Free Printable Acids and Bases

1.

Which of the following values would represent the pH of a strong base?

a)

1

b)

8

c)

7

d)

13

2.

What range of values on the pH scale represent solutions with a higher ratio of hydronium (H₃O⁺) ions?

a)

0-14

b)

below 7

c)

7

d)

above 7

3.

Common salt is

a)

Acidic

b)

Neutral

c)

Basic

d)

all of them

4.

Neutralization is a reaction between

a)

Strong acid and a weak acid

b)

Strong base and a weak acid

c)

Strong acid and a strong base

d)

Strong acid and a weak base

5.

Name the acid present in our stomach.

a)

Sulphuric acid

b)

Hydrochloric acid

c)

Nitric acid

d)

Carbonic acid

6.

What is NOT a characteristic of a strong acid?

a)

High concentration of H+

b)

High concentration of OH-

c)

completely dissociates in an aqueous solution

d)

large distance between atoms

7.

Which of the following is a strong acid?

a)

Ethanoic acid

b)

Nitric acid

c)

Carbonic acid

d)

Citric acid

8.

Which of the following is the correct balanced equation showing the dissociation of sulfuric acid into ions?

a)

H₂SO₄ (aq) → H⁺ (aq) + SO₄^–(aq)

b)

H₂SO₄ (aq) ⇌ 2H⁺ (aq) + SO₄^2-(aq)

c)

HSO₄(aq) → H⁺(aq) + SO₄^–(aq)

d)

H₂SO₄ (aq) → 2H⁺ (aq) + SO₄^2-(aq)

9.

Which of the following statements is true?

a)

If the H⁺ ion concentration in a solution increases by a factor of 10, the pH of the solution increases by 1

b)

If the H⁺ ion concentration in a solution increases by a factor of 10, the pH of the solution decreases by 1

10.

What ions do Metals form when they react?

a)

Negative

b)

Positive

11.

Name the following in order:
HCl, HBr, HI

a)

hydrochloric acid, hydrobromic acid, hydroiodic acid

b)

chloric acid, bromic acid, iodic acid

c)

chlorous acid, bromous acid, iodous acid

d)

hydrochlorous acid, hydrobromous acid, hydroiodous acid

12.

What are the formulas for the following?
--sulfuric acid--
--nitric acid--

a)

H₂SO, HNO

b)

H₂SO₃, HNO₃

c)

H₂S, H₃N

d)

H₂SO₄, HNO₃

13.

What are the formulas for the following?
--hydrochloric acid--
--hydrobromic acid--
--hydroiodic acid--

a)

HClO₃, HBrO₃, HIO₃

b)

HCl, HBr, HI

c)

HClO₄, HBrO₄, HIO₄

d)

HClO, HBrO, HIO

14.

Which of the following is a weak acid

a)

$HClO_3$

b)

$H_2S$

c)

$HNO_3$

d)

HBr

15.

Which of the following is NOT a strong base

a)

$Be\left(OH\right)_2$

b)

$CsOH$

c)

KOH

d)

NaOH

16.

acid + base -->

a)

salt + water

b)

salt + oxygen

c)

salt + carbon dioxide

17.

Complete the following reaction:

HCl + MgOH -->

a)

$MgCl\ +H_2O$

b)

$Mg^+\ +\ H_2O$

c)

$MgCl+H^+$

d)

$MgCl+OH^-+CO_2$

18.

Complete the following reaction:

Sulfuric acid + magnesium oxide -->

a)

Magnesium sulfate + water

b)

Magnesium + water

c)

Magnesium sulfate + hydrogen

19.

Which is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

20.

pH is the measure of the concentration of ______.

a)

Acids

b)

H+ ion

c)

OH- ion

d)

Bases

21.

According to Arrhenius, what is the definition of an ACID?

a)

a substance that contains hydroxide and ionizes to produce OH-

b)

a substance that contains hydrogen and ionizes to produce H+

c)

a substance that contains hydrogen and ionizes to produce OH-

d)

a substance that contains hydroxide and ionizes to produce H+

22.

According to Bronsted-Lowry, what is the definition of an BASE?

a)

a substance that donates a hydrogen (H+) ion

b)

a substance that donates a hydroxide (OH-) ion

c)

a substance that accepts a hydrogen (H+) ion

d)

a substance that accepts a hydroxide (OH-) ion

23.

What is being donated/accepted between conjugate acid-base pairs?

a)

a hydrogen (H+) ion

b)

a hydroxide (OH-) ion

c)

water

d)

a neutron

24.

What is the conjugate base in the following reaction?

a)

HCO₃^-

b)

HCl

c)

H₂CO₃

d)

Cl-

25.

What is the conjugate acid in the following equation?

a)

PO₄^3-

b)

HNO₃

c)

NO₃^-

d)

HPO₄^2-

26.

Which of the following shows the correct conjugate acid base pair?

a)

HCI (acid) / H₃O⁺ (conjugate base)

b)

HCI (acid) / CI^- (conjugate base)

c)

HCI (base) / CI^- (conjugate acid)

d)

HCI (base) / H₃O⁺ (conjugate acid)

27.

Which of the following are properties of acids but not bases? Select all that apply.

a)

Changes the color of an indicator

b)

Sour taste

c)

Reacts with metals to produce hydrogen gas

d)

Feels slippery

28.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

29.

An arrhenius acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

30.

An arrhenius base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

31.

A bronsted lowry acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

32.

Water can act as both an acid and a base according to the bronsted lowry model. This means water is

a)

neutral

b)

conjugate

c)

ionic

d)

amphoteric

33.

Identify the true statement about the following reaction:

F^- + H₂O --> HF +OH^-

a)

H₂O is a bronsted lowry base

b)

H₂O is not an acid or base according to either model

c)

H₂O is a bronsted lowry acid

d)

H₂O is an arrhenius acid

34.

Acid-base conjugate pairs differ by a single

a)

Electron

b)

Proton

c)

Neutron

d)

Oxygen

35.

Which of the following show an acid and its conjugate base pair (in that order)

a)

H₂SO₄, SO₄^2-

b)

OH^-, H₂O

c)

NH₄⁺, H₂O

d)

H₂CO₃, HCO₃^-

36.

What is the conjugate acid of water?

a)

$OH^-$

b)

$H_3O^+$

c)

$H_2O_2$

d)

$HOH$

37.

A strong base in a water solution

a)

is a weak electrolyte

b)

produces many H⁺ ions

c)

will not dissolve

d)

completely dissociates into ions.

38.

What is the pH of a solution with a hydrogen ion concentration of 1.0 x 10^-8 M?

(HINT...pH = -log [H⁺] )

a)

-8

b)

6

c)

8

d)

14

39.

What is the pH of a 0.0001 M HCl solution

a)

1

b)

4

c)

7

d)

11

40.

What is the pOH of a 1 x 10^-8M solution of HNO₃?

a)

8

b)

6

c)

7

d)

7.5

41.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10^-14

d)

-log (1.0 x 10 ^-14)

42.

What is the pH of a solution that has a [H+] of 2.5 x 10^-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

43.

Acids have a ______ pH and a _________ pOH

a)

low, high

b)

high, low

c)

An acid will not have a pOH

44.

Find the pH of a solution with [OH-] = 8.41 x 10^-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

45.

What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__H₂SO₃ + __KOH--> __H₂O+ __K₂SO₃

a)

2,1 --> 2,1

b)

1,2 --> 1,1

c)

1,2 --> 1,2

d)

1,2 --> 2,1

46.

Which problem is balanced?

a)

PbO₂ + 2H₂

b)

SO₂ + H₂0 --> H₂SO₄

c)

2Na + 2H₂O --> 2NaOH + H₂

47.

Balance this equation
_Zn+_HCl-->_ZnCl₂+_H₂

a)

1,1,2,1

b)

1,1,1,2

c)

1,2,1,1

d)

2,1,1,1

48.

A solution has a [OH-] of $7.23\ \times10^7$ . This solution has a pOH of

a)

$1.7\ \times10^7$

b)

$5.89\ \times10^{-8}$

c)

11.9

d)

2.14

49.

Calculate the $\left[H^+\right]$ for the following $\left[OH^-\right]$ .

$\left[OH^-\right]\ =\ 6.83\ x\ 10^{-11}$

a)

$\left[H^+\right]\ =\ 3.8$

b)

$\left[H^+\right]\ =\ 1.48\ x\ 10^{-4}$

c)

$\left[H^+\right]\ =\ 1.02\ x\ 10^{-1}$

d)

$\left[H^+\right]\ =\ 1.5\ x\ 10^5$

50.

Calculate the pOH for the following concentration.

$\left[H^+\right]\ =\ 4.72\ x\ 10^{-3}$

a)

pOH = $1.0\ \times10^{-12}$

b)

pOH = 2.33

c)

pOH = $2.12\ \times\ 10^{-12}$

d)

pOH = 11.7

Acids and Bases

Total questions: 50

Worksheet time: 38mins

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