Free Printable Acids & Bases

1.

Which of the following conditions represents a neutral solution at 25 degrees Celsius?

a)

[OH^-] = 1.0 x 10^-7 M

b)

[H⁺] = 1.0 x 10^-7 M

c)

K_w = [H⁺][OH^-] = 1.0 x 10^-14 M

d)

All of the answer choices!

2.

Which substance could not be classified as an Arrhenius acid?

a)

HBr

b)

HCl

c)

H₂SO₄

d)

NaCl

3.

Use the Common Acids & Bases table in your notes for this question: Which acid would be considered a weak electrolyte?

a)

hydrochloric acid

b)

potassium hydroxide

c)

dihydrogen monoxide

d)

carbonic acid

4.

Which statement is true about Bronste-Lowery acids?

a)

Arrhenius acids are also Bronsted-Lowery acids.

b)

Bronsted-Lowery acids are hydrogen ion acceptors.

c)

A Bronsted-Lowery acid will form a conjugate acid after losing a hydrogen ion.

d)

Bronsted-Lowery acids contain hydroxide ions.

5.

Sulfuric acid reacts with lithium hydroxide to produce a salt and water. What is the correct name and formula of the salt that is produced? *Salt = Cation from the base + Anion from the acid

a)

Lithium Sulfuric; LiSO₄

b)

Lithium Sulfate; Li₂SO₄

c)

Lithium Sulfate; Li(SO₄)₂

6.

Zachary prepared an aqueous solution with a [H⁺] = 8.03 x 10^-9 M. Is his solution acidic, basic, or neutral?

a)

acidic

b)

basic

c)

neutral

7.

Which substance can be classified as an Arrhenius base?

a)

Mg(OH)₂

b)

CH₃COOH

c)

NH₃

8.

The pH of a solution is 4.91. What is the pOH of the solution?

a)

18.91

b)

1.2 x 10^-5

c)

9.09

9.

Zarinah made a buffer solution with a pH 8.31. What is the hydroxide ion concentration, [OH^-], of her solution?

a)

5.0 x 10^-9 M

b)

1.0 x 10^-5 M

c)

2.0 x 10^-6 M

10.

Use the table of Common Acids & Bases in your notes to answer this question: Which list of acids is arranged in order of decreasing strength?

a)

H₃PO₄, H₂SO₄, HNO₃

b)

HC₂H₃O₂, H₂CO₃, HClO

c)

HClO, HCl, HC₂H₃O₂

11.

Which balanced neutralization reaction represents the following: phosphoric acid reacts with beryllium hydroxide to produce beryllium phosphate and water?

a)

$3Be\left(OH\right)_2\ +\ 2H_3PO_4\ \ \rightarrow\ \ 6H_2O\ +\ Be_3\left(PO_4\right)_2$

b)

$BeOH_2\ +\ H_3PO_4\ \ \rightarrow\ \ 3H_2O\ +\ BePO_4$

c)

$3BeOH_2\ +\ 2H_3PO_4\ \ \rightarrow\ \ 3H_2O\ +\ Be_3\left(PO_4\right)_2$

12.

Niara has an aqueous solution with a pOH of 5.95. What is the hydrogen ion concentration, [H⁺], of her solution?

a)

8.05 M

b)

8.91 x 10^-9 M

c)

1.12 x 10^-6 M

13.

Calculate the pH of a solution that has a hydrogen ion concentration, [H⁺], equal to 1.0 x 10^-13.

a)

13

b)

1

c)

27

14.

Polly created an aqueous solution that has a pOH = 10.4. What is the hydrogen ion concentration, [H⁺], of her solution?

a)

3.98 x 10^-11 M

b)

3.6 M

c)

2.51 x 10^-4 M

15.

A(n) _ is hydrogen ion acceptor.

a)

Arrhenius Acid

b)

Brønsted-Lowry Acid

c)

Arrhenius Base

d)

Brønsted-Lowry Base

16.

Arsenic acid, H₃AsO₄, would be classified as a __ Arrhenius acid.

a)

monoprotic

b)

diprotic

c)

triprotic

17.

Which substance would not be classified as a base?

a)

bleach

b)

vinegar

c)

dish detergent

18.

What is the "conjugate acid - conjugate base" pair in the following reaction: $H_3PO_4\ +\ H_2O\ \ \rightarrow\ \ H_3O^+\ +\ H_2PO_4^-$

a)

$H_3PO_4\ and\ H_2O$

b)

$H_3PO_4\ and\ H_2PO_4^-$

c)

$H_3O^+\ and\ H_2PO_4^-$

d)

$H_2O\ and\ H_3O^+$

19.

What is the "base - conjugate acid" pair in the following reaction: $NH_3\ +\ H_2SO_4\ \ \rightarrow\ \ HSO_4^-\ +\ NH_4^+$

a)

$H_2SO_4\ and\ HSO_4^-$

b)

$NH_3\ and\ H_2SO_4$

c)

$HSO_4^-\ and\ NH_4^+$

d)

$NH_3\ and\ NH_4^+$

20.

Richard made a buffer solution with a pOH of 12.09. What is the pH of his solution? Is his buffer solution acidic or basic?

a)

1.91; acidic

b)

1.91; basic

c)

8.13 x 10^-13; acidic

d)

26.09; basic

Acids & Bases - Calculations

Total questions: 20

Worksheet time: 19mins

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