Acid Base Questions
ACID/BASE
You might need to know the following K values:
CH3COOH Ka = 1.8 x 10–5 Benzoic Acid Ka = 6.5 x 10–5
HNO2 Ka = 4.5 x 10–4 NH3 Kb = 1.8 x 10–5
HF Ka = 7.2 x 10–4 H2S Ka = 5.7 x 10–8
HSO4– Ka = 1.2 x 10–2 HS– Ka = 1.2 x 10–13
HCOOH Ka = 1.8 x 10–4 HOCl Ka = 3.0 x 10–8
SIMPLE ACIDS AND BASES
1. According to the Brønsted–Lowry definition, which species can function both as an acid and as a base?
(A) Cl– (B) SO42– (C) NH4+ (D) HCO3– (E) H3O+
2. Which of the following species can function as both a Brønsted-Lowry acid and a Brønsted-Lowry base in water?
(A) HCl (B) HPO42- (C) NH2– (D) H3O+ (E) NaOH
3. In this reaction, CH3COOH + H2O H3O+ + CH3COO–, which substances are bases according to the Brønsted–Lowry definition?
(A) CH3COOH and H2O (B) CH3COOH and CH3COO-
(C) H2O and CH3COO– (D) H3O+ and CH3COO–
4. In the reaction CN– + H2O HCN + OH–, which is an acid–base conjugate pair?
(A) H2O and HCN (C) CN– and H2O
(B) H2O and OH– (D) HCN and OH–
5. Which species is not either an Arrhenius acid or base?
(A) HCO3– (B) NaOH (C) HIO4 (D) NH3
6. When we say an ion or a molecule is a base, we mean that it has a tendency to
(A) combine with protons. (B) combine with electrons.
(C) liberate hydroxide ions as the only anions. (D) liberate hydronium ions as the only cations.
(E) Form only weakly dissociated salts.
7. Select the pair of substances in which an acid is listed followed by its conjugate base:
(A) NH3, NH4+ (B) HPO42-, H2PO4– (C) HCO3–, CO32-
(D) CH3COOH, CH3COOH2+ (E) H2O, H3O+
8. The conjugate acid of HPO42- is:
(A) P2O5 (B) PO43- (C) H2PO4- (D) H3O+ (E) H3PO4
Acid/Base Strengths
9. Given that HX is a stronger Brønsted acid than HY in aqueous solution, which is true of a 1 M solution of NaX?
(A) It is less basic than a 1 M solution of NaY. (B) It is more basic than a 1 M solution of NaY.
(C) It yields a neutral solution. (D) It is more concentrated than a l M solution of NaY.
10. Which
You might need to know the following K values:
CH3COOH Ka = 1.8 x 10–5 Benzoic Acid Ka = 6.5 x 10–5
HNO2 Ka = 4.5 x 10–4 NH3 Kb = 1.8 x 10–5
HF Ka = 7.2 x 10–4 H2S Ka = 5.7 x 10–8
HSO4– Ka = 1.2 x 10–2 HS– Ka = 1.2 x 10–13
HCOOH Ka = 1.8 x 10–4 HOCl Ka = 3.0 x 10–8
SIMPLE ACIDS AND BASES
1. According to the Brønsted–Lowry definition, which species can function both as an acid and as a base?
(A) Cl– (B) SO42– (C) NH4+ (D) HCO3– (E) H3O+
2. Which of the following species can function as both a Brønsted-Lowry acid and a Brønsted-Lowry base in water?
(A) HCl (B) HPO42- (C) NH2– (D) H3O+ (E) NaOH
3. In this reaction, CH3COOH + H2O H3O+ + CH3COO–, which substances are bases according to the Brønsted–Lowry definition?
(A) CH3COOH and H2O (B) CH3COOH and CH3COO-
(C) H2O and CH3COO– (D) H3O+ and CH3COO–
4. In the reaction CN– + H2O HCN + OH–, which is an acid–base conjugate pair?
(A) H2O and HCN (C) CN– and H2O
(B) H2O and OH– (D) HCN and OH–
5. Which species is not either an Arrhenius acid or base?
(A) HCO3– (B) NaOH (C) HIO4 (D) NH3
6. When we say an ion or a molecule is a base, we mean that it has a tendency to
(A) combine with protons. (B) combine with electrons.
(C) liberate hydroxide ions as the only anions. (D) liberate hydronium ions as the only cations.
(E) Form only weakly dissociated salts.
7. Select the pair of substances in which an acid is listed followed by its conjugate base:
(A) NH3, NH4+ (B) HPO42-, H2PO4– (C) HCO3–, CO32-
(D) CH3COOH, CH3COOH2+ (E) H2O, H3O+
8. The conjugate acid of HPO42- is:
(A) P2O5 (B) PO43- (C) H2PO4- (D) H3O+ (E) H3PO4
Acid/Base Strengths
9. Given that HX is a stronger Brønsted acid than HY in aqueous solution, which is true of a 1 M solution of NaX?
(A) It is less basic than a 1 M solution of NaY. (B) It is more basic than a 1 M solution of NaY.
(C) It yields a neutral solution. (D) It is more concentrated than a l M solution of NaY.
10. Which