Question 1

A 200-mL solution contains 0.018 mol each of I-, Br-, and Cl-. When the solution is mixed with 200 mL of 0.24 M AgNO3, how much AgCl(s)  precipitates out? -, Br-, and Cl-. When the solution is mixed with 200 mL of 0.24 M AgNO3, how much AgCl(s)  precipitates out?   A)  2.6 g B)  0.0 g C)  3.3 g D)  5.0 g E)  1.7 g" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   2.6 g
B)   0.0 g
C)   3.3 g
D)   5.0 g
E)   1.7 gF) C) and D)
G) A) and E)

Question 2

Differentiate between the equivalence point and the endpoint in an acid-base titration.

Accepted Answer

See Sectio...

Question 3

Calculate the concentration of [H+] of a buffered solution containing 5.0 × 10−4 M HCN (Ka = 6.2 × 10−10)  and 1.5 × 10−4 M NaCN.

Accepted Answer

A)   3.06 × 10−9 M​
B)   ​0.22 × 10−9 M
C)   2.07 × 10−9 M
D)   4.12 × 10−9 M
E)   4.58 × 10−9 MF) A) and E)
G) None of the above

Question 4

You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00 × 10-4) . A buffer of pH 3.000 is needed. What volumes of HNO2 and KNO2 are required to make 1 L of buffered solution?

Accepted Answer

A)   286 mL HNO2; 714 mL KNO2
B)   714 mL HNO2; 286 mL KNO2
C)   413 mL HNO2; 587 mL KNO2
D)   500 mL of each
E)   587 mL HNO2; 413 mL KNO2F) None of the above
G) A) and B)

Question 5

In the titration of 100.0 mL of a 0.200 M solution of H2A (Ka1 = 1.0 × 10-5, Ka2 = 1.0 × 10-8) , what volume of 0.400 M NaOH must be added to reach a pH of 5.00?

Accepted Answer

A)   25.0 mL
B)   100.0 mL
C)   0 mL
D)   150.0 mL
E)   50.0 mLF) A) and B)
G) D) and E)

Question 6

A 200.0-mL sample of the weak acid H3A (0.100 M)  is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) 
-After 300.0 mL of 0.200 M NaOH is added

Accepted Answer

A)   A3-
B)   OH-, A3-
C)   H3A, H2A-, HA2-, A3-
D)   H2A-, OH-
E)   OH-, HA2-, A3-F) A) and B)
G) A) and C)

Question 7

Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8 × 10-10)  with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

Accepted Answer

A)   8.70
B)   2.68
C)   11.62
D)   -0.85
E)   none of theseF) D) and E)
G) A) and D)

Question 8

The contents of the flask are transferred quantitatively to a 2L volumetric. 100ml of 1 M HCL is added and the flask filled to the mark with water. There is still observable solid calcium hydroxide in the bottom of the new flask. What is the pH of this solution?

Accepted Answer

A)   2.94
B)   12.14
C)   2.16
D)   7.00
E)   11.83F) B) and D)
G) All of the above

Question 9

One milliliter (1.00 mL)  of acid taken from a lead storage battery is pipetted into a flask. Water and phenolphthalein indicator are added, and the solution is titrated with 0.38 M NaOH until a pink color appears; 15.8 mL is required. Find, to within 5%, the number of grams of H2SO4 (formula weight = 98)  present in 1 L of the battery acid.

Accepted Answer

A)   480 g
B)   240 g
C)   580 g
D)   290 g
E)   750 gF) B) and D)
G) A) and B)

Question 10

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10)  is titrated with the following volumes of 1.00 M NaOH.
-0 mL of 1.00 M NaOH

Accepted Answer

A)   3.00
B)   6.00
C)   0
D)   3.35
E)   none of theseF) B) and E)
G) C) and E)

Question 11

A 50.00-mL sample of 0.100 M Ca(NO3) 2 is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0 × 10-11. 3) 2 is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0 × 10-11.   A)  10.0 × 10-3 1.3 × 10-5 M 1.3 × 10-5 M B)  5.0 × 10-3 3.5 × 10-4 M 7.0 × 10-4 M C)  5.0 × 10-3 2.2 × 10-4 M 4.3 × 10-4 M D)  5.0 × 10-3 3.5 × 10-4 M 4.3 × 10-4 M E)  5.0 × 10-3 3.4 × 10-9 M 5.0 × 10-2 M" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   10.0 × 10-3 1.3 × 10-5 M 1.3 × 10-5 M
B)   5.0 × 10-3 3.5 × 10-4 M 7.0 × 10-4 M
C)   5.0 × 10-3 2.2 × 10-4 M 4.3 × 10-4 M
D)   5.0 × 10-3 3.5 × 10-4 M 4.3 × 10-4 M
E)   5.0 × 10-3 3.4 × 10-9 M 5.0 × 10-2 MF) A) and B)
G) None of the above

Question 12

A titration of 100.0 mL of 1.00 M malonic acid (H2A)  was done with 1.00 M NaOH. For malonic acid, Ka1 = 1.49 × 10-2, Ka2 = 2.03 × 10-6.
-Calculate [H+] after 300.0 mL of 1.00 M NaOH has been added.

Accepted Answer

A)   1.00 × 10-7 M
B)   4.00 × 10-14 M
C)   1.41 × 10-10 M
D)   1.00 M
E)   none of theseF) D) and E)
G) B) and E)

Question 13

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10)  is titrated with the following volumes of 1.00 M NaOH.
-300.0 mL of 1.00 M NaOH

Accepted Answer

A)   10.00
B)   11.21
C)   9.50
D)   9.30
E)   none of theseF) None of the above
G) A) and C)

Question 14

Consider the following information about the diprotic acid ascorbic acid (H2As for short, molar mass = 176.1) . 2As for short, molar mass = 176.1) .   The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below:   -What is the pH at point I (V1/2 HCl added) ? A)  7.95 B)  12.39 C)  10 D)  11.79 E)  none of these " class="answers-bank-image d-inline" rel="preload" > The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below: 2As for short, molar mass = 176.1) .   The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below:   -What is the pH at point I (V1/2 HCl added) ? A)  7.95 B)  12.39 C)  10 D)  11.79 E)  none of these " class="answers-bank-image d-inline" rel="preload" >
-What is the pH at point I (V1/2 HCl added) ?

Accepted Answer

A)   7.95
B)   12.39
C)   10
D)   11.79
E)   none of theseF) C) and E)
G) A) and E)

Question 15

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10)  is titrated with the following volumes of 1.00 M NaOH.
-200.0 mL of 1.00 M NaOH

Accepted Answer

A)   9.50
B)   6.48
C)   6.00
D)   8.00
E)   none of theseF) B) and D)
G) A) and D)

Question 16

What is the molarity of a sodium hydroxide solution if 25.0 mL of this solution reacts exactly with 22.30 mL of 0.253 M sulfuric acid?

Accepted Answer

A)   0.284 M
B)   0.451 M
C)   0.567 M
D)   0.226 M
E)   0.113 MF) A) and B)
G) A) and C)

Question 17

A 0.012-mol sample of Na2SO4 is added to 400 mL of each of two solutions. One solution contains 1.5 × 10-3 M BaCl2; the other contains 1.5 × 10-3 M CaCl2. Ksp for BaSO4 = 1.5 × 10-9 and Ksp for CaSO4 = 6.1 × 10-5. Which of the following statements is true?

Accepted Answer

A)   Both BaSO4 and CaSO4 would precipitate.
B)   Not enough information is given to determine whether precipitation would occur.
C)   CaSO4 would precipitate but BaSO4 would not.
D)   BaSO4 would precipitate but CaSO4 would not.
E)   Neither BaSO4 nor CaSO4 would precipitate.F) D) and E)
G) A) and B)

Question 18

Which of the following salts shows the lowest solubility in water? Ksp values are as follows:
Ag2S = 1.6 × 10-49; Bi2S3 = 1.0 × 10-72; HgS = 1.6 × 10-54; Mg(OH) 2 = 8.9 × 10-12; MnS = 2.3 × 10-13)

Accepted Answer

A)   HgS
B)   MnS
C)   Bi2S3
D)   Ag2S
E)   Mg(OH) 2F) A) and D)
G) B) and C)

Question 19

A 50.0-mL sample of 2.0 × 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN) 32-: -4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN) 32-:   Calculate the solubility of CuBr(s)  (Ksp = 1.0 × 10-5)  in 1.0 L of 1.0 M NaCN. A)  0.33 mol/L B)  1.0 × 10-6 mol/L C)  1.0 × 103 mol/L D)  1.0 mol/L E)  none of these" class="answers-bank-image d-inline" rel="preload" > Calculate the solubility of CuBr(s)  (Ksp = 1.0 × 10-5)  in 1.0 L of 1.0 M NaCN.

Accepted Answer

A)   0.33 mol/L
B)   1.0 × 10-6 mol/L
C)   1.0 × 103 mol/L
D)   1.0 mol/L
E)   none of theseF) A) and C)
G) A) and D)

Question 20

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH+. Which statement is true?

Accepted Answer

A)   The pH and the pOH remain unchanged.
B)   The pH and the pOH both decrease.
C)   The pH and the pOH both increase.
D)   The pH increases and pOH decreases.
E)   The pH decreases and the pOH increases.F) A) and B)
G) A) and C)

Exam 8: Applications of Aqueous Equilibria

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -200.0 mL of 1.00 M NaOH

Correct Answer
verified

What is the molarity of a sodium hydroxide solution if 25.0 mL of this solution reacts exactly with 22.30 mL of 0.253 M sulfuric acid?

Correct Answer
verified

Correct Answer
verified

Which of the following salts shows the lowest solubility in water? K_sp values are as follows: Ag₂S = 1.6 × 10^-49; Bi₂S₃ = 1.0 × 10^-72; HgS = 1.6 × 10^-54; Mg(OH) ₂ = 8.9 × 10^-12; MnS = 2.3 × 10^-13)

Correct Answer
verified

A 0.012-mol sample of Na₂SO₄ is added to 400 mL of each of two solutions. One solution contains 1.5 × 10^-3 M BaCl₂; the other contains 1.5 × 10^-3 M CaCl₂. K_sp for BaSO₄ = 1.5 × 10^-9 and K_sp for CaSO₄ = 6.1 × 10^-5. Which of the following statements is true?

Correct Answer
verified

Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8 × 10^-10) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

Correct Answer
verified

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH⁺. Which statement is true?

Correct Answer
verified

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 300.0 mL of 0.200 M NaOH is added

Correct Answer
verified

You have solutions of 0.200 M HNO₂ and 0.200 M KNO₂ (K_a for HNO₂ = 4.00 × 10^-4) . A buffer of pH 3.000 is needed. What volumes of HNO₂ and KNO₂ are required to make 1 L of buffered solution?

Correct Answer
verified

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1) . The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What is the pH at point I (V₁/2 HCl added) ?

Correct Answer
verified

The contents of the flask are transferred quantitatively to a 2L volumetric. 100ml of 1 M HCL is added and the flask filled to the mark with water. There is still observable solid calcium hydroxide in the bottom of the new flask. What is the pH of this solution?

Correct Answer
verified

A 50.00-mL sample of 0.100 M Ca(NO₃) ₂ is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The K_sp for CaF₂ is 4.0 × 10^-11.

Correct Answer
verified

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

Correct Answer
verified

Differentiate between the equivalence point and the endpoint in an acid-base titration.

Correct Answer
verified
See Sectio...
View Answer

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -0 mL of 1.00 M NaOH

Correct Answer
verified

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49 × 10^-2, K_a2 = 2.03 × 10^-6. -Calculate [H⁺] after 300.0 mL of 1.00 M NaOH has been added.

Correct Answer
verified

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN) ₃^2-: Calculate the solubility of CuBr(s) (K_sp = 1.0 × 10^-5) in 1.0 L of 1.0 M NaCN.

Correct Answer
verified

Calculate the concentration of [H⁺] of a buffered solution containing 5.0 × 10⁻⁴ M HCN (K_a = 6.2 × 10⁻¹⁰) and 1.5 × 10⁻⁴ M NaCN.

Correct Answer
verified

A 200-mL solution contains 0.018 mol each of I^-, Br^-, and Cl^-. When the solution is mixed with 200 mL of 0.24 M AgNO₃, how much AgCl(s) precipitates out?

Correct Answer
verified

In the titration of 100.0 mL of a 0.200 M solution of H₂A (K_a1 = 1.0 × 10^-5, K_a2 = 1.0 × 10^-8) , what volume of 0.400 M NaOH must be added to reach a pH of 5.00?

Correct Answer
verified

Exam 8: Applications of Aqueous Equilibria

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. -200.0 mL of 1.00 M NaOH

Correct AnswerverifiedShow Answer

What is the molarity of a sodium hydroxide solution if 25.0 mL of this solution reacts exactly with 22.30 mL of 0.253 M sulfuric acid?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following salts shows the lowest solubility in water? Ksp values are as follows: Ag2S = 1.6 × 10-49; Bi2S3 = 1.0 × 10-72; HgS = 1.6 × 10-54; Mg(OH) 2 = 8.9 × 10-12; MnS = 2.3 × 10-13)

Correct AnswerverifiedShow Answer

A 0.012-mol sample of Na2SO4 is added to 400 mL of each of two solutions. One solution contains 1.5 × 10-3 M BaCl2; the other contains 1.5 × 10-3 M CaCl2. Ksp for BaSO4 = 1.5 × 10-9 and Ksp for CaSO4 = 6.1 × 10-5. Which of the following statements is true?

Correct AnswerverifiedShow Answer

Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8 × 10-10) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

Correct AnswerverifiedShow Answer

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH+. Which statement is true?

Correct AnswerverifiedShow Answer

A 200.0-mL sample of the weak acid H3A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 300.0 mL of 0.200 M NaOH is added

Correct AnswerverifiedShow Answer

You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00 × 10-4) . A buffer of pH 3.000 is needed. What volumes of HNO2 and KNO2 are required to make 1 L of buffered solution?

Correct AnswerverifiedShow Answer

Consider the following information about the diprotic acid ascorbic acid (H2As for short, molar mass = 176.1) . The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below: -What is the pH at point I (V1/2 HCl added) ?

Correct AnswerverifiedShow Answer

The contents of the flask are transferred quantitatively to a 2L volumetric. 100ml of 1 M HCL is added and the flask filled to the mark with water. There is still observable solid calcium hydroxide in the bottom of the new flask. What is the pH of this solution?

Correct AnswerverifiedShow Answer

A 50.00-mL sample of 0.100 M Ca(NO3) 2 is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0 × 10-11.

Correct AnswerverifiedShow Answer

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

Correct AnswerverifiedShow Answer

Differentiate between the equivalence point and the endpoint in an acid-base titration.

Correct AnswerverifiedSee Sectio...View AnswerShow Answer

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. -0 mL of 1.00 M NaOH

Correct AnswerverifiedShow Answer

A titration of 100.0 mL of 1.00 M malonic acid (H2A) was done with 1.00 M NaOH. For malonic acid, Ka1 = 1.49 × 10-2, Ka2 = 2.03 × 10-6. -Calculate [H+] after 300.0 mL of 1.00 M NaOH has been added.

Correct AnswerverifiedShow Answer

A 50.0-mL sample of 2.0 × 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN) 32-: Calculate the solubility of CuBr(s) (Ksp = 1.0 × 10-5) in 1.0 L of 1.0 M NaCN.

Correct AnswerverifiedShow Answer

Calculate the concentration of [H+] of a buffered solution containing 5.0 × 10−4 M HCN (Ka = 6.2 × 10−10) and 1.5 × 10−4 M NaCN.

Correct AnswerverifiedShow Answer

A 200-mL solution contains 0.018 mol each of I-, Br-, and Cl-. When the solution is mixed with 200 mL of 0.24 M AgNO3, how much AgCl(s) precipitates out?

Correct AnswerverifiedShow Answer

In the titration of 100.0 mL of a 0.200 M solution of H2A (Ka1 = 1.0 × 10-5, Ka2 = 1.0 × 10-8) , what volume of 0.400 M NaOH must be added to reach a pH of 5.00?

Correct AnswerverifiedShow Answer

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -200.0 mL of 1.00 M NaOH

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Which of the following salts shows the lowest solubility in water? K_sp values are as follows: Ag₂S = 1.6 × 10^-49; Bi₂S₃ = 1.0 × 10^-72; HgS = 1.6 × 10^-54; Mg(OH) ₂ = 8.9 × 10^-12; MnS = 2.3 × 10^-13)

Correct Answer
verified

A 0.012-mol sample of Na₂SO₄ is added to 400 mL of each of two solutions. One solution contains 1.5 × 10^-3 M BaCl₂; the other contains 1.5 × 10^-3 M CaCl₂. K_sp for BaSO₄ = 1.5 × 10^-9 and K_sp for CaSO₄ = 6.1 × 10^-5. Which of the following statements is true?

Correct Answer
verified

Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8 × 10^-10) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

Correct Answer
verified

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH⁺. Which statement is true?

Correct Answer
verified

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 300.0 mL of 0.200 M NaOH is added

Correct Answer
verified

You have solutions of 0.200 M HNO₂ and 0.200 M KNO₂ (K_a for HNO₂ = 4.00 × 10^-4) . A buffer of pH 3.000 is needed. What volumes of HNO₂ and KNO₂ are required to make 1 L of buffered solution?

Correct Answer
verified

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1) . The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What is the pH at point I (V₁/2 HCl added) ?

Correct Answer
verified

Correct Answer
verified

A 50.00-mL sample of 0.100 M Ca(NO₃) ₂ is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The K_sp for CaF₂ is 4.0 × 10^-11.

Correct Answer
verified

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

Correct Answer
verified

Correct Answer
verified
See Sectio...
View Answer

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -0 mL of 1.00 M NaOH

Correct Answer
verified

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49 × 10^-2, K_a2 = 2.03 × 10^-6. -Calculate [H⁺] after 300.0 mL of 1.00 M NaOH has been added.

Correct Answer
verified

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN) ₃^2-: Calculate the solubility of CuBr(s) (K_sp = 1.0 × 10^-5) in 1.0 L of 1.0 M NaCN.

Correct Answer
verified

Calculate the concentration of [H⁺] of a buffered solution containing 5.0 × 10⁻⁴ M HCN (K_a = 6.2 × 10⁻¹⁰) and 1.5 × 10⁻⁴ M NaCN.

Correct Answer
verified

A 200-mL solution contains 0.018 mol each of I^-, Br^-, and Cl^-. When the solution is mixed with 200 mL of 0.24 M AgNO₃, how much AgCl(s) precipitates out?

Correct Answer
verified

In the titration of 100.0 mL of a 0.200 M solution of H₂A (K_a1 = 1.0 × 10^-5, K_a2 = 1.0 × 10^-8) , what volume of 0.400 M NaOH must be added to reach a pH of 5.00?

Correct Answer
verified