SCH 4UI – Acid-Base Review
A.
Acid-Base Theory. State which compounds or ions are the acid, base, conjugate
acid and conjugate base of each equilibrium equation.
1.
2.
3.
4.
5.
6.
7.
8.
9.
H2O(l) + CO32-(aq) ↔ OH-(aq) + HCO3-(aq)
HNO3(aq) + H2O(l) ↔ NO3-(aq) + H3O+(aq)
H2SO4(aq) + HClO4(aq) ↔ H3SO4+(aq) + ClO4-(aq)
H2O(l) + H2O(l) ↔ OH-(aq) + H3O+(aq)
HCl(aq) + OH-(aq) ↔ H2O(l) + Cl-(aq)
H3PO4(aq) + H2O(l)
H2PO4-(aq) + H3O+(aq)
HCO3–(aq) + HSO4–(aq) → CO32–(aq) + H2SO4(aq)
NH3(aq) + H2O(l)
NH4+(aq) + OH-(aq)
HNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq)
B.
Name and write the formula of the conjugate base for each molecule:
1) HCl
2) HCO33) H2SO4
C.
Name and write the conjugate acid of each molecule:
1) NO32) OH3) H2O
4) HCO3-
D.
Acid-Base Theory. State the conjugate acid or base for each substance listed.
1) HC2H3O2(aq)
E.
2) CO32-(aq)
3) HCO3-(aq)
Strong Acids and Bases
1. Calculate the concentration of the hydroxide ions of a 0.15 mol/L solution of
hydrochloric acid at SATP.
2. Calculate the hydrogen ion concentration in a 0.25 mol/L solution of barium hydroxide (a
strong base).
3. Find the values of [H+], pOH and [OH-] that correspond to each of the following values
of pH.:
a) 2.90 (the approximate pH of lemon juice)
b) 3.85 ( the approximate pH of sauerkraut)
c) 4.11 (the pH of orange juice, on the average)
d) 11.61 (the pH of dilute, household ammonia)
F.
Acid-Base (Determining pK, Kw, Ka, Kb, pH and pOH)
1. The pH of a 0.10 mol/L methanoic (formic) acid solution is 2.38. Calculate the percent
ionization of methanoic acid.
2. Determine the pH of 0.100 mol/l Acetic Acid (HC2H3O2(aq)) if the percent ionization is
1.3%
3. Calculate the acid ionization constant, Ka, of acetic acid if a 0.1000 mol/L solution at
equilibrium at SATP has a percent ionization of 1.3%
4. What is the value of the base ionization constant, Kb for the acetate ion, C2H3O2-(aq), at
SATP?
5. Calculate [H+(aq)] and pH of 0.10 mol/L acetic acid. Ka for acetic acid is 1.8 x 10-5.
6. The pH of a 0.100 mol/L hypochlorous acid (HClO) solution is 4.23. What is the K a for
hypochlorous acid?
7. Calculate the pH of a 0.100 mol/L solution of hydrazine, N2H4, a weak base.
8. Calculate the pH of a 0.10 mol/L solution of ascorbic acid, H2C6H6O6, if Ka1 = 7.9 x 10-5
and Ka2 = 1.6 x 10-12
9. Calculate the pH of a 0.10 mol/L solution of NaNO2(aq)
10.Calculate the pH of a 0.20 mol/L solution of NH4Cl(aq)
G.
Acid-Base Salts
 Be ready to refer to the summary of The Acid-Base Properties of Salts on page 592
 You will need Appendix C9 on page 803
1. Determine whether the following compounds will be acids, bases or neutral:
a) NaCN
d)
AlCl3
g)
NH4I
j)
SO2
b) CaO
e)
HNO3
h)
Fe(NO3)3 k)
LiF
c) Ca(OH)2
f)
N2H4
i)
NH4NO2
l)
NaBrO4
2. Write a 1, 2 or 3-step dissociation equation for the following compounds:
a)
AlBr3
b)
NH3
c)
benzoic acid
b)
H2O
d)
C5H5N
f)
H2SO3
g)
CaCO3
h)
HCl
i)
NH4Cl
3. Which acid will be stronger; benzoic acid or phenol? Use Appendix C9 to help you
answer the question. Which ion will form a stronger base:C6H5O2-(aq) or C6H5O-(aq)?
4. What is the pH of 0.100 mol/L solution of NaNO2?
5. What is the pH of a 0.025 mol/L solution of NH4Cl?
6. What is the pH of a 0.200 mol/L solution of FeCl3?