Question 1

The pOH of a solution is 10.40.Calculate the hydrogen ion concentration in the solution.

Accepted Answer

A) 4.0 * 10-11 M 
B) 3.6 M 
C) 4.0 * 10-10 M 
D) 2.5 * 10-4 M 
E) 1.8 * 10-4 M 
A) 4.0 * 10-11 M 
B) 3.6 M 
C) 4.0 * 10-10 M 
D) 2.5 * 10-4 M 
E) 1.8 * 10-4 M

Question 2

Identify the conjugate acid of CO32- in the reaction CO32- + H2PO4-   HCO3- + HPO42-

Accepted Answer

A) H2CO3 
B) HCO3- 
C) H2O 
D) HPO42- 
E) H2PO4- 
A) H2CO3 
B) HCO3- 
C) H2O 
D) HPO42- 
E) H2PO4-

Question 3

Which of the following yields an acidic solution when dissolved in water?

Accepted Answer

A) NO2 
B) LiOH 
C) K2O 
D) NaCl 
E) Ca(OH)2 
A) NO2 
B) LiOH 
C) K2O 
D) NaCl 
E) Ca(OH)2

Question 4

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.00 and 10.0 mL of a strong acid solution with pH = 6.00?

Accepted Answer

A) 2.0 
B) 2.3 
C) 4.0 
D) 6.0 
E) 8.0 
A) 2.0 
B) 2.3 
C) 4.0 
D) 6.0 
E) 8.0

Question 5

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 * 10-8 and Ka2 = 1 *10-19.Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Accepted Answer

A) 0.10 M 
B) 7.5 * 10-5 M 
C) 5.7 * 10-9 M 
D) 1 * 10-19 M 
E) 1 * 10-20 M 
A) 0.10 M 
B) 7.5 * 10-5 M 
C) 5.7 * 10-9 M 
D) 1 * 10-19 M 
E) 1 * 10-20 M

Question 6

Identify the conjugate base of HPO42- in the reaction HCO3- + HPO42-   H2CO3 + PO43-

Accepted Answer

A) H2O 
B) HCO3- 
C) H2CO3 
D) PO43- 
E) None of these. 
A) H2O 
B) HCO3- 
C) H2CO3 
D) PO43- 
E) None of these.

Question 7

What mass of ammonium chloride must be added to 250.mL of water to give a solution with pH = 4.85? [Kb(NH3)= 1.8 *10-5]

Accepted Answer

A) 4.7 g 
B) 75 g 
C) 2.3 * 10-3 g 
D) 19 g 
E) 10.g 
A) 4.7 g 
B) 75 g 
C) 2.3 * 10-3 g 
D) 19 g 
E) 10.g

Question 8

Write the formula for the conjugate base of H2PO4-.

Accepted Answer

Question 9

P4O10 is classified as an acidic oxide because it

Accepted Answer

A) reacts with acids to produce a salt. 
B) is insoluble in water. 
C) reacts with water to produce OH-. 
D) gives a solution of phosphoric acid, H3PO4, on dissolving in water. 
E) can act as a Lewis base by donating electron pairs. 
A) reacts with acids to produce a salt. 
B) is insoluble in water. 
C) reacts with water to produce OH-. 
D) gives a solution of phosphoric acid, H3PO4, on dissolving in water. 
E) can act as a Lewis base by donating electron pairs.

Question 10

Lime is used in farming to reduce the acidity of the soil. The chemical name for lime is calcium oxide. When water in the soil reacts with lime, what base is formed?

Accepted Answer

The answer of Lime is used in farming to reduce...

Question 11

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

Accepted Answer

A) 1.3 * 10-3 M 
B) 7.7 * 10-2 M 
C) 7.7 * 10-12 M 
D) 0.13 M 
E) 0.10 M 
A) 1.3 * 10-3 M 
B) 7.7 * 10-2 M 
C) 7.7 * 10-12 M 
D) 0.13 M 
E) 0.10 M

Question 12

In aqueous solutions at 25°C, the sum of the ion concentrations ([H+] + [OH -])equals
1 * 10 - 14.

Accepted Answer

A) True 
 B)False

Question 13

What is the pH of an aqueous solution that contains 5.3 *1017 OH- ions per liter of solution?

Accepted Answer

A) 5.30 
B) 6.06 
C) 7.94 
D) 8.70 
E) 11.3 
A) 5.30 
B) 6.06 
C) 7.94 
D) 8.70 
E) 11.3

Question 14

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

Accepted Answer

A) 2.9 * 10-2 M 
B) 5.7 * 10-2 M 
C) 1.3 * 10-3 M 
D) 2.9 * 10-3 M 
E) 5.7 * 10-4 M 
A) 2.9 * 10-2 M 
B) 5.7 * 10-2 M 
C) 1.3 * 10-3 M 
D) 2.9 * 10-3 M 
E) 5.7 * 10-4 M

Question 15

Write the chemical formula for nitric acid.

Accepted Answer

The answer of Write the chemical formula for nitric acid....

Question 16

Which of these acids is stronger, H3PO4 or H3AsO4?

Accepted Answer

Question 17

The pH of a sample of river water is 6.0. A sample of effluent from a food processing plant has a pH of 4.0. What is the ratio of hydronium ion concentration in the effluent to the hydronium ion concentration in the river?

Accepted Answer

The hydronium ion concentratio

Question 18

What is the pH of 10.0 mL of 0.0020 M HCl?

Accepted Answer

A) 0.70 
B) 2.70 
C) 3.70 
D) 5.70 
E) 10.0 
A) 0.70 
B) 2.70 
C) 3.70 
D) 5.70 
E) 10.0

Question 19

Which one of these salts will form a basic solution upon dissolving in water?

Accepted Answer

A) NaCl 
B) NaNO2 
C) NH4NO3 
D) KBr 
E) AlCl3 
A) NaCl 
B) NaNO2 
C) NH4NO3 
D) KBr 
E) AlCl3

Question 20

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000.mL of solution.

Accepted Answer

The answer of Calculate the pH of a solution containing...

Exam 15: Acids and Bases

The pOH of a solution is 10.40.Calculate the hydrogen ion concentration in the solution.

Identify the conjugate acid of CO32- in the reaction CO32- + H2PO4- HCO3- + HPO42-

Which of the following yields an acidic solution when dissolved in water?

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.00 and 10.0 mL of a strong acid solution with pH = 6.00?

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 * 10-8 and Ka2 = 1 *10-19.Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Identify the conjugate base of HPO42- in the reaction HCO3- + HPO42- H2CO3 + PO43-

What mass of ammonium chloride must be added to 250.mL of water to give a solution with pH = 4.85? [Kb(NH3)= 1.8 *10-5]

Write the formula for the conjugate base of H2PO4-.

P4O10 is classified as an acidic oxide because it

Lime is used in farming to reduce the acidity of the soil. The chemical name for lime is calcium oxide. When water in the soil reacts with lime, what base is formed?

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

In aqueous solutions at 25°C, the sum of the ion concentrations ([H+] + [OH -])equals 1 * 10 - 14.

What is the pH of an aqueous solution that contains 5.3 *1017 OH- ions per liter of solution?

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

Write the chemical formula for nitric acid.

Which of these acids is stronger, H3PO4 or H3AsO4?

The pH of a sample of river water is 6.0. A sample of effluent from a food processing plant has a pH of 4.0. What is the ratio of hydronium ion concentration in the effluent to the hydronium ion concentration in the river?

What is the pH of 10.0 mL of 0.0020 M HCl?

Which one of these salts will form a basic solution upon dissolving in water?

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000.mL of solution.

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

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Filters

Identify the conjugate acid of CO₃^2- in the reaction CO₃^2- + H₂PO₄^- HCO₃^- + HPO₄^2-

Hydrosulfuric acid is a diprotic acid, for which K_a1 = 5.7 * 10^-8 andK_a2 = 1 *10^-19.Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Identify the conjugate base of HPO₄^2- in the reaction HCO₃^- + HPO₄^2- H₂CO₃ + PO₄^3-

What mass of ammonium chloride must be added to 250.mL of water to give a solution with pH = 4.85? [K_b(NH₃)= 1.8 *10^-5]

Write the formula for the conjugate base of H₂PO₄^-.

P₄O₁₀ is classified as an acidic oxide because it

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

In aqueous solutions at 25°C, the sum of the ion concentrations ([H⁺] + [OH^-])equals 1 * 10^{- 14}.

What is the pH of an aqueous solution that contains 5.3 *10¹⁷ OH^- ions per liter of solution?

Which of these acids is stronger, H₃PO₄ or H₃AsO₄?