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Acid Base Salts

Total questions: 45

Worksheet time: 1hrs 17mins

Name
Class
Date
1.

According to which scientist's theory is a base a substance which produces OH- ions in water?

a)

Arrhenius

b)

Bronsted-Lowry

c)

Lewis

2.

According to Bronsted-Lowry acid base theory, an acid is a.....

a)

proton donor

b)

proton acceptor

c)

produces H+ when added to water

d)

made of H+

3.

According to Lewis acid-base theory, a Lewis base is.....

a)

an electron pair acceptor

b)

an electron pair donor

c)

an oxidising agent

d)

a reducing agent

4.

According to Arrhenius acid-base theory, an acid is....

a)

an H+ acceptor

b)

a H+ donor

c)

a substance that produces H+ in water

d)

anything with an H+

5.
According to which acid-base theory is a base a proton acceptor?
a)
Arrhenius
b)
Bronsted-Lowry
c)
Lewis
6.

Which reactant in the following equation is a Bronsted acid?

a)

ammonium

b)

ammonia

c)

hydroxide

d)

water

7.

Which reactant in the following equation is a Bronsted acid?

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

8.

HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq)

Identify the Acid in the above reaction.

a)

HSO4-

b)

H2O

c)

H3O+

d)

SO42-

9.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
10.

A substance that remains when a base has accepted an H+ ion is

a)

An acid

b)

A base

c)

A conjugate acid

d)

A conjugate base

11.

In the equation below, what is the Bronsted Lowry acid?

HCl + NH3 --> Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

12.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

13.

True or false: a neutral solution has equal amounts of H+ and OH-.

a)

True

b)

False

14.

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

a)

4.60

b)

5.0

c)

2.5

d)

7

15.

What is a solution's [H+] concentration if the pH is 10.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-4 M

c)

1.0 x 10-14 M

d)

1.0 x 10-7 M

16.

The lower the pH, the greater the concentration of:

a)

OH-

b)

H-

c)

H3O+

d)

Na+

17.

HClO4 is a strong acid and dissociates completely. What is the pH of a 0.15 M solution of HClO4?

a)

0.82

b)

13.18

c)

0.15

d)

1

18.

Acidic solutions exhibit a higher ratio of H3O+ ions, known as...

a)

neutrons

b)

hydroxide

c)

electrons

d)

hydronium

19.

What completely ionizes in solution?

a)

Weak acids

b)

Strong acids

c)

Strong Salts

d)

Neutral salts

20.

This solution is filled with:

a)

Weak Acid

b)

Strong Base

c)

Strong Acid

d)

Weak Base

21.

Tastes bitter

a)

acid

b)

base

c)

both an acid and a base

22.

Turns indicators different colors

a)

acid

b)

base

c)

both an acid and a base

23.

What are the formulas for the following?


--sulfuric acid--

--nitric acid--

a)

H2SO, HNO

b)

H2SO3, HNO3

c)

H2S, H3N

d)

H2SO4, HNO3

24.
Which of the following is a pH for a strong base? 
a)
1
b)
8
c)
7
d)
13
25.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
NaOH
a)
NaOH(s) --> Na+(aq) + OH-(aq) 
b)
NaOH --> Na+ + OH- 
c)
NaOH --> Na + OH
d)
NaOH(s) --> NaO-(aq) + H+(aq) 
26.

Kw for water is called

a)

water dissociation constant

b)

product constant

c)

ionic product constant

d)

acid dissociation constant

27.

dissociation of weak acid, HA, is represented by following equation :


HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)


The equilibrium constant for this reaction is represented by Ka . Which of the following equation represents expression of equilibrium constant, Ka?

a)
b)
c)
d)
28.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
29.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

30.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
31.

What is the molarity of a 30 mL HCl which is neutralized by 48 mL of 0.3 M sodium hydroxide? HCl + NaOH --> H2O + NaCl

a)

0.16 M

b)

6.25 M

c)

0.48 M

32.

What is the endpoint of a titration?

a)

Where the amount of acid and base are equal as shown by a color change

b)

Where there is no base

c)

When the volume of base in the burette is used up

d)

When there is no acid

33.

What is the main purpose of acid-base titrations?

a)

To test if reactants react.

b)

To calculate the concentration of unknown analyte.

c)

To calculate the concentration of known analyte.

d)

To test quality of reactants.

34.

What is the role of an indicator in a reaction?

a)

To help reactants react successfully.

b)

To bind to the analyte to form a product.

c)

To show when the reaction has reached or past the equivalence point.

d)

To provide a surface for the reaction to occur.

35.

What is an equivalence point?

a)

It is the point when enough analyte has been added.

b)

It is the point when the amount of added titrant is equal to the amount of analyte in the solution.

c)

It is the point when the volume of titrant is equivalent the volume of analyte.

d)

It is the point when the concentration of titrant added is equivalent to the volume of analyte.

36.

Which of the following best represents a 0.100-molar solution of H2SO4 in water?

a)
b)
c)
d)
37.

Which of the following best approximates the Ka value for this weak acid?

a)

1 x 10–4

b)

1 x 10–5

c)

5x 10–6

d)

5 x 10–7

38.

Which of the following indicators is the best choice for this titration?

a)

Methyl orange (pH range of color change is 3.2 - 4.4)

b)

Methyl red (pH range of color change is 4.8 - 6.0)

c)

Bromothymol blue (pH range of color change is 6.1 - 7.6)

d)

Phenolphthalein (pH range of color change is 8.2 - 10.0)

39.
Buffer is defined as
a)
ability to resist pH change
b)
ability to prevent pH from decreasing
c)
ability to resist a pH increase
d)
ability to resist pH change when small amount of acid added
40.
Acidic buffer is made up of
a)
weak acid and weak base
b)
weak acid and its conjugate salt
c)
weak acid and its conjugate base
d)
strong acid and its conjugate base
41.

This equation produces...

a)

Kb

b)

pKb

c)

Ka

d)

pOH

42.

H3PO4 is an example of a ...

a)

monoprotic acid

b)

diprotic acid

c)

triprotic acid

43.

Which is a diprotic acid?

a)

chlorous acid (HClO2)

b)

nitrous acid (HNO2)

c)

sulfurous acid (H2SO3)

d)

phosphorous acid (H3SO4)

44.

Since water can act as an acid or a base, it is called _____.

a)

hydroprotic

b)

amphoteric

c)

weird

d)

conjugate

45.

Acids are __________, which means they "eat away" at other materials.

a)

transitional metal

b)

alkaline

c)

flammable

d)

corrosive

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