Chemistry chapter 11
Which of the following is NOT a property of acids?
-Acids have a slippery feel. Acids turn litmus paper red. Acids have a sour taste. Acids dissolve many metals. All of the above are properties of acids.
weak acid
1.25 M H3PO4 [H3O+]=3.75 M [H3O+]<3.75 M -[H3O+]<1.25 M [H3O+]=1.25 M
weak base
1.94 M NH3 [OH−]<2.98 M [OH−]=1.94 M [OH−]=0.97 M -[OH−]<1.94 M
strong base
2.5 M KOH [OH−]<2.5 M [OH−]=5.0 M -[OH−]=2.5 M [OH−]<5.0 M
Determine [OH−] in each base solution. If the acid or the base is weak, indicate the value that [OH−] is less than
2.5 M KOH [OH−]=2.5 M
strong acid
2.77 M HCl [H3O+]<5.54 M -[H3O+]=2.77 M [H3O+]=5.54 M [H3O+]<2.77 M
PH+POH=14
4.76+9.24
How many moles of Ba(OH)2 are present in 145 mL of 0.400 M Ba(OH)2?
5.80×10−2 mol
Equivalence point
= PH7
KA lower
= weaker acid
Which of the following is the definition of a Brønsted-Lowry base?
A Brønsted-Lowry base is a proton acceptor.
Bronsted-Lowry base
A compound that acts in a reaction to d to accept a hydrogen Ion (proton / hydrogen accepter)
Bronsted-Lowry acid
A compound that acts in a reaction to donate a hydrogen ion (a hydrogen donor or a proton donor)
Neutralization
A reaction of an acid with a base, yielding a solution that is not as acidic or basic as the starting solutions were.
ate> ic+acid ite> ous+acid ide>hydro + ic +acid My R-ide has hydro-l-ic s Spr-ite is delici-ous I-ate dirt-ic
H2SO4 >SO4>Sulfate>sulfuric acid H2SO3>SO3>Sulfite>sulfurous acid H2S> S> Sulfide> Hydrosulfuric acid
EX: strong acid
HCl + H2O > H3O + Cl-
EX: weak acid
HF + H20 <> H30+ + F-
KA =
HF <> H + F KA= [H+][F-]/HF
Write a neutralization reaction for each acid and base pair HI(aq) and NaOH(aq) Express your answer as a balanced chemical equation. Identify all of the phases in your answer.
HI(aq)+NaOH(aq)→H2O(l)+NaI(aq)
H2SO3 Express your answer as an ion.
HSO3−
Strong acids
Hcl - Hydrochloric Hbr - Hydrobromic HI - HydroIodic HClO4 - percloric HNO3 - Nitric acid H2So4 - Sulfuric Acid
H30+
Hydronium
ion product constant for water
Kw = [H+][OH-] = 1.00x10^-14
Ca(OH)2
Ca(OH)2(aq)→Ca2+(aq)+2OH−(aq)
HCl Express your answer as an ion.
Cl−
weak Acid
Weak = dose not ionize completely, Equilibrium is Established
Polyprotic acid
an acid that can donate more than one proton per molecule H3Po4+H2O>H3O + H2Po4 H2Po4+H2O>H3O + HPo4 HPo4+H2O>H3O + Po4
Strong acid
an acid that ionizes completely in aqueous solution no equilibrium and goes to products
pOH = 6.5 Express your answer using one decimal place. pH = 7.5
basic
bases
bitter changes indicator blue feels slippery neutralizes acids to make salt water conducts electricity in solution corrodes flesh
weak base
other hydroxide and nitrogen
What is the pH of an aqueous solution with [H3O+] = 6×10−12 M ?
pH = 11.2
Phosphoric Acid
phosphate > PO4^-3 H+ H3PO4
KA higher =
stronger the acid
End Point
when the indicator changes color
Forward reaction favored
H C l ( l ) + O H − ( a q ) ⇌ H 2 O ( l ) + C l − ( a q ) HCl(l)+OH−(aq)⇌H2O(l)+Cl−(aq) H 2 S O 4 ( l ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + H S O 4 − ( a q ) H2SO4(l)+H2O(l)⇌H3O+(aq)+HSO4−(aq)
HbrO3 + H2O <> H30 + BrO3
acid base >< conacid conbase
HPO4^-2+H2O<>PO4^-3+H3O
acid base conbase conacid
pOH = 11.0 Express your answer using one decimal place. pH = 3.0
acidic
Reverse reaction favored
H S O 4 − ( a q ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + S O 4 2 − ( a q ) HSO4−(aq)+H2O(l)⇌H3O+(aq)+SO42−(aq) H 2 C O 3 ( l ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + H C O 3 − ( a q ) H2CO3(l)+H2O(l)⇌H3O+(aq)+HCO3−(aq)
The titration of a 20.0-mL sample of an H2SO4 solution of unknown concentration requires 22.87 mL of a 0.158 M KOH solution to reach the equivalence point. What is the concentration of the unknown H2SO4 solution?
.090 M H2SO4
A 25.00-mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the unknown H2SO4 solution?
0.1090 M H2SO4
How many moles of HNO3 are present if 5.80×10−2 mol of Ba(OH)2 was needed to neutralize the acid solution?
0.116 mol
What is the concentration of HNO3 if 0.116 mol are present in 895 mL of the solution?
0.130 M
strong base *mole ratios
0.225 M Ba(OH)2 [OH−]=0.225 M [OH−]<0.225 M [OH−]<0.450 M [OH−]=0.450 M
A 15.00-mL sample of a NaOH solution of unknown concentration requires 17.88 mL of a 0.1053 M H2SO4 solution to reach the equivalence point in a titration. What is the concentration of the NaOH solution?
0.2510 M
H2CO3+H2O⇌HCO3−+H3O+
Acid carbonic acid: H2CO3 Conjugate base bicarbonate: HCO3(-) Base water: H2O Conjugate acid hydronium ion
Arrhenius model of acids and bases
Acid - a compound that contains hydrogen and Ionizes to produce hydrogen Ions in water solution Base - a compound that produces hydroxide ions in water solutions
Which of the following is the definition of an Arrhenius base?
An Arrhenius base produces OH− ions in aqueous solutions.
Which of the following is NOT a property of bases?
Bases have a bitter taste. Bases have a slippery feel. -Bases dissolve many metals. Bases turn litmus paper blue. All of the above are properties of bases.
Strong base
First two rows w/ Hydroxide
Titration
Moles of acid = Moles of base MaVa=MbVb (only one to one ratio)
Determine whether each pair is a conjugate acid-base pair.
PO3−4, HPO2−4 HI, I−
Acid+Base>Water+Salt
SAlt is the +Ion base and - Ion Acid
acid
Sour change indicators red reacts with some metals to make h2 Neutralize basses to make salt and water conducts electricity in the solution corrodes flesh
Neutral
[ O H − ] = 1 × 10 − 7 M [OH−] = 1×10−7 M
Basic
[ O H − ] = 9 × 10 − 4 M [OH−] = 9×10−4 M [ O H − ] = 3 × 10 − 2 M [OH−] = 3×10−2 M [ O H − ] = 5 × 10 − 5 M [OH−] = 5×10−5 M
Acidic
[ O H − ] = 9 × 10 − 9 M [OH−] = 9×10−9 M [ O H − ] = 1 × 10 − 10 M [OH−] = 1×10−10 M [ O H − ] = 7 × 10 − 13 M [OH−] = 7×10−13 M [ O H − ] = 6 × 10 − 12 M [OH−] = 6×10−12 M
[H+][OH-]
[H+]>[OH-] = more acidic [H+]=[OH-] = neutral [H+]<[OH-] = more basic
Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric acid. What is the molar concentration of H3O+ in a cola that has a pH of 4.240?
[H3O+] = 5.75×10−5 M
most acidic to least acidic
[H3O+]=10−2[{\rm H_3O^+}] = 10^{-2} pH=3\rm pH = 3 pH=5\rm pH = 5 [H3O+]=10−6[{\rm H_3O^+}] = 10^{-6} pH=14
[H3O+] = 3.3×10−3 M
[OH−] = 3.0×10−12 M acidic
[H3O+] = 7.6×10−12 M
[OH−] = 1.3×10−3 M basic
1.94 M NH3
[OH−]<1.94 M
Amphoteric
a substance that can act as both an acid and a base
titration
is a method for determining the concentration of a solution by reacting a known volume of the solution with a solution of known concentration
