Question 1

When dissolved in water,which of the following compounds is an Arrhenius acid?

Accepted Answer

A) HCN 
B) NaOH 
C) NaF 
D) CH3CH2OH

Question 2

What is the pH of a 0.020 M RbOH solution?

Accepted Answer

A) 0)020 
B) 0)040 
C) 1)70 
D) 12.30

Question 3

What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?

Accepted Answer

A) 1)00 
B) 1)60 
C) 2)00 
D) 3)20

Question 4

In order for the reaction A^- + H₂CO₃ ⇌ HA + HCO₃^- to have an equilibrium constant K_c < 1,the K_a of HA must be ________ (greater,less)than the K_a of H₂CO₃.

Accepted Answer

The answer of In order for the reaction A^- +...

Question 5

What is the pH of a solution prepared by dissolving 0.45 grams of solid CaO (lime)in enough water to make 2.00 L of aqueous Ca(OH)2 (limewater)?
CaO(s)+ H2O(l)→ Ca2+(aq)+ 2 OH-(aq)

Accepted Answer

A) 2)10 
B) 2)40 
C) 11.60 
D) 11.90

Question 6

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 6)6 × 10-5 M 
B) 4)3 × 10-7 M 
C) 4)3 × 10-9 M 
D) 5)6 × 10-11 M

Question 7

Undersea flora prefer a maximum concentration of OH^- of 1.58 × 10^-5.The concentration of H₃O⁺ in the seawater is ________,and this solution is ________ (acidic,basic,neutral).

Accepted Answer

The answer of Undersea flora prefer a maximum concentration of...

Question 8

Normal rainfall has a concentration of OH- that is 3.98 × 10-9.The concentration of H3O+ in normal rainfall is

Accepted Answer

A) greater than 3.98 × 10-9,and the rain is acidic. 
B) greater than 3.98 × 10-9,and the rain is basic. 
C) less than 3.98 × 10-9,and the rain is acidic. 
D) less than 3.98 × 10-9,and the rain is basic.

Question 9

BF3 and NH3 undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

Accepted Answer

A) Picture (1)is correct;NH3 is the Lewis acid and BF3 is the Lewis base. 
B) Picture (2)is correct;BF3 is the Lewis acid and NH3 is the Lewis base. 
C) Picture (3)is correct;NH3 is the Lewis acid and BF3 is the Lewis base. 
D) Picture (4)is correct;BF3 is the Lewis acid and NH3 is the Lewis base.

Question 10

A 0.10 M KNO₂ solution will have a pH ________ seven.

Accepted Answer

The answer of A 0.10 M KNO₂ solution will have...

Question 11

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A) NaHSO4 
B) LiClO4 
C) MgO 
D) CH3NH3I

Question 12

A solution with a hydrogen ion concentration of 3.25 × 10- 6 M is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A) acidic,3.08 × 10- 8 M 
B) acidic,3.08 × 10- 9 M 
C) basic,3.08 × 10- 8 M 
D) basic,3.08 × 10- 9 M

Question 13

Potassium hydrogen phthalate (molar mass = 204.2 g/mol)is one of the most commonly used acids for standardizing solutions containing bases.KHP is a monoprotic weak acid with Ka = 3.91 × 10-6.Calculate the pH of the solution that results when 0.50 g of KHP is dissolved in enough water to produce 25.0 mL of solution.

Accepted Answer

A) 2)05 
B) 3)21 
C) 4)40 
D) 5)41

Question 14

In the following reaction the unshaded spheres represent H atoms. 
-Identify the Br∅nsted-Lowry acid/base conjugate pairs.

Accepted Answer

A) (1)/(2)and (3)/(4) 
B) (1)/(3)and (2)/(4) 
C) (1)/(4)and (2)/(3)

Question 15

CO2 reacts with H2O to form HCO3- and H+.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base? 
(1)(2)

Accepted Answer

A) Picture (1)is correct;H2O is the Lewis acid and CO2 is the Lewis base. 
B) Picture (1)is correct;CO2 is the Lewis acid and H2O is the Lewis base. 
C) Picture (2)is correct;H2O is the Lewis acid and CO2 is the Lewis base. 
D) Picture (2)is correct;CO2 is the Lewis acid and H2O is the Lewis base.

Question 16

One way to prepare a solution with a pH of 10.00 is to dissolve ________ grams of CaO in enough water to make 500 mL of solution.

Accepted Answer

The answer of One way to prepare a solution with...

Question 17

Erythromycin is a basic antimicrobial with pK_b = 5.2.A 1.0 × 10^-3 M solution of erythromycin has a pH of and a percent ionization.

Accepted Answer

The answer of Erythromycin is a basic antimicrobial with pK_b...

Question 18

The percent dissociation of acetic acid changes as the concentration of the acid decreases.A 100-fold decrease in acetic acid concentration results in a ________ fold ________ in the percent dissociation.

Accepted Answer

A) 10,increase 
B) 10,decrease 
C) 100,increase 
D) 100,decrease

Question 19

What is the strongest acid among the following?

Accepted Answer

A) H2SO3 
B) H2SO4 
C) H2SeO3 
D) H2SeO4

Question 20

Calculate the pH of a 0.100 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7 × 10-4.

Accepted Answer

A) 2)22 
B) 5)78 
C) 8)22 
D) 11.78

Exam 14: Aqueous Equilibria: Acids and Bases

When dissolved in water,which of the following compounds is an Arrhenius acid?

What is the pH of a 0.020 M RbOH solution?

What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?

In order for the reaction A^- + H₂CO₃ ⇌ HA + HCO₃^- to have an equilibrium constant K_c < 1,the K_a of HA must be ________ (greater,less)than the K_a of H₂CO₃.

What is the pH of a solution prepared by dissolving 0.45 grams of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH) ₂ (limewater) ? CaO(s) + H₂O(l) → Ca²⁺(aq) + 2 OH^-(aq)

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.010 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Undersea flora prefer a maximum concentration of OH^- of 1.58 × 10^-5.The concentration of H₃O⁺ in the seawater is ,and this solution is (acidic,basic,neutral).

Normal rainfall has a concentration of OH^- that is 3.98 × 10^-9.The concentration of H₃O⁺ in normal rainfall is

BF₃ and NH₃ undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

A 0.10 M KNO₂ solution will have a pH ________ seven.

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

A solution with a hydrogen ion concentration of 3.25 × 10^{- 6} M is and has a hydroxide ion concentration of .

In the following reaction the unshaded spheres represent H atoms. -Identify the Br∅nsted-Lowry acid/base conjugate pairs.

CO₂ reacts with H₂O to form HCO₃^- and H⁺.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base? (1) (2)

One way to prepare a solution with a pH of 10.00 is to dissolve ________ grams of CaO in enough water to make 500 mL of solution.

Erythromycin is a basic antimicrobial with pK_b = 5.2.A 1.0 × 10^-3 M solution of erythromycin has a pH of and a percent ionization.

The percent dissociation of acetic acid changes as the concentration of the acid decreases.A 100-fold decrease in acetic acid concentration results in a fold in the percent dissociation.

What is the strongest acid among the following?

Calculate the pH of a 0.100 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7 × 10^-4.

Exam 14: Aqueous Equilibria: Acids and Bases

When dissolved in water,which of the following compounds is an Arrhenius acid?

What is the pH of a 0.020 M RbOH solution?

What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?

In order for the reaction A- + H2CO3 ⇌ HA + HCO3- to have an equilibrium constant Kc < 1,the Ka of HA must be ________ (greater,less)than the Ka of H2CO3.

What is the pH of a solution prepared by dissolving 0.45 grams of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH) 2 (limewater) ? CaO(s) + H2O(l) → Ca2+(aq) + 2 OH-(aq)

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Undersea flora prefer a maximum concentration of OH- of 1.58 × 10-5.The concentration of H3O+ in the seawater is ________,and this solution is ________ (acidic,basic,neutral).

Normal rainfall has a concentration of OH- that is 3.98 × 10-9.The concentration of H3O+ in normal rainfall is

BF3 and NH3 undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

A 0.10 M KNO2 solution will have a pH ________ seven.

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

A solution with a hydrogen ion concentration of 3.25 × 10- 6 M is ________ and has a hydroxide ion concentration of ________.

In the following reaction the unshaded spheres represent H atoms. -Identify the Br∅nsted-Lowry acid/base conjugate pairs.

CO2 reacts with H2O to form HCO3- and H+.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base? (1) (2)

One way to prepare a solution with a pH of 10.00 is to dissolve ________ grams of CaO in enough water to make 500 mL of solution.

Erythromycin is a basic antimicrobial with pKb = 5.2.A 1.0 × 10-3 M solution of erythromycin has a pH of and a percent ionization.

The percent dissociation of acetic acid changes as the concentration of the acid decreases.A 100-fold decrease in acetic acid concentration results in a ________ fold ________ in the percent dissociation.

What is the strongest acid among the following?

Calculate the pH of a 0.100 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7 × 10-4.

In order for the reaction A^- + H₂CO₃ ⇌ HA + HCO₃^- to have an equilibrium constant K_c < 1,the K_a of HA must be ________ (greater,less)than the K_a of H₂CO₃.

What is the pH of a solution prepared by dissolving 0.45 grams of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH) ₂ (limewater) ? CaO(s) + H₂O(l) → Ca²⁺(aq) + 2 OH^-(aq)

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.010 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Undersea flora prefer a maximum concentration of OH^- of 1.58 × 10^-5.The concentration of H₃O⁺ in the seawater is ,and this solution is (acidic,basic,neutral).

Normal rainfall has a concentration of OH^- that is 3.98 × 10^-9.The concentration of H₃O⁺ in normal rainfall is

BF₃ and NH₃ undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

A 0.10 M KNO₂ solution will have a pH ________ seven.

A solution with a hydrogen ion concentration of 3.25 × 10^{- 6} M is and has a hydroxide ion concentration of .

CO₂ reacts with H₂O to form HCO₃^- and H⁺.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base? (1) (2)

Erythromycin is a basic antimicrobial with pK_b = 5.2.A 1.0 × 10^-3 M solution of erythromycin has a pH of and a percent ionization.

The percent dissociation of acetic acid changes as the concentration of the acid decreases.A 100-fold decrease in acetic acid concentration results in a fold in the percent dissociation.

Calculate the pH of a 0.100 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7 × 10^-4.