+ and OH−
B
Which of these is not crucial to human blood? (A) Ammonium ion-ammonia, (B) ethanoic acid-ethanoate ion, (C) Dihydrogen phosphate-monohydrogen phosphate
B
Which, if any, of the following species is in the greatest concentration in a 0.100-molar solution of H2SO4 in water? (A) H2SO4 molecules (B) H3O+ ions (C) HSO4− ions (D) SO42− ions (E) All species are in equilibrium and therefore have the same concentrations.
B
Why does cellular respiration not oxidize glucose in a single step?
B/c there is a Stepwise Energy Harvest via NAD+ and the Electron Transport Chain -- it requires a metabolic pathway. it must be harvested slowly and in steps, not all at once
BaS + PtF₂ → BaF₂ + PtS
BaS + PtF₂ → BaF₂ + PtS
According to Bronsted-Lowry, is ammonia a base or acid?
Base
Cleaning agents, antacids
Base
Example: milk of magnesia
Base
React with acids
Base
Used as antacids (neutralization reaction)
Base
Used in chemical reactions (making polymers, drugs, etc)
Base
Used in making soaps, detergents, etc
Base
Why would the electrons be attracted to the oxygen?
Because Oxygen is highly electronegative .. it's pulling the electrons down the electron chain
What is respiration?
Biological organisms burn fuel sources inside their cells in order to release energy to do the work of running the biochemical reactions that keep them alive The basic oxidation reaction is : C6H12O6 + 6O2-> 6CO2 + 6H2O
Changes the color of an acid-base indicator (acid, base, or both)
Both
Who defines a base as a hydrogen-ion acceptor
Bronsted-Lowry
Who defines an acid as a hydrogen-ion donor
Bronsted-Lowry
2 NH3 ⇄ NH4+ + NH2− In liquid ammonia, the reaction represented above occurs. In the reaction NH4+ acts as... (A) a catalyst (B) both an acid and a base (C) the conjugate acid of NH3 (D) the reducing agent (E) the oxidizing agent
C
Correct procedures for a titration include which of the following? I. Draining a pipet by touching the tip to the side of the container used for the titration II. Rinsing the buret with distilled water just before filling it with the liquid to be titrated III. Swirling the solution frequently during the titration (A) I only (B) II only (C) I and III only (D) II and III only (E) I, II, and III
C
How can 100. mL of sodium hydroxide solution with a pH of 13.00 be converted to a sodium hydroxide solution with a pH of 12.00? (A) By diluting the solution with distilled water to a total volume of 108 mL (B) By diluting the solution with distilled water to a total volume of 200 mL (C) By diluting the solution with distilled water to a total volume of 1.00 L (D) By adding 100. mL of 0.10 M HCl (E) By adding 100. mL of 0.10 M NaOH
C
In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment? (A) The pH is 7 at the equivalence point. (B) The pH at the equivalence point depends on the indicator used. (C) The graph of pH versus volume of base added rises gradually at first and then much more rapidly. (D) The graph of pH versus volume of base added shows no sharp rise. (E) The [H+] at the equivalence point equals the ionization constant of the acid.
C
To determine the molar mass of a solid monoprotic acid, a student titrated a weighed sample of the acid with standardized aqueous NaOH. Which of the following could explain why the student obtained a molar mass that was too large? I. Failure to rinse all acid from the weighing paper into the titration vessel II. Addition of more water than was needed to dissolve the acid III. Addition of some base beyond the equivalence point (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III
C
What volume of 0.150-molar HCl is required to neutralize 25.0 milliliters of 0.120-molar Ba(OH)2? (A) 20.0 mL (B) 30 0 mL (C) 40.0 mL (D) 60.0 mL (E) 80.0 mL
C
cellular respiration with the oxidation of sugar glucose:
C6H12O6 + 6O2 --> 6CO2 + 6H2O + Energy (ATP + heat) sugar glucose + oxygen --> break down to carbon dioxide + water + Energy such as ATP + heat is produce Another explanation: When glucose is oxidized, carbon dioxide, water and energy are produced. The food that is consumed by most organisms is basically glucose. The other carbohydrates consumed are ultimately reduced to glucose during digestion. Glucose acts as a fuel and a source of energy for the organism's activities. The energy in glucose is released during respiration. During respiration, the oxygen taken in is used to oxidise glucose. The glucose molecule is broken down to produce carbon dioxide and water. This process releases a lot of energy. This energy is used in formation of ATP molecules. These ATP molecules thus become storehouses of energy. The numbers in the equation represent the proportions in which the ingredients react and the proportion in which the products are formed. It is clear that, to oxidize every molecule of glucose, you need 6 molecules of oxygen. After the process is complete, you are left with 6 moles of CO2 and 6 moles of water along with some energy.
cellular respiration vs. photosynthesis
C6H12O6 + 6O2 --> 6CO2 + 6H2O + Energy (ATP + heat) vs. 6CO2 + 6H2O + light energy ---> C6H12O6 + 6O2
CF₄ + Br₂ → CBr₄ + F₂
CF₄ + 2Br₂ → CBr₄ + 2F₂
example of weak acidic compounds ionising
CH₃COOH ⇌ CH₃COO- + H+
CH₄ + O₂ → CO₂ + H₂O
CH₄ + 2O₂ → CO₂ + 2H₂O
CO₂ → C + O₂
CO₂ → C + O₂
Ca + H₂O → Ca(OH)₂ + H₂
Ca + 2H₂O → Ca(OH)₂ + H₂
Ca(NO₃)₂ + Na₂CO₃ → CaCO₃ + NaNO₃
Ca(NO₃)₂ + Na₂CO₃ → CaCO₃ + 2NaNO₃
Formula for Calcium hydroxide
Ca(OH)₂
Ca(OH)₂ + HCl → CaCl₂ + H₂O
Ca(OH)₂ + 2HCl → CaCl₂ + 2H₂O
CaCO₃ + HNO₃ → Ca(NO₃)₂ + H₂O + CO₂
CaCO₃ + 2HNO₃ → Ca(NO₃)₂ + H₂O + CO₂
2 factors of acne
Can blood supply perform any rehealing, or will pathogenic bacteria spread
CO3 (-2 charge)
Carbonate
Electric current
Causes a chemical reaction that breaks down the ionic compound.
Ca₃(PO₄)₂ + H₂SO₄ → CaSO₄ + Ca(H₂PO₄)₂
Ca₃(PO₄)₂ + 2 H₂SO₄ → 2 CaSO₄ + Ca(H₂PO₄)₂
Ca₃(PO₄)₂ + SiO₂ + C → CaSiO₃ + CO + P
Ca₃(PO₄)₂ + 3SiO₂ + 5C → 3CaSiO₃ + 5CO + 2P
FSH
Changed testosterone to estrogen
LA
Changes testosterone to progesterone
What is the redox reaction, aka Oxidation and Reduction reaction?
Chemical reactions that transfer electrons between reactants The transfer of electrons during chemical reactions releases energy stored in organic molecules
ClO3 (-1 charge)
Chlorate
The conjugate base of the acid HCl (what ion?)
Chloride ion
Electrolysis of brine produces...
Chlorine, hydrogen, sodium hydroxide.
ClO2 (-1 charge)
Chlorite
CrO4 (-2 charge)
Chromate
Cr (+3 charge)
Chromium (III)
Conjugate base of HCl (formula)
Cl-
Co (+3 charge)
Cobalt (III)
Archard-theirs syndrome
Combination of cushings and virilism disease. Woman who have beards
Brine
Concentrated aqueous solution of sodium chloride, obtained from seams of rock salt underground.
what is brine
Concentrated sodium chloride solution
Difference between strength of an acid and concentration
Concentration = the measure of how much acid there is in a litre (1dm3) of water Strength = the proportion of the acid molecules ionised in water
Vocabulary: The particle formed when a base gains a hydrogen ion
Conjugate acid
Consists of two substances related by the loss or gain of a single hydrogen ion.
Conjugate acid-base pair
The particle that remains when an acid has donated a hydrogen ion
Conjugate base
Cu (+1 charge)
Copper (I) Cuprous
Cu (+2 charge)
Copper (II) Cupric
Consider the half reaction below. Cu2+(aq)+2e--->Cu(s) Which statement best describes what is taking place?
Copper is being reduced.
How does iron corrode?
Corrodes by being oxidized to ions of iron by oxygen.
Which half-reaction correctly describes an oxidation?
Cr(s)-->Cr3+(aq)+3e-
Why is a mixture of aluminium oxide and cryolite used, rather than aluminium oxide alone?
Cryolite lowers the melting point and reduces some of the energy costs involved in extracting aluminium oxide.
Cr₂(SO₄)₃ + NaOH → Cr(OH)₃ + Na₂SO₄
Cr₂(SO₄)₃ + 6NaOH → 2Cr(OH)₃ + 3Na₂SO₄
C₂H₄O₂ + O₂ → CO₂ + H₂O
C₂H₄O₂ + 2O₂ → 2CO₂ + 2H₂O
C₆H₁₂O₆ + O₂ → CO₂ + H₂O
C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O
C₆H₆ → C + H₂
C₆H₆ → 6C + 3H₂
C₉H₂₀ + O₂ → CO₂ + H₂O
C₉H₂₀ + 14O₂ → 9CO₂ + 10H₂O
49. Each of the following can act as both a Brönsted acid and a Brönsted base EXCEPT... (A) HCO3− (B) H2PO4− (C) NH4+ (D) H2O (E) HS−
D
Acid Acid Dissociation Constant, Ka H3PO4 7 x 10−3 H2PO4− 8 x 10−8 HPO42− 5 x 10−13 On the basis of the information above, a buffer with a pH = 9 can best be made by using... (A) pure NaH2PO4 (B) H3PO4 + H2PO4− (C) H2PO4− + PO43− (D) H2PO4− + HPO42− (E) HPO42− + PO43−
D
The graph below shows the titration curve that results when 100. mL of 0.0250 M acetic acid is titrated with 0.100 M NaOH. Which of the following indicators is the best choice for this titration? pH Range of Color Change (A) Methyl orange 3.2 - 4.4 (B) Methyl red 4.8 - 6.0 (C) Bromthymol blue 6.1 - 7.6 (D) Phenolphthalein 8.2 - 10.0
D
The pH of 0.1-molar ammonia is approximately... (A) 1 (B) 4 (C) 7 (D) 11 (E) 14
D
The safest and most effective emergency procedure to treat an acid splash on skin is to do which of the following immediately? (A) Dry the affected area with paper towels (B) Sprinkle the affected area with powdered Na2SO4(s) (C) Flush the affected area with water and then with a dilute NaOH solution (D) Flush the affected area with water and then with a dilute NaHCO3 solution (E) Flush the affected area with water and then with a dilute vinegar solution
D
Use these answers for questions 8 - 10. (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10−5 NH3 = 1.8 x 10−5 H2CO3; K1 = 4 x 10−7 H2CO3; K2 = 4 x 10−11 9. A solution prepared to be initially 1 M in Na2CO3 and 1 M in CH3COONa
D
What is the H+(aq) concentration in 0.05 M HCN(aq) ? (The Ka for HCN is 5.0 x 10−10) (A) 2.5 x 10−11 (B) 2.5 x 10−10 (C) 5.0 x 10−10 (D) 5.0 x 10−6 (E) 5.0 x 10−4
D
What is the pH of a 1.0 x 10−2-molar solution of HCN? (Ka = 4.0 x 10 −10 ) (A) 10 (B) Between 7 and 10 (C) 7 (D) Between 4 and 7 (E) 4
D
Insulin
Decreases sugar in the blood
Cr2O7 (-2 charge)
Dichromate
Drugs that caused hair growth
Dilatin, loestrin, minoxidil, prednisone, Premarin
Reducing agent
Donates electrons and becomes oxidized.
What happens when an electron continuously gets passed between oxidation agents and reducing agents?
During each pass, it will lose energy. Eventually, the electrons will have no energy/use left
. Which of the following ions is the strongest Lewis acid? (A) Na+ (B) Cl− (C) CH3COO− (D) Mg2+ (E) Al3+
E
22. HSO4− + H2O ⇄ H3O+ + SO42− In the equilibrium represented above, the species that act as bases include which of the following? I. HSO4− II. H2O III. SO42− (A) II only (B) III only (C) I and II (D) I and III (E) II and III
E
As the number of oxygen atoms increases in any series of oxygen acids, such as HXO, HXO2, HXO3, ...., which of the following is generally true? (A) The acid strength varies unpredictably. (B) The acid strength decreases only if X is a nonmetal. (C) The acid strength decreases only if X is a metal. (D) The acid strength decreases whether X is a nonmetal or a metal. (E) The acid strength increases.
E
Ascorbic acid H2C6H6O6(s), is a diprotic acid with K1 = 7.9 × 10−5 and K2 = 1.6 × 10−12. In a 0.005 M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration? (A) H2O(l) (B) H3O+(aq) (C) H2C6H6O6(aq) (D) HC6H6O6−(aq) (E) C6H6O62−(aq)
E
If the acid dissociation constant, Ka, for an acid HA is 8 x 10−4 at 25 °C, what percent of the acid is dissociated in a 0.50-molar solution of HA at 25 °C? (A) 0.08% (B) 0.2% (C) 1% (D) 2% (E) 4%
E
Questions 9-12 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of substances. Assume all concentrations are 1 M. (A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 10. The most nearly neutral solution
E
The net ionic equation for the reaction that occurs during the titration of nitrous acid with sodium hydroxide is... (A) HNO2 + Na+ + OH− NaNO2 + H2O (B) HNO2 + NaOH Na+ + NO2− + H2O (C) H+ + OH− H2O (D) HNO2 + H2O NO2− + H3O+ (E) HNO2 + OH− NO2− + H2O
E
Which of the following acids can be oxidized to form a stronger acid? (A) H3PO4 (B) HNO3 (C) H2CO3 (D) H3BO3 (E) H2SO3
E
Which of the following reactions does NOT proceed significantly to the right in aqueous solutions? (A) H3O+ + OH− 2 H2O (B) HCN + OH− H2O + CN− (C) Cu(H2O)42+ + 4 NH3 Cu(NH3)42+ + 4H2O (D) H2SO4 + H2O H3O+ + HSO4− (E) H2O + HSO4− H2SO4 + OH−
E
Cushing syndrome
Enlarged face, muscle weakness. is caused from *to much cortisol
Oxidation of number of a monatomic ion is...?
Equal to the charge of the ion
The sum of the individual oxidation numbers of all atoms in the formula for a polyatomic ion is...?
Equal to the charge of the ion
During cellular respiration, the fuel (such as glucose) is oxidized and oxygen is reduced:
Every time we pull off a hydrogen, the sugar glucose becomes oxidize ..
Pre treatment and post Electrolysis
FDA 70% alcohol, minimum 30% alcohol= antiseptic
True or False Not all oxidation reactions are accompanied by reduction reactions
False
True or False: All compounds that contain hydrogen are acids
False
True or False The presence of salts and acids halts the process of corrosion.
False, the presence of salts and acids speed of the process of corrosion.
True or False The oxidation numbers of elements in a compound are not written per atom.
False, they are written per atom.
FeCl₃ + NaOH → Fe(OH)₃ + NaCl
FeCl₃ + 3NaOH → Fe(OH)₃ + 3NaCl
Fe₂(C₂O₄)₃ → FeC₂O₄ + CO₂
Fe₂(C₂O₄)₃ → 2 FeC₂O₄ + 2 CO₂
Fe₂O₃ + H₂ → Fe + H₂O
Fe₂O₃ + 3H₂ → 2Fe + 3H₂O
Fe₂O₃ + H₂O → Fe(OH)₃
Fe₂O₃ + 3H₂O → 2Fe(OH)₃
The process of photosynthesis
First you would need energy. Not ATP but energy from the sun..Then it needs water and C02 to release oxygen and make some glucose or other organic molecules 6CO2 + 6H2O + light energy >>> C6H12O6 + 6O2
Positive ions
Form at the cathode.
Diabetes symptoms
Frequent thirst; polydipsia, fragile blood vessels=bruising, HBP, cardio problems, obesity, neuropathy
GaF₃ + Cs → CsF + Ga
GaF₃ + 3Cs → 3CsF + Ga
Define reduction?
Gain of electrons
Glycogen is broken into?
Glucose
what happens at the cathode during the electrolysis of a solution
H+ ions and metal ions are present - hydrogen gas will be produced if the metal is more reactive than hydrogen, a layer of pure metal will be produced if the metal is less reactive than hydrogen
Oxygen -1
H2O2
Conjugate acid of HSO₄⁻
H2SO4
Sulfuric Acid
H2SO4 (Strong Acid)
what virus in the Heps family can survive in dry blood for 7 days
HBV
Gastric acid is also known as
HCl
Example of monoprotic acids (formula)
HNO3
HNO₃ + NaHCO₃ → NaNO₃ + H₂O + CO₂
HNO₃ + NaHCO₃ → NaNO₃ + H₂O + CO₂
Conjugate base of H₂SO₄
HSO₄⁻
HAV
Hepatitis A: most innocent of heps family
HSO3 (-1 charge)
Hydrogen Sulfite
OH (-1 charge)
Hydroxide
ClO (-1 charge)
Hypochlorite
Conjugate acid of OH-
H₂O
H₂SO₃ → H₂O + SO₂
H₂SO₃ → H₂O + SO₂
Example of diprotic acid (formula)
H₂SO₄
H₂SO₄ + NaNO₂ → HNO₂ + Na₂SO₄
H₂SO₄ + 2NaNO₂ → 2HNO₂ + Na₂SO₄
example of strong acidic compounds ionising
H₂SO₄ ---> 2H+ (aq) + SO₄2- - sulfuric acid --> hydrogen + sulphate
Example of triprotic acids (formula)
H₃PO₄
H₃PO₄ + KOH → K₃PO₄ + H₂O
H₃PO₄ + 3KOH → K₃PO₄ + 3H₂O
Why do we have to do the tumble and go through the ETC? Why don't we want to do a combustion reaction (explosive reaction) or do everything in one giant step?
If we did one giant step, we would release all of the heat/light energy at once. That would cause us to explode.
Explain why oxidation cannot occur without reduction, and vice versa.
In a redox reaction one element has a complete or partial loss of electrons (oxidation) therefore another element must have a complete or partial gain of electrons (reduction).
Diabetes type 1
Insulin dependent, childhood onset, not producing enough insulin
Half-equations
Ionic equations that only show what is happening at only one of the electrodes.
Why do ionic compounds only conduct when molten or aqueous?
Ions are fixed when ionic compounds are solid, meaning they can't move so can't conduct electricity. When the compounds are molten or in aqueous solution, the ions (that are electrically charged) are able to move and carry charge.
Fe (+2 charge)
Iron (II) Ferrous
Fe (+3 charge)
Iron (III) Ferric
Consider the half reaction below. Fe--->Fe2+ +2e- Which statement best describes what is taking place in this half reaction?
Iron is being oxidized.
Hydrogen
Is +1 except in hydrides where it is -1
Oxygen
Is -2 except in peroxdes where it is -1
How does temperature affect an enzyme?
It affects the shape and rate at which an enzyme will react
What happens when ATP release energy/loses its 3 phosphate group?
It becomes ADP ATP + H2O--> ADP + Pi ATP goes through hydrolysis by breaking bonds using water.. it turns to ADP. ADP is adenosine diphosphate. Pi is inorganic phosphate
Which statement is true of the following reaction? H2+O2-->2H+ +O2-
It is not balanced for charge or for number of atoms.
What is the final electron acceptor?
It is oxygen. Oxygen's only role is to be the final acceptor of electrons that is being passed by NADH
Oxidation number of nitrogen is 0 in
Its free state of N2
K + MgBr → KBr + Mg
K + MgBr → KBr + Mg
potassium dichromate
K2Cr2O7. A strong oxidizing agent.
Formula for potassium hydroxide
KOH
Acid dissociation constant
Ka
Base dissociation constant
Kb
Give 2 uses for chlorine
Kills harmful bacteria in swimming pools To sterelise the domestic water supply To manafacture PVC
The ion-product constant for water
Kw
Pb (+2 charge)
Lead (II)
Pb (+4 charge)
Lead (IV)
To which electrodes do the lead and bromide ions go during the electrolysis of PbBr2
Lead is positively charged and moves to the negative electrode (cathode). Bromine is negatively charged and move to the positive electrode (anode).
Hypopigmentation
Less melanocytes = white
Who proposed an base donates a pair of electrons during a reaction?
Lewis
Who proposed that an acid accepts a pair of electrons during a reaction?
Lewis
Overview:
Living cells require energy from outside sources •Some animals, such as the giant panda, obtain energy by eating plants; others feed on organisms that eat plants •Energy flows into an ecosystem as sunlight and leaves as heat •Photosynthesis generates oxygen and organic molecules, which are used in cellular respiration •Cells use chemical energy stored in organic molecules to regenerate ATP, which powers work
Define oxidation?
Loss of electrons
Dilute acid
Lots of water, small amount of acid
Hg2 (+2 charge)
Mercury (I) Mercurous
Hg (+2 charge)
Mercury (II) Mercuric
Formula for Magnesium hydroxide
Mg(OH)₂
Magnesium Oxide Oxidation Number
Mg:+2,O:-2
MgF₂ + Li₂CO₃ → MgCO₃ + LiF
MgF₂ + Li₂CO₃ → MgCO₃ + 2LiF
Mg₃N₂ + H₂O → NH₃ + Mg(OH)₂
Mg₃N₂ + 6H₂O → 2NH₃ + 3Mg(OH)₂
Mn(NO₂)₂ + BeCl₂ → Be(NO₂)₂ + MnCl₂
Mn(NO₂)₂ + BeCl₂ → Be(NO₂)₂ + MnCl₂
calculating moles (1)
Moles = mass/Mr
Acids that contain one ionizable hydrogen
Monoprotic
Hyper-pigmentation
More active melanocytes= brown
Addison's disease
Muscle weakness, low bp, hyperpigment on face and arms, *not enough cortisol
The role of NAD in cellular respiration
NAD is a co-enzyme.. this means its going to be continuously reused and help carry out another reaction in cellular respiration NAD is going to carry electrons from the glucose molecule to use them in a different type of reaction
When NAD accepts electron and changes from an oxidize to reduce state, it beomes
NADH
What is NADH?
NADH is NAD's reduced form because it is now carrying the hydrogens and electrons
An electron transport chain...
NADH passes the electrons to the electron transport chain. Electron transport chain passes electrons in a series of steps.. Each time the electrons get transferred it is LOOSING energy.
Reversible reaction - alkaline
NH3 + H2O ⇌ NH4+ + OH-
Conjugate base of NH₄⁺
NH₃
NH₄NO₃ → N₂O + H₂O
NH₄NO₃ → N₂O + 2H₂O
Sodium chloride oxidation number
Na:+1,Cl=-1
examples of alkaline compounds ionising
NaOH(aq) --> Na+(aq) + OH-
Na₃PO₄ + KOH → NaOH + K₃PO₄
Na₃PO₄ + 3KOH → 3NaOH + K₃PO₄
The cathode is the .......
Negative electrode
Cathode
Negative electrode.
Anions
Negative ions.
What is NAD called?
Nicotinamide
NO3 (-1 charge)
Nitrate
NO2 (-1 charge)
Nitrite
When we harvest energy out of a molecule, are we using all of the molecule's energy?
No, because we are very inefficient at it. We do not use all of the energy to make ATP, we release some in the form of heat
Are double-replacement reactions redox reactions?
No, never.
Does ADP have a high energy bond?
No. It was broken off and used during its transformation of ATP to ADP.
Diabetes type 2
Non insulin dependent, adulthood, *insulin resistant patients
N₂ + H₂ → NH₃
N₂ + 3H₂ → 2NH₃
Acronym that helps us understand redox reaction...
O.I.L.R.I.G Oil - oxidation I loose [electrons, or other elements caring electrons] Rig - reduction I gain [electrons, or other elements carrying electrons]
Conjugate base of H₂O
OH-
Acidified potassium dichromate colour change
Orange to green
PCOS = Polycystic ovarian syndrome
Ovaries contain cysts
Oxidation or Reduction Shift of electrons away from an atom in a covalent bond (Increase in oxidation number)
Oxidation
Loss of electrons from an atom or ion Gain of oxygen Example?
Oxidation Burning
OIL
Oxidation is loss of electrons
OILRIG
Oxidation is loss, Reduction is gain.
Rule 2 for oxidation number
Oxidation number of elements that exist as simple ions in ionic compounds is the same as the charge on the ion
Does oxidation occur at the anode or cathode?
Oxidation occurs at the anode. Oxidation is the loss of electrons.
Rule 1 for oxidation numbers
Oxidation state of atoms of an element in its free state is zero
What is oxygen's role?
Oxygen pulls electrons down the chain in an energy-yielding tumble .. Oxygen is used at the very END •The energy yielded is used to regenerate ATP
Pb(OH)₂ + HCl → H₂O + PbCl₂
Pb(OH)₂ + 2HCl → 2H₂O + PbCl₂
ClO4 (-1 charge)
Perchlorate
MnO4 (-1 charge)
Permanganate
O2 (-2 charge)
Peroxide
PO4 (-3 charge)
Phosphate
3 types of visible scars
Pitted scars, Dermal contraction, keloid
what is the test for chlorine
Placing a piece of damp litmus paper into a test tube containing a gas and seeing if it turns from blue to white
Cations
Positive ions.
what is the anode
Positively charged electrode where oxidation takes place
reactivity series
Potassium Sodium Lithium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Hydrogen Copper Silver Gold
KMnO4
Potassium permanganate
what is the test for hydrogen
Put a lit splint where the gas is and if there's a squeaky pop, hydrogen is present.
what is the test for oxygen
Putting a glowing splint into a test tube containing a gas and if it relights oxygen is present
P₄O₁₀ + H₂O → H₃PO₄
P₄O₁₀ + 6H₂O → 4H₃PO₄
Pseudofolliculitis barbe
Razor bumps, Ingrown hairs
Reduction
Reaction with gain of electrons.
Oxidation
Reaction with loss of electrons.
oxidizing agent
Reduced
Gain of electrons by atoms or ions Loss of oxygen
Reduction
Oxidation or Reduction Shift of electrons toward an atom in a covalent bond (Gain of hydrogen)
Reduction
Does reduction occur at the anode or cathode?
Reduction occurs at the cathode. Reduction is the gain of electrons.
Delta A
Regulates the activity of £ & B
Electrodes
Rods that carry electric current to and from the electrolyte.
Why during the extraction of aluminium from aluminium oxide, do the anodes need to be replaced during ?
Since the positive electrodes are made of carbon they get corroded by the oxygen forming carbon dioxide and so must be replaced every few weeks
Concentrated acid
Small amount of water, lots of acid
Are acid-base reactions redox reactions?
Sometimes, they can be.
Are single-replacement reactions redox reactions?
Sometimes, they can be.
Ex redox reaction
Start out with a molecule name josh. he has some electrons that he's going to give to tran.. he just lost an electron and became *oxidized tran gained an electron so she became *reduced This situation allowed them to transfer energy by transferring electrons.. some energy did get lost in the transfer could be used in the cells to do other reactions now tran is going to give the electrons to daisy.. she became oxidized and daisy just got electrons so she just became reduced.. once again, in the transfer.. energy was lost so the energy could be used to do some type of work such as generate ATP or heat
If a substance gains electrons readily it is known as a...?
Strong oxidizing agent
Glycogen
Sugar stored in the muscle & liver converted to glucose (source of energy)
SO4 (-2 charge)
Sulfate
S₈ + O₂ → SO₃
S₈ + 12O₂ → 8SO₃
How do you turn ADP back to ATP?
Take the energy released in the reactions, from the electrons in the Redox reaction to use its molecules and reattach phosphate back into ADP and turn it back into ATP.. use the same energy that was broken off and through cellular respiration, turn it back into ATP The process of cellular respiration
What does cell respiration mean?
The cell is exchanging gases. It takes in oxygen from air and release C02 To do cellular respiration, we are going to oxidize glucose, break off all of the hydrogen and use it to generate ATP
Electrolyte
The compound that conducts electricity when molten and breaks down during electrolysis.
In compounds, the oxidation number corresponds with what?
The element's position in the periodic table.
Why can molten ionic compounds be electrolysed?
The ions can move freely and conduct electricity
What is phosphorylation
The process of adding phosphate back onto ADP to turn it into ATP
What is electrolysis?
The process of splitting up a chemical compound into its elements by the passage of an electric current.
Rule 4 for oxidation number
The sum of all the oxidation numbers of the elememts in a radical is equal to the charge on the ion
Rule 3 for oxidation number
The sum of all the oxidation numbers of the elements in a compound is zero
Our body heat that we generate on a daily basis ultimately comes from?
The sun
Titration
The use of volume measurements to solve for concentrations, often of unknown substances.
Sn (+4 charge)
Tin (IV)
SnCl4
Tin (IV) Chloride
Acids that contain three ionizable hydrogens
Triprotic
True or False Oxidation reactions are the principal source of energy on Earth
True
True or False Some atoms have several possible oxidation numbers.
True
Inert conductor
Unreactive conductor that won't interfere with the electrolysis.
Give 2 uses for sodium hydroxide
Used to make soap Manufacture bleach (with chlorine)
How much NAD we have at one time?
Very limited amount. because it is a co enzyme, it needs to get regenerated. While a NADH is carrying a hydrogen, it cannot pick up another one. It needs to get rid of it to restart the process
smallest living organisms, contains dna structures and requires a target host for reproduction
Virus
V₂O₅ + CaS → CaO + V₂S₅
V₂O₅ + 5CaS → 5CaO + V₂S₅
Why do we have to harvest energy in a metabolic pathway
We cannot produce it because our bodies would have to go through a combustion reaction.. we are unable to do that because it would make us burn up. We have to harvest our energy instead in a metabolic pathway
Why are humans called an aerobic organism instead of an anrobic organism?
We need oxygen to do metabolic pathway Anrobic can do the pathway without the need of oxygen
how are aqueous solutions formed
When solutes are dissolved in the solvent water
How does ATP release energy?
When the third phosphate group of ATP is removed by hydrolysis, a substantial amount of free energy is released.
When do we use ADP vs ATP?
When we don't need as much energy for a reaction
Iron(III) salts colour change
Yellow to pale green
Is the corrosion of metal a redox reaction?
Yes
Can ADP be used as an energy molecule?
Yes. you can break off the next phosphate and turn it into AMP Adenosine monophosphate
What happens when NADH pass the electron through electron transport chain?
You started out as NADH because you were reduced, once you passed the electron to another you became NAD again (oxidized)
The sum of individual oxidation numbers of all the atoms in a formula must equal...?
Zero
Zn + HCl → ZnCl₂ + H₂
Zn + 2 HCl → ZnCl₂ + H₂
Consider the half reactions below for a chemical reaction. Zn--->Zn2+(aq)+2e- Cu2+(aq)+2e---->Cu(s) What is the overall equation for this chemical reaction?
Zn(s)+Cu2+(aq)--->Zn2+(aq)+Cu(s)
Consider the redox reaction below. Zn(s)+2HCl(aq)--->ZnCl2(aq)+H2(g) Which half reaction correctly describes the oxidation that is taking place?
Zn(s)---->Zn2+(aq)+2e-
ZnSO₄ + Li₂CO₃ → ZnCO₃ + Li₂SO₄
ZnSO₄ + Li₂CO₃ → ZnCO₃ + Li₂SO₄
Oxidizing agents
[organic redox] agents that have high affinity for electrons (O2, O3, Cl2) or unusually high electron states (Mn7+, Cr6+)
nitrogen dioxide
a highly poisonous brown gas (NO2)
what forms at the anode
a non metal other than hydrogen
The molecule that functions as the reducing agent in a redox reaction will...
a reducing agent is the donor (oxidation i lose --giving electrons away).. this makes it loses electrons and loses potential energy
titrant
a solution of known concentration and volume
analyte/titrand
a substance that has a known volume but an unknown concentration
In cellular respiration, the C02 carbon dioxide released is considered what?
a waste we exhale
According to Bronsted-Lowry, a base is an H+ _____
acceptor
According to Lewis, an acid is an electron-pair_____
acceptor
According to Lewis, an acid (accepts/donates) a pair of electrons during a reaction
accepts
A solution with a pOH >7
acidic
Below 7
acidic
Strong acid + Weak base = _________ solution
acidic
Type of solution in which [H+] is greater than [OH-]
acidic
2 stages of bacteria life..
active phase: vegetable, reproductive, and dormant phase: non vegetable, non-reproductive
how to calculate the titre
add the values of the volume of acid added to the burette (excluding the rough volume) and divide by the number of readings taken
Basic solutions are also known as ______ solutions
alkaline
Over 7
alkaline
This acid is associated with protein
amino acid
Name the buffer system involving amm-
ammonium ion-ammonia
A substance can act as both an acid and a base is said to be ___________
amphoteric
NAD is
an electron acceptor or electron carrier As we're stripping the electrons off the molecules such as glucose, NAD is going to carry it
The process in which you take the CO2+H20 and used its energy to build organic molecules is what type of process?
anabolic (taking smaller molecules, used some energy to build larger molecules)
A salt consists of an ____ of an acid and a ____ of a base
anion, cation
which electrode does oxidation take place
anode
in electrolysis which direction do the electrons travel
anode ➔ cathode
where is the reading taken
at the bottom of the meniscus
__C + __O₂ --> __CO₂
balanced
__CaO + __H₂O --> __Ca(OH)₂
balanced
__Cu +__Cl₂ --> __CuCl₂
balanced
A solution with a pOH < 7
basic
Type of solution in which [H+] is less than [OH-]
basic
Weak acid + Strong base = ________ solution
basic
Why do anodes need to be replaced regularly?
because they are made of graphite (carbon) and this reacts with the oxygen to produces carbon dioxide
What are the high energy bonds in ATP
bond between the second and third (last bond) phosphates is commonly described as a "high-energy" bond and is depicted in the figure by a wavy red line
The amount of acid or base that can be added to a puffer solution before a significant change in pH occurs
buffer capacity
How do Catabolic pathways yield energy?
by oxidizing (combined chemically with oxygen) organic fuels .. "catabolic pathways yield energy by oxidizing organic fuels" because transferring electrons from an organic molecule to an oxygen molecule is commonly termed "oxidizing" process is catabolic/destructive and yields storage energy
Name the buffer system involving ca--
carbonic acid-hydrogen carbonate ion
The process of cellular respiration is what type of process?
catabolic process .. takes the large organic molecules and some oxygen.. breaks them down to release energy and waste products
which electrode does reduction take place
cathode
Cellular respiration is what type of process? Photosynthesis is what type of process?
cellular respiration is the catabolic process photosynthesis is the anabolic process
electrolysis of calcium chloride is performed: what is formed at the anode
chlorine
what are the 4 ions that are present in a copper sulphate solution
copper ions, sulphate ions, hydrogen ions and hydroxide ions
what would happen during the electrolysis of copper sulphate solution
copper will be produced at the cathode and oxygen will be produced at the anode from the hydroxide ions (seen by bubbling)
Some redox reactions do not transfer electrons but change the electron sharing in
covalent bonds. An example is the reaction between methane and O2
things that affect treatment
dermatitis/ eczema, cold sores, moles, or anything raised dont treat
Which is an important step in the alternate method for balancing equations in redox reactions?
determining the half reactions of chemical equations
Name the buffer system involving dihy--
dihydrogen phosphate ion-hydrogenphosphate ion,
what is spread through bacteria
dipheria and typhoid
According to Lewis, an base (accepts/donates) a pair of electrons during a reaction
donates
According to Bronsted-Lowry, an acid is an H⁺______
donor
According to Lewis, a base is an electron pair _______
donor
In cellular respiration, we are transferring?
electron-- which is energy
When we are harvesting energy out of a molecule, we are pulling apart that molecule's?
electrons (electrons hold energy therefore when you're harvesting energy, you're pulling apart the electrons)
The point of neutralization is the _____ point of the titration
end
The point at which the indicator changes color is the ______ _______ of the titration
end point
The moving of an electron from oxidation to reduction is transferring..
energy. This released energy is ultimately used to synthesize ATP
When an acid and base are mixed, the ____________ _________ is when the number of moles of hydrogen ions equals the number of moles of hydroxide ions
equivalence point
The break down of organic molecules is?
exergonic, this means that energy is being released
If it is a reduction, I will..
gain an electron (negative charge) and reducing the positive charges
Reduction
gain of electrons
reduction
gain of electrons
Which of the following statements describes the results of this reaction? C6H12O6 (Glucose) + 6O2 --> 6CO2 + 6 H2O + Energy
glucose is oxidized and oxygen is reduced When glucose is oxidized, carbon dioxide, water and energy are produced.
why are electrodes made from graphite (3)
graphite is insoluble in water, has high melting and boiling points and can conduct electricity
In a respiration reaction, what are the 2 key components?
he oxidation of glucose. this means glucose (sugar) is combined with oxygen to produce carbon dioxide, water and energy
Viral infection is
herps= cold sores, flat warts
Basic solutions have a pH ____ than
higher
shallow insertion causes
higher % of over treatment, HF blow out and % of re growth increases
HCO3 (-1 charge)
hydrogen carbonate (bicarbonate)
HPO4 (-2 charge)
hydrogen phosphate
HSO4 (-1 charge)
hydrogen sulfate (bisulfate)
When we break down glucose to get its energy.. we essentially want its?
hydrogens
Aside of carry electrons, NAD will also carry?
hydrogens .. ex: in glucose C6H12O6 .. NAD can carry 12 H
A water molecule that gains a hydrogen ion becomes a positively charged _________
hydronium ion
Conjugate acid of the base water (what ion?)
hydronium ion
A base is a source of ______________ ions
hydroxide
The number of moles of hydrogen ions provided by an acid are equivalent to the number of _________ ions provided by the base
hydroxide
Equations can be balanced by using the half-reaction method. Which step should be completed immediately after finding the oxidation states of atoms?
identifying the half reactions
what happens at the anode during the electrolysis of solutions
if OH‐ ions and halide ions are present, molecules of chlorine, bromine or iodine form if no halide ions are present the hydroxide ions are discharged and oxygen will be formed
A valuable tool for measuring pH because its acid form and base have different colors in solution
indicator
An acid or a base that undergoes dissociation in a known pH range
indicator
The product of the concentrations of the hydrogen ions and hydroxide ions in water is called the (long name)
ion-product constant for water
Acids are classified as strong or weak depending on the degree to which they ___ in water
ionize
what ions are present in an aqueous solution
ions from the ionic compound, hydrogen ions and hydroxide ions
ionise
ions in a compound split up when in water
electrometallic phenomenon
is a chemical injury belongs to blend and galvanic electrolysis
bacteria: prokaryoctic
is a single celled, vegetable in nature, grow by the thousands to form a mass called a colony
What can the energy that is lost during a redox reaction be used as ?
it can be used in the cell to do other reaction such as generate ATP, or as heat
what is a disadvantage of using electrolysis to extract a metal from its ore
it's expensive as lots of energy is required to heat the ionic compound
During electrolysis what do you understand by the term 'discharge'?
lose its charge, become neutral
Oxidation
loss of electrons
why is cryolite used in the electrolysis of aluminium oxide
lower melting point
bacterial: Non-pathogenic
majority, useful, helpful, necessary
pH scale
measurement system used to indicate the concentration of hydrogen ions (H+) and hydroxide ions in a solution; ranging from 0 to 14
Define molten?
melted by heat
Neutralisation of dilute acids with bases - metal oxide (3rd acid equation)
metal oxide + acid --> metal salt + water CuO + H2SO4 --> CuSO4 + H2O
For precise and continuous measurements, what sort of device would you use to measure the pH of a substance?
meter
bacteria: pathogenic
minority, 100% disease, harmful
concentration of solution units
mol/dm-3
what happens to the negative ions during electrolysis and where does it happen
move towards the anode and lose electrons so they are oxidized
what does MSS stand for
muscular skeletal symptoms
An electron donor, otherwise known as the reducing agent is giving away..
negative (electrons) if he is giving someone a negative, he is reducing them.. this makes him the reducing agent
What type of salt produces a basic solution? One that contains ________ ____ _____ _______ ____________ _____ __________
negative ions that attract protons from water
Salts that produce basic solutions contain (negative/positive) ions that attract (neutrons, protons, electrons)
negative, protons
In a reduction, you are gaining an electron.. this actually means you are gaining..
negativity.. Why? because electrons are negatively charged.. In a negative charge, it reduces a positively charged molecule. *You are gaining an electron that reduces positive charged molecules.
Strong acid + Strong base = ______ solution
neutral
Any aqueous solution in which [H+] and [OH-] are equal is described as a _______ ________
neutral solution
You can determine the concentration of acid (or base) in a solution by performing a __________________ reaction
neutralization
Reactions in which an acid and a base react in an aqueous solution to produce a salt and water are called
neutralization reactions
Nitric acid forms
nitrate salts
Example of monoprotic acid (name)
nitric acid
Does plants produce more than one organic molecule?
no- it can produce glucose, lipids, proteins, oils
In cellular respiration, does glucose get turned into ATP?
no. energy stored in glucose is used to REGENERATE ATP.. glucose does not turn into atp, we only use the energy to turn it into ATP
Type of acid in DNA and RNA
nucleic acid
the complete or partial loss of electrons or the gain of oxygen
oxidation
a positive or negative number assigned to an atom according to a set of arbitrary rules
oxidation number
the balancing of a redox reaction by comparing the increases and decreases in oxidation numbers
oxidation-number-change method
the chemical changes that occur when electrons are transferred between reactants
oxidation-reduction reactions
substance in a redox reaction that gains electrons Contains the atoms that are reduced
oxidizing agent
NAD+ functions as an_____during cellular respiration.
oxidizing agent, also an electron acceptor
The electron acceptor in a redox reaction is called the ____________? During the course of the reaction it becomes ____________.
oxidizing agent; reduced
Cellular respiration consumes___ and yields ____
oxygen and organic molecules ATP
-log[H+] =
pH
The __ of a solution is the negative logarithm of the hydrogen-ion concentration
pH
-log[OH-] = ___
pOH
The ____ of a solution equals the negative logarithm of the hydroxide-ion concentration
pOH
____ = 14 - pH
pOH
pH = 14 - ___
pOH
Example of triprotic acid (name)
phosphoric acid
What is the opposite of a respiration?
photosynthesis-- the reverse process of respiration, combing carbon dioxide and water to make sugar 6CO2 + 6H2O + light energy >>> C6H12O6 + 6O2
Salts that produce acidic solutions contain ________ ions that release protons to water
positive
What type of type of salt produces an acidic solution? One that contains ________ ____ _____ _______ ____________ _____ __________
positive ions that release protons to water
According to Arrhenius, a base is an OH- _____
producer
According to Arrhenius, an acid is an H⁺________
producer
what are the three types of scabs
pus crust, blood crust, honey crust=lymph crust=eschar
bacterial: Boil
pus pocket
pseudofolliculitis barbe
razor bumps, ingrown hairs
another name for an oxidation-reduction reaction
redox reactions
the electron donor?
reducing agent
the substance in a redox reaction that gives up electrons Contains the atoms oxidized
reducing agent
The electron donor in a redox reaction is called the ____________? During the course of the reaction it becomes ____________.
reducing agent; oxizidized.
the complete or partial gain of electrons or the loss of oxygen
reduction
NADH
represents stored energy that is "trapped" to synthesize ATP
fungal infection is
ringworm and candida
Compounds consisting of an anion from an acid and a cation from a base
salt
In general, the reaction of an acid with a base produces and ______
salt
In this process, the cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water
salt hydrolysis
The reaction in which water molecules produce ions is called
self-ionization
miss pone
sharp pain and bleeding, higher % of infection, petechiae
what is another name for Herpes zoster
shingles, chicken pox, small pox, cow pox
Weak acids have ____ Ka values
small
K2SO4 (potassium sulfate)
soluble
these ions do not change oxidation number or composition during a reaction
spectator ions
bacterial: folliculitis
staph and pustules
bacterial: impetigo
staph and strep
___ bases dissociate completely into metal ions and hydroxide ions in aqueous solution
strong
Our waste products are the plant's The plant's waste products are our
substrate substrate
Fermentation is a partial degradation (break down) of?
sugars that occurs without oxygen
edema
swelling, blood serum, blood vessels widen
which electrode do the negatively charged ions move towards
the anode
which electrode does the positive ion go towards
the cathode (negative electron)
what is the cathode
the electrode at which reduction occurs
heparin and heparoids aid in what
the healing process, bleeding, and bruising
why can't a solid ionic compound be electrolysed
the ions are fixed in position and are not free to move, therefore can't carry charge
Which cation (metal or hydrogen) gets discharged during electrolysis of an aqueous solution?
the least reactive
The entire reaction of cellular respiration is...
the oxidation of glucose in order to form carbon dioxide and water (loses an hydrogen during oxidation..) oxidation refers to i lose an electron electrons in this case are associated with hydrogens Electrons are basically pulling all of the hydrogens off
what is electrolysis
the splitting up of an ionic compound using electricity
How to decide which solution is more concentrated in a titration
the substance that requires less volume to neutralise the other substance is more concentrated
what happens when ions gain or lose electrons at the electrode
they are discharged and form neutral atoms
what happens to the positive ions during electrolysis and where does it happen
they gain electrons so they are reduced at the cathode
Where does NADH pass the electrons?
through the electron transport chain
The process of adding a known amount of solution of known concentration to determine the concentration of another solution is called
titration
why is a trial run taken during a titration
to get a rough estimate of what volume is required o
What is the purpose of finding oxidation states in the half-reaction method for balancing equations?
to identify the half reactions for the equation
True or false: A buffer solution is better able to resist drastic changes in pH than is purse water
true
True or false: not all solution are neutral
true
Most heat resistant bacteria in the world
tuberculosis TB
how are viruses observed
under an electronic microscope
O oxidation number
usually -2, -1 in peroxide (H2O2)
Which anion (OH- or halide) gets discharged during electrolysis of an aqueous solution?
usually the halide ion (unless very dilute)
___ acids ionize only slightly in aqueous solution
weak
____ bases react with water to form the hydroxide ion and the conjugate acid of the base
weak
A buffer is a solution of a ____ acid and on of its salts, or a solution of a ____ base and one of its salts
weak, weak
