Question 1

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. 
-Which point a-d represents the equivalence point for the titration of a strong acid?

Accepted Answer

A) point a 
B) point b 
C) point c 
D) point d

Question 2

What is the molar solubility of AgCl in 0.30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3)2+ is 1.7 × 107.

Accepted Answer

A) 1.3 × 10-5 M 
B) 1.5 × 10-2 M 
C) 1.7 × 10-2 M 
D) 5.5 × 10-2 M

Question 3

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A+ with NaOH.Which point a-d represents the isoelectric point?

Accepted Answer

A) point a 
B) point b 
C) point c 
D) point d

Question 4

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.24? Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A) 0.31:1 
B) 0.89:1 
C) 1.1:1 
D) 3.2:1

Question 5

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pKa = 4.10?

Accepted Answer

A) 96% 
B) 10% 
C) 5% 
D) 1%

Question 6

What is the pH at the first equivalence point?

Accepted Answer

A) pH = pKa1 
B) pH = 14 - pKa1 
C) pH = (pKa1 + pKa2)/2 
D) pH = pKa1 + pKa2

Question 7

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. 
-Which point a-d represents the equivalence point for the titration of a weak acid?

Accepted Answer

A) point a 
B) point b 
C) point c 
D) point d

Question 8

What is the approximate value of the equilibrium constant,Kn,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HBr(aq)+ LiOH(aq)⇌ H2O(l)+ LiBr(aq)

Accepted Answer

A) 1.0 × 102 
B) 1.0 × 107 
C) 1.0 × 1014 
D) 1.0 × 1028

Question 9

A solution may contain the following ions Ag+,Cu2+,Cd2+,Mn2+,Ni2+ and Na+.A white precipitate formed when 0.10 M NaCl was added and after this was removed the solution was treated with H2S gas under acidic conditions and no precipitate formed.When the solution was made basic and again treated with H2S gas a dark colored precipitate formed.If no further tests were made then what conclusions can you draw?

Accepted Answer

A) possible ions present Ag+,Mn2+,Ni2+ 
B) possible ions present Ag+,Mn2+,Ni2+,Na+ 
C) possible ions present Ag+,Cu2+,Cd2+ 
D) possible ions present Ag+,Cu2+,Cd2+,Na+

Question 10

The pH of a 0.150 M formic acid/0.250 M sodium formate buffer = ________? The K_a of formic acid is 1.8 × 10^-4.

Accepted Answer

The answer of The pH of a 0.150 M formic...

Question 11

The half equivalence point in the titration of 0.100 M HCO₂H (K_a = 1.8 × 10^-4)with 0.250 M NaOH occurs at pH = ________.

Accepted Answer

The answer of The half equivalence point in the titration...

Question 12

Which of the following metal hydroxides are amphoteric?

Accepted Answer

A) Al(OH)3,Zn(OH)2,Cr(OH)3,Sn(OH)2 
B) Cu(OH)2,Mn(OH)2,Fe(OH)2,Fe(OH)3 
C) Be(OH)2,Ca(OH)2,Ba(OH)2,Sr(OH)3 
D) LiOH,NaOH,KOH,RbOH

Question 13

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? Ka = 1.8 × 10-4 for formic acid.

Accepted Answer

A) 2.46 
B) 5.88 
C) 8.12 
D) 11.54

Question 14

Which of the following titrations result in a basic solution at the equivalence point?

Accepted Answer

A) HCl titrated with LiCH3CO2 
B) HOCl titrated with KOH 
C) HI titrated with LiOH 
D) Pb(NO3)2 titrated with NaI

Question 15

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH. 
-Which point a-d represents the H2X/HX- buffer region?

Accepted Answer

A) point a 
B) point b 
C) point c 
D) point d

Question 16

A solution may contain the following ions Ag+,Cu2+,Mn2+,Ca2+,and Na+.No precipitate formed when 0.10 M NaCl was added but a dark colored precipitate formed when H2S was added to an acidic portion of the solution.After the removal of the solid the solution was made basic and more H2S was added and a dark precipitate again formed.Treatment of the filtrate with (NH4)2CO3 resulted in a white precipitate.If no further tests were made then what conclusions can you draw?

Accepted Answer

A) possible ions present Cu2+,Mn2+,Na+ 
B) possible ions present Cu2+,Mn2+,Ca2+ 
C) possible ions present Cu2+,Mn2+,Ca2+,Na+ 
D) possible ions present Ag+,Cu2+,Mn2+,Ca2+,Na+

Question 17

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. ) 
-For which solution(s)is pH = pKa?

Accepted Answer

A) only solution (1) 
B) only solution (2) 
C) only solution (3) 
D) solutions (1)and (3)

Question 18

What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

Accepted Answer

The answer of What is the K_a of the amino...

Question 19

The following pictures represent solutions of AgCl,which may also contain ions other than AgS1U1P1+S1S1P0 and ClS1U1P1-S1S1P0 which are not shown.Gray spheres represent AgS1U1P1+S1S1P0 ions and dotted spheres represent ClS1U1P1-S1S1P0 ions. 
-If solution (1)is a saturated solution of AgCl,which of solutions (1)-(4)represents the solution after a small amount of AgNO3 is added and equilibrium is restored?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 20

The following pictures represent solutions at various stages in the titration of a weak diprotic acid HS1U1B12S1U1B0A with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P12-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0 initially present,OHS1U1P1-S1S1P0 initially present and solvent water molecules have been omitted for clarity). 
-Which picture represents the system with the highest pH?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4)

Exam 16: Applications of Aqueous Equilibria

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which point a-d represents the equivalence point for the titration of a strong acid?

What is the molar solubility of AgCl in 0.30 M NH₃? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(NH₃) ₂⁺ is 1.7 × 10⁷.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A⁺ with NaOH.Which point a-d represents the isoelectric point?

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.24? K_a = 1.8 × 10^-5for CH₃CO₂H.

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pK_a = 4.10?

What is the pH at the first equivalence point?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which point a-d represents the equivalence point for the titration of a weak acid?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HBr(aq) + LiOH(aq) ⇌ H₂O(l) + LiBr(aq)

The pH of a 0.150 M formic acid/0.250 M sodium formate buffer = ________? The K_a of formic acid is 1.8 × 10^-4.

The half equivalence point in the titration of 0.100 M HCO₂H (K_a = 1.8 × 10^-4)with 0.250 M NaOH occurs at pH = ________.

Which of the following metal hydroxides are amphoteric?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? K_a = 1.8 × 10^-4for formic acid.

Which of the following titrations result in a basic solution at the equivalence point?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the H₂X/HX^- buffer region?

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -For which solution(s) is pH = pK_a?

What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

Exam 16: Applications of Aqueous Equilibria

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which point a-d represents the equivalence point for the titration of a strong acid?

What is the molar solubility of AgCl in 0.30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3) 2+ is 1.7 × 107.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A+ with NaOH.Which point a-d represents the isoelectric point?

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.24? Ka = 1.8 × 10-5 for CH3CO2H.

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pKa = 4.10?

What is the pH at the first equivalence point?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which point a-d represents the equivalence point for the titration of a weak acid?

What is the approximate value of the equilibrium constant,Kn,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HBr(aq) + LiOH(aq) ⇌ H2O(l) + LiBr(aq)

The pH of a 0.150 M formic acid/0.250 M sodium formate buffer = ________? The Ka of formic acid is 1.8 × 10-4.

The half equivalence point in the titration of 0.100 M HCO2H (Ka = 1.8 × 10-4)with 0.250 M NaOH occurs at pH = ________.

Which of the following metal hydroxides are amphoteric?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? Ka = 1.8 × 10-4 for formic acid.

Which of the following titrations result in a basic solution at the equivalence point?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -Which point a-d represents the H2X/HX- buffer region?

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A- ions.(K+,H3O+,OH-,and solvent H2O molecules have been omitted for clarity. ) -For which solution(s) is pH = pKa?

What is the Ka of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

What is the molar solubility of AgCl in 0.30 M NH₃? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(NH₃) ₂⁺ is 1.7 × 10⁷.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A⁺ with NaOH.Which point a-d represents the isoelectric point?

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.24? K_a = 1.8 × 10^-5for CH₃CO₂H.

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pK_a = 4.10?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HBr(aq) + LiOH(aq) ⇌ H₂O(l) + LiBr(aq)

The pH of a 0.150 M formic acid/0.250 M sodium formate buffer = ________? The K_a of formic acid is 1.8 × 10^-4.

The half equivalence point in the titration of 0.100 M HCO₂H (K_a = 1.8 × 10^-4)with 0.250 M NaOH occurs at pH = ________.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? K_a = 1.8 × 10^-4for formic acid.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the H₂X/HX^- buffer region?

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -For which solution(s) is pH = pK_a?

What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?