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Acid-Base Test Review 1

Total questions: 25

Worksheet time: 4hrs 10mins

Name
Class
Date
1.

What allows us to know when the end point has been reached?

a)

Bubbles

b)

Feels warm

c)

indicator changing color

d)

Turns to a solid

2.
acid + base ₋>
a)
salt + hydrogen
b)
salt + water
c)
salt + carbon dioxide + water
d)
salt
3.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
4.
A solution with a pH of 8.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
5.

Why do we perform a titration?

a)

To determine the concentration of an unknown solution

b)

To see if a reaction will occur between an acid and base

c)

To find the mass of an unknown acid

d)

To find the molar mass of an unknown solution

e)

To calculate the viscosity of the solution

6.

If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? (record you answer with the correct unit)

a)

0.043 M

b)

0.034 M

c)

0.065 M

d)

0.77 M

7.

A 25.0 mL sample of HCl was titrated to the endpoint with 15.0 mL of 2.0 M NaOH. What is the molarity of HCl?

a)

1.6 M HCl

b)

0.03 M HCl

c)

0.6 M HCl

d)

1.2 M HCl

8.

What is a substance that increases the amount of H+ in a solution?

a)

Acid

b)

Base

c)

Litmus Paper

d)

Hydronium

9.

A 5.00 mL sample of household ammonia was analyzed by titration with hydrochloric acid according to the following reaction:   HCl  +  NH3  →  NH4 +   +  Cl −HCl\ \ +\ \ NH_3\ \ \rightarrow\ \ NH_4^{\ +}\ \ \ +\ \ Cl^{\ -}  
This titration required 19.5 mL of 0.750 M HCl. What is the molarity of the ammonia sample? 

a)

1.97 M

b)

2.19 M

c)

2.44 M

d)

2.92 M

10.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

11.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
12.

H3PO4

a)

hydrophsophorus acid

b)

phosphoric acid

c)

hydrogen phosphorous

d)

phosphori hydroxide

13.

Name this acid: HNO2

a)

hydronitrous acid

b)

hydrogen nitrogen oxygen

c)

nitrous acid

d)

hyponitrous acid

14.

A Bronsted-Lowry acid is a substance that...

a)

accepts H+ ions

b)

donates OH- ions

c)

increases the concentration of OH- ions

d)

donates H+ ions

15.

Which of the following could NOT act as a Bronsted-

Lowry acid?

a)

HCN

b)

H2SO4

c)

NH4+

d)

CN-

16.

A Bronsted-Lowry base is defined as a

substance that __________.

a)

increases [H+ ] when dissolved in H2O

b)

decreases [H+ ] when dissolved in H2O

c)

increases [OH-] when dissolved in H2O

d)

acts as a proton acceptor

17.

Which of the following compounds could never

act as a Bronsted-Lowry acid?

a)

SO4 2-

b)

HSO4-

c)

H2SO4

d)

NH4+

18.

According to the following reaction, which reactant

molecule is acting as an acid?


H2O + H2SO4 → H3O+ + HSO4-

a)

H2SO4

b)

H2O

c)

H3O+

d)

HSO4-

19.

According to the following reaction, which reactant

molecule is acting as a base?


H2O + H2SO4 → H3O+ + HSO4-

a)

H2SO4

b)

H2O

c)

H3O+

d)

HSO4-

20.

What is the conjugate base in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

21.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
22.

Which of the following is an Arrhenius Acid?

a)

LiOH

b)

CO32-

c)

OH-

d)

H3PO4

23.

Which of the following shows the correct acid / conjugate 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)
24.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
25.

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

a)

H2SO4, SO42-

b)

OH-, H2O

c)

NH4+, H2O

d)

H2CO3, HCO3-

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