chapter 16
Which one of the following is a Bronsted-Lowry base? HF CH3COOH HNO2 (CH3)3N None of the above
(CH3)3N
Designate the Bronsted-Lowry acid and the Bronsted-Lowry base; designate the conjugate acid and conjugate base (CH3)3N (aq) + H2O (l) = (CH3)3NH+ (aq) + OH- (aq)
(CH3)3N (aq) is the B-L base; H2O (l) is the B-L acid. (CH3)3NH+ is the conj. acid; OH- (aq) is the conj. base.
Which solution has the higher pH, a 0.001 M solution of NaOH or a 0.001 M solution of Ba(OH)2
0.001 M solution of Ba(OH)2
Which solution will be the most basic?
0.03 M Ca(OH)2
Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00
1.0 x 10^-3
In a certain acidic solution at 25C, [H+] is 100 times greater than [OH-]. What is the value for [OH-] for the solution?
1.0 x 10^-8
A 6.0 x 10^-3 M aqueous solution of Ca(OH)2 at 25 C has a pH of
12.08
The Ka for HCN is 4.9 x 10^-10. What is the value of Kb for CN-?
2.0 x 10^-5
At 25 C the following data was collected: Solution A: pH = 8.46 Solution B: pH = 9.30 Solution C: [H+] = 2.5 x 10^-4 M Solution D: [OH-] = 1.1 x 10^10 M Which lists the solutions in order of increasing acidity?
A<B<D<C
Which one of the following is a Bronsted-Lowry acid? (CH3)3NH+ CH3COOH HF HNO2
All of the above
Predict the stronger acid in each pair: Part A: CH3COOH CH3OH Part B: H2S H2O Part C: H2SO4 H2SeO4 Part D: CCl3COOH CH3COOH
CH3COOH H2S H2SO4 CCl3COOH
What two ions are central to the Arrhenius definitions of acids and bases?
H+, OH-
The hydride ion, H-, is a stronger base than the hydroxide ion, OH-. The product(s) of the reaction of hydride ion with water is/are
H- + H2O = H2 + OH-
Give the conjugate acid of the following Bronsted-Lowry base: H2PO4-
H2PO4- = H3PO4
Using the data in the table, which of the conjugate acids below is the strongest acid? CIO- Kb = 3.3 x 10^-7 CO3 2- Kb = 1.8 x 10^-4 HS- Kb = 1.8 x10^-7 NH2CH3 Kb = 4.4 x 10^-4
H2S
Designate the Bronsted-Lowry acid and the Bronsted-Lowry base; designate the conjugate acid and conjugate base HCHO2 (aq) + PO4 3- (aq) = CHO2 - (aq) + HPO4 2- (aq)
HCHO2 (aq) is the B-L acid; PO4 3- (aq) is the B-L base. HPO4 2- (aq) is the conj. acid; CHO2- (aq) is the conj. base.
Of the following, _______ is a weak acid. HCI HCIO4 HNO3 HBr HF
HF
Of the acids in the table below, _________ is the strongest acid. HOAc Ka: 1.8 x 10^-5 HCHO2 Ka: 1.8 x 10^-4 HCIO Ka: 3.0 x 10^-8 HF Ka: 6.8 x 10^-4
HF Ka: 6.8 x 10^-4
Give the conjugate base of the following Bronsted-Lowry acid: HIO3
HIO3 = IO3-
Of the following acids, ________ is a strong acid. HF HNO2 HCIO H2CO3 HNO3
HNO3
Consider the following equilibrium reaction: HSO4- (aq) + OH- (aq) = SO4 2- (aq) + H2O (l) which substances are acting as acids in the reaction?
HSO4- and H2O
The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25 C is 2.03. What is the value of Ka for HF?
Ka = 3.5 x 10^-4
HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25 C. The Ka of HZ is
Ka = 6.9 x 10^-9
Designate the Bronsted-Lowry acid and the Bronsted-Lowry base; designate the conjugate acid and conjugate base NH4+ (aq) + CN- (aq) = HCN (aq) + NH3 (aq)
NH4+ (aq) is the B-L acid; CN- (aq) is the B-L base. HCN (aq) is the conj. acid; NH3 (aq) is the conj. base.
Give the conjugate base of the following Bronsted-Lowry acid: NH4+
NH4+ = NH3
Give the conjugate acid of the following Bronsted-Lowry base: O2-
O2- = OH-
Using the data in the table, which of the following of the conjugate bases below is the strongest base? HOAC Ka = 1.8 x 10^-5 HC7H5O6 Ka = 6.3 x 10^-5 HNO2 Ka = 4.5 x 10^-4 HF Ka = 6.8 x 10^-4
OAC-
For the reaction: H2NNH (aq) + H2O (l) - H2NNH3+ (aq) + OH- (aq) Determine the conjugate base of the acid?
OH-
Which of the following aqueous solutions has the highest [OH-]? A solution with a pH of 3.0 A 1 x 10^-4 solution of HNO3 A solution with a pOH of 12.0 Pure water A 1 x 10^-3 M solution of NH4Cl
Pure water
The hypochlorite ion, CIO-, acts as a weak base. Part A: Is CIO- a stronger or weaker base than hydroxylamine? Part B: When CIO- acts as a base, which atom acts as the proton acceptor?
Stronger O
Which one of the following statements regarding Kw is false?
The value of Kw is always 1.0 x 10^-14
Which of the following ions will act as a weak base in water? OH- NO3- CIO- Cl- none of the above will act as a weak base in water
[CIO-]
The pH of an aqueous solution at 25 C is 10.00. What is the molarity of H= in this solution?
[H+] = 1 x 10^10
The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 x 10^-4 at 25 C. The [H+] in a 1.3 x 10^-2 M solution of ethylamine is ________ M
[H+] = 3.9 x 10^-12
In neutral solution,
[H3O+] = [OH-]
What is an Arrhenius base?
a substance that produces OH- in water
An aqueous solution at 25.0 C contains [H+] = 0.095 M. What is the pH of the solution?
pH = 1.02
Calculate the pH of a 0.500 M aqueous solution of NH3. The Kb of NH3 is 1.77 x 10^-5
pH = 11.47
What is the pH of an aqueous solution at 25 C in which [H+] IS 0.0015 M?
pH = 2.82
Which solution below has the highest concentration of hydronium ions?
pH = 3.7
The Ka of hypochlorous acid (HCIO) is 3.00 x 10^-8. What is the pH at 25 C of an aqueous solution that is 0.0200 M in HCIO?
pH = 4.61
What is the pH of a solution that is 3.5 x 10^-9 M in NaOH?
pH = 7.01
If colorless solution turns pink when we add phenolphthalein, what can we conclude about the pH of the solution?
pH>10
The acid-dissociation constant at 25 C of hypochlorous acid (HCIO) is 3.0 x 10^-8. At equilibrium, the molarity of H3O+ in a 0.033 M solution of HCIO is
x = 3.1 x 10^-5
