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