Question 1

What is the pH of a solution prepared by dissolving 0.30 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) 2.27 
B) 2.57 
C) 11.42 
D) 11.73

Question 2

At 50°C the value of K_w is 5.5 × 10^-14,and the pH of a neutral solution at 50°C is ________.

Accepted Answer

The answer of At 50°C the value of K_w is...

Question 3

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. 
-Arrange the three acids in order of increasing acid strength.

Accepted Answer

A) HZ < HY < HX 
B) HY < HZ < HX 
C) HZ < HX < HY 
D) HX < HZ < HY

Question 4

A 0.50 M KNO₂ solution will have a pH ________ seven.

Accepted Answer

The answer of A 0.50 M KNO₂ solution will have...

Question 5

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 6

Calculate the pH of a 0.20 M H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.

Accepted Answer

A) 1.26 
B) 1.32 
C) 1.82 
D) 2.52

Question 7

What is the pH of a 0.020 M Ba(OH)2 solution?

Accepted Answer

A) 1.40 
B) 1.70 
C) 12.30 
D) 12.60

Question 8

What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq).

Accepted Answer

A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38

Question 9

The acid strength of an oxoacid having the general formula H_nYO_m increases as the electronegativity of Y ________ and as the oxidation number of Y ________.

Accepted Answer

The answer of The acid strength of an oxoacid having...

Question 10

What is the hydroxide ion concentration of a lye solution that has a pH of 13.20?

Accepted Answer

A) 6.31 × 10-14 M 
B) 1.58 × 10-1 M 
C) 0.80 M 
D) 13.20 M

Question 11

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 12

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest). HNO3(aq)+ H2O(l)→ H3O+(aq)+ NO3-(aq)
HF(aq)+ H2O(l)⇌ H3O+(aq)+ F-(aq)

Accepted Answer

A) HNO3 > H3O+ > HF 
B) NO3- > H2O > F- 
C) F- > H2O > NO3- 
D) F- > NO3- > H2O

Question 13

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-5 M in hydronium ion.

Accepted Answer

A) 2.86 × 10-2 M 
B) 2.86 × 10-9 M 
C) 2.86 × 10-10 M 
D) 3.50 × 10-10 M

Question 14

A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC9H7O4)was dissolved in enough water to make 100 mL of solution.Given that Ka = 3.0 × 10-4 for aspirin,what is the pH of the solution?

Accepted Answer

A) 1.57 
B) 2.54 
C) 3.52 
D) 5.08

Question 15

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 16

A 0.050 M solution of hydroxylamine,NH₂OH,having K_b = 9.1 × 10^-9 has a pH of ________.

Accepted Answer

The answer of A 0.050 M solution of hydroxylamine,NH₂OH,having K_b...

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

Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87.Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is CH3COOH(aq)+ H2O(l)⇌ H3O+(aq)+ CH3CO2-(aq).

Accepted Answer

A) 1.3 × 10-2 
B) 1.3 × 10-3 
C) 1.8 × 10-5 
D) 1.8 × 10-6

Question 19

Calculate the pH for an aqueous solution of acetic acid that contains  hydronium ion.

Accepted Answer

A) 2.41 × 10-12 M 
B) 4.15 × 10-3 M 
C) 2.38 
D) 11.62

Question 20

What is the approximate pH of a solution X that gives the following responses with the indicators shown?

Accepted Answer

A) 3.2 - 4.4 
B) 4.8 - 6.0 
C) 6.0 - 7.6 
D) 8.2 - 10.0

Exam 15: Aqueous Equilibria: Acids and Bases

What is the pH of a solution prepared by dissolving 0.30 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)

At 50°C the value of K_w is 5.5 × 10^-14,and the pH of a neutral solution at 50°C is ________.

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z) ;water molecules have been omitted for clarity. -Arrange the three acids in order of increasing acid strength.

A 0.50 M KNO₂ solution will have a pH ________ seven.

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)

Calculate the pH of a 0.20 M H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and K_a2 = 6.3 × 10^-8.

What is the pH of a 0.020 M Ba(OH) ₂ solution?

What is the pH of a 0.30 M pyridine solution that has a K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is C₅H₅N(aq) + H₂O(l) ⇌ C₅H₅NH⁺(aq) + OH^-(aq) .

The acid strength of an oxoacid having the general formula H_nYO_m increases as the electronegativity of Y and as the oxidation number of Y .

What is the hydroxide ion concentration of a lye solution that has a pH of 13.20?

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.

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest) . HNO₃(aq) + H₂O(l) → H₃O⁺(aq) + NO₃^-(aq) HF(aq) + H₂O(l) ⇌ H₃O⁺(aq) + F^-(aq)

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-5 M in hydronium ion.

A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC₉H₇O₄) was dissolved in enough water to make 100 mL of solution.Given that K_a = 3.0 × 10^-4 for aspirin,what is the pH of the solution?

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).

A 0.050 M solution of hydroxylamine,NH₂OH,having K_b = 9.1 × 10^-9 has a pH of ________.

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.

Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87.Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is CH₃COOH(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CH₃CO₂^-(aq) .

Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion.

What is the approximate pH of a solution X that gives the following responses with the indicators shown?

Exam 15: Aqueous Equilibria: Acids and Bases

What is the pH of a solution prepared by dissolving 0.30 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)

At 50°C the value of Kw is 5.5 × 10-14,and the pH of a neutral solution at 50°C is ________.

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z) ;water molecules have been omitted for clarity. -Arrange the three acids in order of increasing acid strength.

A 0.50 M KNO2 solution will have a pH ________ seven.

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)

Calculate the pH of a 0.20 M H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.

What is the pH of a 0.020 M Ba(OH) 2 solution?

What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH-(aq) .

The acid strength of an oxoacid having the general formula HnYOm increases as the electronegativity of Y ________ and as the oxidation number of Y ________.

What is the hydroxide ion concentration of a lye solution that has a pH of 13.20?

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.

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest) . HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq) HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-5 M in hydronium ion.

A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC9H7O4) was dissolved in enough water to make 100 mL of solution.Given that Ka = 3.0 × 10-4 for aspirin,what is the pH of the solution?

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).

A 0.050 M solution of hydroxylamine,NH2OH,having Kb = 9.1 × 10-9 has a pH of ________.

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.

Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87.Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is CH3COOH(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq) .

Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion.

What is the approximate pH of a solution X that gives the following responses with the indicators shown?

What is the pH of a solution prepared by dissolving 0.30 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)

At 50°C the value of K_w is 5.5 × 10^-14,and the pH of a neutral solution at 50°C is ________.

A 0.50 M KNO₂ solution will have a pH ________ seven.

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)

Calculate the pH of a 0.20 M H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and K_a2 = 6.3 × 10^-8.

What is the pH of a 0.020 M Ba(OH) ₂ solution?

What is the pH of a 0.30 M pyridine solution that has a K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is C₅H₅N(aq) + H₂O(l) ⇌ C₅H₅NH⁺(aq) + OH^-(aq) .

The acid strength of an oxoacid having the general formula H_nYO_m increases as the electronegativity of Y and as the oxidation number of Y .

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.

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest) . HNO₃(aq) + H₂O(l) → H₃O⁺(aq) + NO₃^-(aq) HF(aq) + H₂O(l) ⇌ H₃O⁺(aq) + F^-(aq)

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-5 M in hydronium ion.

A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC₉H₇O₄) was dissolved in enough water to make 100 mL of solution.Given that K_a = 3.0 × 10^-4 for aspirin,what is the pH of the solution?

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).

A 0.050 M solution of hydroxylamine,NH₂OH,having K_b = 9.1 × 10^-9 has a pH of ________.

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.

Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87.Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is CH₃COOH(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CH₃CO₂^-(aq) .