Question 1

Which of the following compounds has the lowest solubility, in moles per liter, in water?

Accepted Answer

A)  MgC2O4 Ksp = 8.6 F1F1F1S1F1F1F10 10-5 
B)  PbSO4 Ksp = 1.3 F1F1F1S1F1F1F10 10-8 
C)  CdS Ksp = 1.0 F1F1F1S1F1F1F10 10-28 
D)  Al(OH)3 Ksp = 2 F1F1F1S1F1F1F10 10-32 
E)  Sn(OH)2 Ksp = 3 F1F1F1S1F1F1F10 10-27 
A)  MgC2O4 Ksp = 8.6 F1F1F1S1F1F1F10 10-5 
B)  PbSO4 Ksp = 1.3 F1F1F1S1F1F1F10 10-8 
C)  CdS Ksp = 1.0 F1F1F1S1F1F1F10 10-28 
D)  Al(OH)3 Ksp = 2 F1F1F1S1F1F1F10 10-32 
E)  Sn(OH)2 Ksp = 3 F1F1F1S1F1F1F10 10-27

Question 2

A 0.012-mol sample of Na2SO4 is added to 400 mL of each of two solutions. One solution contains 1.5 F1F1F1S1F1F1F10 10-3 M BaCl2; the other contains 1.5 F1F1F1S1F1F1F10 10-3 M CaCl2. Ksp for BaSO4 = 1.5 F1F1F1S1F1F1F10 10-9 and Ksp for CaSO4 = 6.1 F1F1F1S1F1F1F10 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. 
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.

Question 3

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 0.44 M NaOH until a pink color appears; 13.6 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 g 
A)  480 g 
B)  240 g 
C)  580 g 
D)  290 g 
E)  750 g

Question 4

Titrating 30.00 mL of a saturated calcium iodate solution requires 28.91 mL of a 0.092 M solution of Na2S2O3 according to the equation IO3- + 6S2O32- + 6H+ F1F1F1S1F1F1F10 I- + 2S3O62- + 3H2O
Calculate Ksp for Ca(IO3)2.

Accepted Answer

A)  7.14 F1F1F1S1F1F1F10 10-8 
B)  6.97 F1F1F1S1F1F1F10 10-4 
C)  2.79 F1F1F1S1F1F1F10 10-3 
D)  1.61 F1F1F1S1F1F1F10 10-6 
E)  none of these 
A)  7.14 F1F1F1S1F1F1F10 10-8 
B)  6.97 F1F1F1S1F1F1F10 10-4 
C)  2.79 F1F1F1S1F1F1F10 10-3 
D)  1.61 F1F1F1S1F1F1F10 10-6 
E)  none of these

Question 5

Consider a solution consisting of the following two buffer systems: H2CO3   HCO3- + H+ pKa = 6.4
H2PO4-   HPO42- + H+ pKa = 7.2
At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

Accepted Answer

A)  [H2CO3] > [HCO3-] and [H2PO4-] > [HPO42-] 
B)  [HCO3-] > [H2CO3] and [HPO42-] > [H2PO4-] 
C)  [H2CO3] > [HCO3-] and [HPO42-] > [H2PO4-] 
D)  [H2CO3] = [HCO3-] and [HPO42-] > [H2PO4-] 
E)  [H2CO3] = [HCO3-] and [H2PO4-] > [HPO42-] 
A)  [H2CO3] > [HCO3-] and [H2PO4-] > [HPO42-] 
B)  [HCO3-] > [H2CO3] and [HPO42-] > [H2PO4-] 
C)  [H2CO3] > [HCO3-] and [HPO42-] > [H2PO4-] 
D)  [H2CO3] = [HCO3-] and [HPO42-] > [H2PO4-] 
E)  [H2CO3] = [HCO3-] and [H2PO4-] > [HPO42-]

Question 6

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 F1F1F1S1F1F1F10 10S1U1P1-3S1S1P0 M CuNOS1U1B13S1U1B0. Cu(I) forms complex ions with cyanide as follows:   Calculate the following concentrations at equilibrium:
-[Cu(CN)2-]

Accepted Answer

A)  1.0 F1F1F1S1F1F1F10 10-3 M 
B)  4.0 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-12 M 
C)  2.0 F1F1F1S1F1F1F10 10-7 M 
D)  2.0 F1F1F1S1F1F1F10 10-3 M 
E)  none of these 
A)  1.0 F1F1F1S1F1F1F10 10-3 M 
B)  4.0 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-12 M 
C)  2.0 F1F1F1S1F1F1F10 10-7 M 
D)  2.0 F1F1F1S1F1F1F10 10-3 M 
E)  none of these

Question 7

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (Ka of HZ is 2.3 F1F1F1S1F1F1F10 10-5.) Assume negligible volume of the HCl.

Accepted Answer

A)  6.8 F1F1F1S1F1F1F10 10-3 mol 
B)  7.5 F1F1F1S1F1F1F10 10-2 mol 
C)  1.0 F1F1F1S1F1F1F10 10-3 mol 
D)  5.0 F1F1F1S1F1F1F10 10-1 mol 
E)  none of these 
A)  6.8 F1F1F1S1F1F1F10 10-3 mol 
B)  7.5 F1F1F1S1F1F1F10 10-2 mol 
C)  1.0 F1F1F1S1F1F1F10 10-3 mol 
D)  5.0 F1F1F1S1F1F1F10 10-1 mol 
E)  none of these

Question 8

Chromate ion is added to a saturated solution of Ag2CrO4 to reach 0.10 M CrO42-. Calculate the final concentration of silver ion at equilibrium (Ksp for Ag2CrO4 is 9.0 F1F1F1S1F1F1F10 10-12).

Accepted Answer

A)  9.5 F1F1F1S1F1F1F10 10-6 M 
B)  1.7 F1F1F1S1F1F1F10 10-6 M 
C)  5.5 F1F1F1S1F1F1F10 10-11 M 
D)  6.6 F1F1F1S1F1F1F10 10-6 M 
E)  1.1 F1F1F1S1F1F1F10 10-13 M 
A)  9.5 F1F1F1S1F1F1F10 10-6 M 
B)  1.7 F1F1F1S1F1F1F10 10-6 M 
C)  5.5 F1F1F1S1F1F1F10 10-11 M 
D)  6.6 F1F1F1S1F1F1F10 10-6 M 
E)  1.1 F1F1F1S1F1F1F10 10-13 M

Question 9

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) is titrated with the following volumes of 1.00 M NaOH.
-250.0 mL of 1.00 M NaOH

Accepted Answer

A)  10.00 
B)  9.52 
C)  8.00 
D)  9.00 
E)  None of these 
A)  10.00 
B)  9.52 
C)  8.00 
D)  9.00 
E)  None of these

Question 10

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, Ka = 6.2 * 10-10.
50.0 mL of 0.10 M HNO3
 60.0 mL of 0.20 M Ba(OH)2
 95.0 mL of 0.20 M HClO4
 195.0 mL of 1.0 *10-4 M HCN

Accepted Answer

The answer of Calculate the pH of the final solution...

Question 11

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) 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 these 
A)  9.50 
B)  6.48 
C)  6.00 
D)  8.00 
E)  None of these

Question 12

The salt AgCl is ________ soluble in strong acid solution than in water.

Accepted Answer

A)  neither more nor less (that is, AgCl is equally soluble in strong acid and in water) 
B)  more 
C)  The Ksp value for AgCl must be known to answer this question. 
D)  less 
A)  neither more nor less (that is, AgCl is equally soluble in strong acid and in water) 
B)  more 
C)  The Ksp value for AgCl must be known to answer this question. 
D)  less

Question 13

The concentration of OH- in a saturated solution of Mg(OH)2 is 3.6 F1F1F1S1F1F1F10 10-4 M. What is Ksp for Mg(OH)2?

Accepted Answer

A)  1.3 F1F1F1S1F1F1F10 10-7 
B)  4.7 F1F1F1S1F1F1F10 10-11 
C)  1.2 F1F1F1S1F1F1F10 10-11 
D)  3.6 F1F1F1S1F1F1F10 10-4 
E)  none of these 
A)  1.3 F1F1F1S1F1F1F10 10-7 
B)  4.7 F1F1F1S1F1F1F10 10-11 
C)  1.2 F1F1F1S1F1F1F10 10-11 
D)  3.6 F1F1F1S1F1F1F10 10-4 
E)  none of these

Question 14

A solution contains 0.34 M HA (Ka = 2.0 F1F1F1S1F1F1F10 10-7) and 0.17 M NaA. Calculate the pH after 0.05 mol of NaOH is added to 1.00 L of this solution.

Accepted Answer

A)  6.58 
B)  6.70 
C)  6.40 
D)  6.82 
E)  6.19 
A)  6.58 
B)  6.70 
C)  6.40 
D)  6.82 
E)  6.19

Question 15

Methyl orange is an indicator with a Ka of 1 F1F1F1S1F1F1F10 10-4. Its acid form, HIn, is red, while its base form, In-, is yellow. At pH 6.0, the indicator will be

Accepted Answer

A)  yellow. 
B)  orange. 
C)  red. 
D)  blue. 
E)  not enough information 
A)  yellow. 
B)  orange. 
C)  red. 
D)  blue. 
E)  not enough information

Question 16

In the titration of 100.0 mL of a 0.200 M solution of H2A (Ka1 = 1.0 F1F1F1S1F1F1F10 10-5, Ka2 = 1.0 F1F1F1S1F1F1F10 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 mL 
A)  25.0 mL 
B)  100.0 mL 
C)  0 mL 
D)  150.0 mL 
E)  50.0 mL

Question 17

Given the following Ksp values   which statement about solubility, in moles per liter, in water is correct?

Accepted Answer

A)  The solubility of MnS in water will not be pH dependent. 
B)  MnS has the highest molar solubility in water. 
C)  PbCrO4 has the lowest solubility in water. 
D)  A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution. 
E)  PbCrO4, Zn(OH)2, and Pb(OH)2 have equal solubilities in water. 
A)  The solubility of MnS in water will not be pH dependent. 
B)  MnS has the highest molar solubility in water. 
C)  PbCrO4 has the lowest solubility in water. 
D)  A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution. 
E)  PbCrO4, Zn(OH)2, and Pb(OH)2 have equal solubilities in water.

Question 18

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

Accepted Answer

See Sectio

Question 19

A 50.0-mL sample of 2.0 F1F1F1S1F1F1F10 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-:   What is the concentration of CN- at equilibrium?

Accepted Answer

A)  6.0 F1F1F1S1F1F1F10 10-4 M 
B)  1.0 M 
C)  4.0 M 
D)  2.0 M 
E)  none of these 
A)  6.0 F1F1F1S1F1F1F10 10-4 M 
B)  1.0 M 
C)  4.0 M 
D)  2.0 M 
E)  none of these

Question 20

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

Which of the following compounds has the lowest solubility, in moles per liter, in water?

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?

Titrating 30.00 mL of a saturated calcium iodate solution requires 28.91 mL of a 0.092 M solution of Na₂S₂O₃ according to the equation IO₃^- + 6S₂O₃²^- + 6H⁺  I^- + 2S₃O₆²^- + 3H₂O Calculate K_sp for Ca(IO₃)₂.

Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + H⁺pK_a = 6.4 H₂PO₄^- HPO₄²^- + H⁺pK_a = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)₂^-]

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (K_a of HZ is 2.3  10^-⁵.) Assume negligible volume of the HCl.

Chromate ion is added to a saturated solution of Ag₂CrO₄ to reach 0.10 M CrO₄²^-. Calculate the final concentration of silver ion at equilibrium (K_sp for Ag₂CrO₄ is 9.0  10^-¹²).

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. -250.0 mL of 1.00 M NaOH

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, K_a = 6.2 * 10^-¹⁰. 50.0 mL of 0.10 M HNO₃ 60.0 mL of 0.20 M Ba(OH)₂ 95.0 mL of 0.20 M HClO₄ 195.0 mL of 1.0 *10^-⁴ M HCN

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

The salt AgCl is ________ soluble in strong acid solution than in water.

The concentration of OH^- in a saturated solution of Mg(OH)₂ is 3.6  10^-⁴ M. What is K_sp for Mg(OH)₂?

A solution contains 0.34 M HA (K_a = 2.0  10^-7) and 0.17 M NaA. Calculate the pH after 0.05 mol of NaOH is added to 1.00 L of this solution.

Methyl orange is an indicator with a K_a of 1  10^-⁴. Its acid form, HIn, is red, while its base form, In^-, is yellow. At pH 6.0, the indicator will be

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?

Given the following K_sp values which statement about solubility, in moles per liter, in water is correct?

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

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^-: What is the concentration of CN^- at equilibrium?

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?

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Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

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Exam 8: Applications of Aqueous Equilibria

Which of the following compounds has the lowest solubility, in moles per liter, in water?

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?

Titrating 30.00 mL of a saturated calcium iodate solution requires 28.91 mL of a 0.092 M solution of Na2S2O3 according to the equation IO3- + 6S2O32- + 6H+  I- + 2S3O62- + 3H2O Calculate Ksp for Ca(IO3)2.

Consider a solution consisting of the following two buffer systems: H2CO3 HCO3- + H+ pKa = 6.4 H2PO4- HPO42- + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10-3 M CuNO3. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)2-]

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (Ka of HZ is 2.3  10-5.) Assume negligible volume of the HCl.

Chromate ion is added to a saturated solution of Ag2CrO4 to reach 0.10 M CrO42-. Calculate the final concentration of silver ion at equilibrium (Ksp for Ag2CrO4 is 9.0  10-12).

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. -250.0 mL of 1.00 M NaOH

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, Ka = 6.2 * 10-10. 50.0 mL of 0.10 M HNO3 60.0 mL of 0.20 M Ba(OH)2 95.0 mL of 0.20 M HClO4 195.0 mL of 1.0 *10-4 M HCN

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

The salt AgCl is ________ soluble in strong acid solution than in water.

The concentration of OH- in a saturated solution of Mg(OH)2 is 3.6  10-4 M. What is Ksp for Mg(OH)2?

A solution contains 0.34 M HA (Ka = 2.0  10-7) and 0.17 M NaA. Calculate the pH after 0.05 mol of NaOH is added to 1.00 L of this solution.

Methyl orange is an indicator with a Ka of 1  10-4. Its acid form, HIn, is red, while its base form, In-, is yellow. At pH 6.0, the indicator will be

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?

Given the following Ksp values which statement about solubility, in moles per liter, in water is correct?

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

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-: What is the concentration of CN- at equilibrium?

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?

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Bonding: General Concepts

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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?

Titrating 30.00 mL of a saturated calcium iodate solution requires 28.91 mL of a 0.092 M solution of Na₂S₂O₃ according to the equation IO₃^- + 6S₂O₃²^- + 6H⁺  I^- + 2S₃O₆²^- + 3H₂O Calculate K_sp for Ca(IO₃)₂.

Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + H⁺pK_a = 6.4 H₂PO₄^- HPO₄²^- + H⁺pK_a = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)₂^-]

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (K_a of HZ is 2.3  10^-⁵.) Assume negligible volume of the HCl.

Chromate ion is added to a saturated solution of Ag₂CrO₄ to reach 0.10 M CrO₄²^-. Calculate the final concentration of silver ion at equilibrium (K_sp for Ag₂CrO₄ is 9.0  10^-¹²).

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. -250.0 mL of 1.00 M NaOH

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, K_a = 6.2 * 10^-¹⁰. 50.0 mL of 0.10 M HNO₃ 60.0 mL of 0.20 M Ba(OH)₂ 95.0 mL of 0.20 M HClO₄ 195.0 mL of 1.0 *10^-⁴ M HCN

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

The concentration of OH^- in a saturated solution of Mg(OH)₂ is 3.6  10^-⁴ M. What is K_sp for Mg(OH)₂?

A solution contains 0.34 M HA (K_a = 2.0  10^-7) and 0.17 M NaA. Calculate the pH after 0.05 mol of NaOH is added to 1.00 L of this solution.

Methyl orange is an indicator with a K_a of 1  10^-⁴. Its acid form, HIn, is red, while its base form, In^-, is yellow. At pH 6.0, the indicator will be

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?

Given the following K_sp values which statement about solubility, in moles per liter, in water is correct?

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^-: What is the concentration of CN^- at equilibrium?