Chem 130 Test 1
List the group 1A strong bases
LiOH, NaOH, KOH, RbOH, CsOH
Chloric acid
HClO3
Monoprotic
acids that contain one hydrogen molecule
Sulfuric Acid
H2SO4
Henry's Law
Sg=kPg
log(a^b)=
b(loga)
The presence of ions in a solution allows it to...
conduct electricity
If system gains entropy the value of ΔS will be...
positive
Give the Greek meaning for the word Metathesis.
"to transpose" or "to change partners"
mass percent=
(mass of solute/total mass) x 100
ppm=
(mass of solute/total mass) x 100 mg/kg or L
Determine the oxidation number of sulfur in SCl2
+2
Determine the oxidation number of sulfur in Na2SO3
+4
Determine the oxidation number of sulfur in H2S
-2
Rule #3 of oxidation numbers
-Oxygen has an oxidation number of -2 except for peroxide (-1) -Hydrogen is -1 when bonded to metal and +1 when bonded to nonmetal -Fluorine is always -1 -Other halogens have -1
Rule #4 of oxidation numbers
-The sum of the oxidation numbers in a neutral compound is 0 -The sum of the oxidation numbers in a polyatomic ion is the charge on the ion
Determine the oxidation number of sulfur in S8
0
Calculate the molarity of a solution made by dissolving 23.4g of Na2SO4 in enough water to form 125 mL of solution.
1.32 M
How many mL of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?
15 mL H2SO4
How many grams of Na2SO4 are required to make 0.350 L of 0.500 M Na2SO4?
24.9 g Na2SO4
Rule #1 of activity series
Any metal may be oxidized by ions of a metal salt below it on the table
List the heavy group 2A strong bases
Ca(OH)2, Sr(OH)2, Ba(OH)2
Rule #1 of oxidation numbers
Elements in their elemental form have an oxidation number of zero.
Acids increase the ___ concentration when dissolved in water.
H+
Hydrobromic Acid
HBr
Hydrochloric Acid
HCl
Perchloric Acid
HClO4
Hydroiodic Acid
HI
Nitric Acid
HNO3
What dissolved species are present in a solution of KCN
K+ (aq) and CN- (aq)
What dissolved species are present in a solution of NaClO4
Na+ (aq) and ClO4- (aq)
Bases increase the ___ concentration when dissolved in water.
OH-
Rule #2 of activity series
Only the metals above hydrogen in the activity series may react with acids
OIL RIG
Oxidation is loss (of electrons) Reduction is gain (of electrons)
What Swedish physicist/chemist defined acids as substances that increase the concentration of H+ when dissolved in water?
S. A. Arrhenius
Rule #2 of oxidation numbers
The oxidation number of a monatomic ion is the same as its charge
What is formed when ions are mixed to create new insoluble compounds?
a precipitate
Redox Reaction
a reaction in which certain atoms undergo changes in oxidation states
Nonelectrolyte
a substance that may dissolve in water, but does form ions when it does
Electrolyte
a substance that readily forms ions when dissolved in water
Tripotic
acids that contain three hydrogen molecules
Diprotic
acids that contain two hydrogen molecules
Other than ___ and ___, molecular compounds tend to be...
acids, bases, nonelectrolytes
Which ionic compounds are strong electrolytes?
all ionic compounds are strong electrolytes
Which antacids produce gaseous products?
any containing CaCO3
Soluble ionic compounds tend to be...
electrolytes
Solution
homogeneous mixture of two or more pure substances
Solubility of gases ___ with increasing mass.
increase
Classify lead sulfate (PbSO4) as soluble or insoluble.
insoluble
What is Henry's Law constant?
k=3.4x10^-2 mol/L-atm
If 10^x=50, then...
log50 = x
log(axb)=
loga + logb
log(a/b)=
loga - logb
mole fraction=
moles of component/total moles
molality (m)=
moles of solute/kg solvent
molarity (M)=
moles of solute/liters solution
If system loses entropy the value of ΔS will be...
negative
Any molecular compound that is not an acid or base is a ___ electrolyte.
non
Classify C2H5OH as strong, weak, or nonelectrolytic and explain your reasoning.
nonelectrolyte b/c it is a molecular compound
Dissociation
occurs when the solvent pulls the individual ions from the crystal and solvates them
The species that increases in oxidation states is...
oxidized
Bronsted and Lowry defined bases as...
proton acceptors
Bronsted and Lowry defined acids as...
proton donors
Oxidation-Reduction reactions are also called...
redox reactions
The species that decreases in oxidation states is...
reduced
Generally, when solutions of an acid and a base are combined, the products are ___ and ___.
salt and water
Classify sodium carbonate (Na2SO4) as soluble or insoluble.
soluble
Aqueous Solution
solution in which the solvent is water
Acids and bases that COMPLETELY ionize in the solution are...
strong
Strong acids and bases tend to be ___ electrolytes.
strong
Classify CaCl2 as strong, weak, or nonelectrolytic and explain your reasoning.
strong electrolyte b/c it is a soluble ionic compound
Classify KOH as strong, weak, or nonelectrolytic and explain your reasoning.
strong electrolyte b/c it is a strong base
Classify HNO3 as strong, weak, or nonelectrolytic and explain your reasoning.
strong electrolyte b/c it is one of the seven strong acids
Solute
substance dissolved into solvent
Solvent
substance having the greatest abundance in a solution
What is the most familiar redox reactions?
the corrosion of metal
Enthalpy (ΔH)
the measure of energy in a system
Spectator Ions
the species that didn't change in the reaction (and where deleted from a net ionic equation)
Entropy (ΔS)
the thermodynamic measure of disorder or randomness in a system
Acids and bases that PARTIALLY ionize in the solution are...
weak
Weak acids and bases tend to be ___ electrolytes.
weak
Classify HCOOH as strong, weak, or nonelectrolytic and explain your reasoning.
weak electrolyte b/c it is a weak acid
