# Take This pH Level Test Of Chemical Solutions!

28 Questions | Total Attempts: 639  Settings  PH is a quantitative measure of the acidity which is measured with a pH meter for chemical solutions and widely used in chemistry, biology, and agronomy. S. P. L. Sørensen, a Danish biochemist, introduced the concept of pH, for measuring acidity and alkalinity. This quiz had been designed to test your knowledge about the pH level and effects of the solution. Read the questions carefully and answer. So, let's try out the quiz. All the best!

• 1.
Calculate the hydroxide ion concentration of a solution if its pH is 6.389
• A.

1.00 x 10 -14 mol/L

• B.

4.08 x 10 -7 mol/L

• C.

2.45 x 10 -8 mol/L

• D.

9.92 x 10 -7 mol/L

• 2.
What is the hydronium ion concentration in a solution with a pH of 2.80?
• A.

6.3 x 10 -2 mol/L

• B.

6.3 x 10 2nd power mol/L

• C.

4.8 x 10 -8 mol/L

• D.

1.6 x 10 -3 mol/L

• 3.
Consider the reaction of the base, ammonia (NH3), with water. The conjugate acid of NH3 is?
• A.

NH4+

• B.

H3O+

• C.

NH2-

• D.

OH-

• 4.
Which of the following is not a strong acid in water?
• A.

HF

• B.

HCl

• C.

HBr

• D.

HNO3

• 5.
Which of the following substances when dissolved in water will form an acid aqueous solution?
• A.

KI

• B.

CH3COONa

• C.

Ba(OH)2

• D.

NH4Cl

• 6.
What is the pH of a 675 mL aqueous solution containing 0.036 mol of NaOH?
• A.

1.27

• B.

3.41

• C.

10.58

• D.

12.73

• 7.
Or which one of the following reactions is the equilibrium constant Kc >1?
• A.

CH3COOH+H2O--CH3COO+H3O+

• B.

CH3COOH +OH--CH3COO +H2O

• C.

NH4+ +H2--NH3 +H2O+

• D.

Cl- +H2O--HCl +OH-

• 8.
Which, if any, of the following is an example of the leveling effect?
• A.

The concentrations of H+ and OH- in pure water are equal

• B.

The number of strong acids equals the number of strong bases

• C.

The number of strong acids equals the number of weak acids

• D.

In water, no acid stronger than H3O+ can exist

• 9.
Which of the following is most likely to act as a Lewis acid?
• A.

NH3

• B.

BF3

• C.

F

• D.

H2O

• 10.
Identify the conjugate base of HCO3- in the following reaction: CO3 2- +HSO4 ---HCO3- +SO4 2-
• A.

HSO4-

• B.

CO3 2-

• C.

OH-

• D.

SO4 2-

• 11.
Identify the conjugate acid of SO4 2- in the following reaction: CO3 2- +HSO4- ----HCO3- +SO4 2-
• A.

CO3 2-

• B.

OH-

• C.

HSO4-

• D.

H3O+

• 12.
The OH- concentration in 1.0 x 10 -3 M Ba(OH)2 is:
• A.

2.00 x 10 -3 M

• B.

0.50 x 10 -3M

• C.

1.00 x 10 -3 M

• D.

1.00 x 10 -2 M

• 13.
A 0.10 M NH3, solution is 1.3% ionized. Calculate the H+ ion concentration. NH3+H2O--NH4+ +OH-
• A.

1.3 x 10 -3 M

• B.

7.7 x 10 -12 M

• C.

7.7 x 10 -14 M

• D.

0.13 M

• 14.
The pH of coffee is approximately 5.0. How many times greater is the [H3O+] in coffee than in tap water with a pH of 8.0?
• A.

0.62

• B.

30

• C.

1.6

• D.

1000

• 15.
Acid strength increases in the series HCN
• A.

H2SO4

• B.

SO4 2-

• C.

F-

• D.

CN-

• 16.
Which one of the following equations represents the reaction of a strong acid with a strong base?
• A.

H+(aq) + OH-===H2O(aq)

• B.

H+(aq)+CH3NH2(aq)--CH3NH3+(aq)

• C.

OH(aq)+HCN(aq)--H2O(aq)+CN-(aq)

• D.

HCN(aq)+CH3NH2(aq)--CH3NH3+(aq)+CN-(aq)

• 17.
Predict the direction in which the equilibrium will lie for the followijng reaction. C5H5COO- +HF--C6H5COOH +F
• A.

To the right

• B.

To the left

• C.

In the middle

• 18.
Hard water deposits (calcium carbonate)have built up around your bathroom sink. Which one of the following would be best to dissolve the deposit?
• A.

Ammonia

• B.

Lye

• C.

Bleach

• D.

Vinegar

• 19.
If a weak acid HA has Ka=10-5, what is the pH of a mixture of 0.1 mole of the acid and 0.1 mole of its conjugate based in 1.0 liter of water?
• A.

3

• B.

4

• C.

5

• D.

9

• 20.
What is the solubility product constant expression (Ksp) for PbCl2?
• A.

[Pb2+](2)[Cl]

• B.

[Pb2+][Cl-]/2

• C.

[Pb2+][Cl-]2

• D.

[Pb2+][Cl-]/[[PbCl2]

• 21.
Which one of the following salts would form an acidic solution when dissolved in water.
• A.

NaBr

• B.

NaF

• C.

NaHSO4

• D.

CaCl2

• 22.
Calculate the pH of a solution that is 0.410 M in HOCl and 0.050M in NaOCl. Ka(HOCl)=3.0 x 10 -8
• A.

6.58

• B.

0.39

• C.

3.94

• D.

7.49

• 23.
What is the pH at the equilvalence point in the titration of 100 mL of 0.10M HCl with 0.10M NaOH?
• A.

1.0

• B.

6.0

• C.

7.0

• D.

13.0

• 24.
Which of these salts has the smallest molar solubility? Solid Ksp _________________________ CdS 3.6 x 10 -29 AgCl 2.0 x 10 -13 Ni(OH)2 2.8 x 10 -16 AgI 1.5 x 10 -16 PbS 8.4 x 10 -28
• A.

CdS

• B.

Ni(OH)2

• C.

AgCl

• D.

AgI

• 25.
What is the pH of a 0.20 M CH3COOH (acetic acid) solution? (Ka=1.8 x 10 -5)
• A.

X=[H+]=1.9x 10 -3--pH=-log{H+]=2.7

• B.

PH=107

• C.

PH=1.0

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