Question 1

What is the pH of a buffer solution that is 0.295 mol L-1 in hypochlorous acid (HClO)and 0.373 mol L-1 in sodium hypochlorite (NaClO)? The $K _ { a }$ of hypochlorous acid is 3.8 × $10 ^ { - 8 }$ .

Accepted Answer

A) 13.04 
B) 8.38 
C) 7.32 
D) 6.48 
E) 7.52

Question 2

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of the base.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 3.46 
B) 4.06 
C) 2.85 
D) 3.63 
E) 4.24

Question 3

A 1.00 L buffer solution is 0.150 mol L-1 in C6H5COOH and 0.250 mol L-1 in C6H5COOLi.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl.The Ka for HC7H5O2 is 6.5 × 10-5.

Accepted Answer

A) 4.19 
B) 5.03 
C) 4.41 
D) 3.34 
E) 3.97

Question 4

A buffer solution is 0.100 mol L-1 in both C6H5COOH and C6H5COOLi and has a pH of 4.19.Which of the following pH values would you expect after the addition of a small amount of a strong base?

Accepted Answer

A) 3.89 
B) 3.69 
C) 5.69 
D) 4.49 
E) 8.89

Question 5

What is the molar solubility of calcium hydroxide (Ca(OH)2)in water? The solubility-product constant for CaOH2 is 4.5 × 10-6 at $25 ^ { \circ } \mathrm { C }$

Accepted Answer

A) 1.5 × 10-6 mol L-1 
B) 3.0 × 10-3 mol L-1 
C) 1.1 × 10-3 mol L-1 
D) 1.7 × 10-2 mol L-1 
E) 1.0 × 10-2 mol L-1

Question 6

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH.Determine the pH of the solution after the addition of 300.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

Accepted Answer

A) 12.40 
B) 9.33 
C) 5.06 
D) 8.94 
E) 12.00

Question 7

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A) 6.44 
B) 1.48 
C) 2.00 
D) 12.52 
E) 12.00

Question 8

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A) 4.74 
B) 9.26 
C) 11.13 
D) 13.00 
E) 12.55

Question 9

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.

Accepted Answer

A) 1.00 
B) 1.40 
C) 1.22 
D) 1.30 
E) 2.11

Question 10

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate formed upon the addition of 6 mol L-1 HCl.

Accepted Answer

A) Ba3(PO4)2 
B) CdS 
C) AgCl 
D) NH4Cl 
E) ZnS

Question 11

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 mol L-1 in AgNO3 and 0.075 mol L-1 in NaCl.What will happen once these solutions are mixed? Ksp (AgCl)= 1.77 × 10-10.

Accepted Answer

A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. 
B) Silver chloride will precipitate out of the solution,leaving an unsaturated solution of AgCl. 
C) Silver chloride will precipitate out of the solution,leaving a saturated AgCl solution. 
D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. 
E) Silver chloride will precipitate,leaving a pure solution of NaNO3.

Question 12

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 mol L-1 HCl for complete neutralization? Ka = 3.0 × 10-8 for HOCl.

Accepted Answer

A) 0.30 
B) 3.18 
C) 3.76 
D) 4.03

Question 13

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 mol L-1 KOH solution.What is the concentration of the H3PO4 solution (in mol L-1)?

Accepted Answer

A) 1.03 mol L-1 
B) 0.343 mol L-1 
C) 0.114 mol L-1 
D) 0.138 mol L-1 
E) 0.0461 mol L-1

Question 14

Calculate the pH of a solution that is 0.445 mol L-1 in sodium formate (HCOONa)and 0.265 $\text { mol L-1 }$ in formic acid (HCOOH).The $K _ { a }$ of formic acid is 1.77 × $10 ^ { - 4 }$ .

Accepted Answer

A) 4.860 
B) 3.527 
C) 10.023 
D) 3.977 
E) 3.752

Question 15

For a strong acid titrated with a strong base,is the equivalence point acidic,basic,or neutral?

Accepted Answer

The answer of For a strong acid titrated with a...

Question 16

Consider the K_sp values for two compounds: MZ,K_sp = 1.5 × 10^-20 and MZ₂,K_sp = 1.5 × 10^-20.Why don't these compounds have the same molar solubility?

Accepted Answer

The answer of Consider the K_sp values for two compounds:...

Question 17

What is the molar solubility of silver iodide (AgI )in water? The solubility-product constant for AgI  is 8.5 × 10-17 at 25 °C.

Accepted Answer

A) 16 mol L-1 
B) 1.3 × 10-8 mol L-1 
C) 1.7 × 10-16 mol L-1 
D) 4.3 × 10-17 mol L-1 
E) 9.2 × 10-9 mol L-1

Question 18

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 3.09 
B) 4.11 
C) 3.82 
D) 3.46 
E) 2.78

Question 19

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 mol L-1 HClO with 200.0 mL of 0.30 mol L-1 KClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A) 5.99 
B) 8.01 
C) 7.54 
D) 7.06 
E) 6.46

Question 20

Which of the following compounds' solubility will not be affected by a low pH in solution?

Accepted Answer

A) AgCl 
B) Mg(OH)2 
C) CaF2 
D) CuS 
E) BaCO3

Exam 16: Aqueous Ionic Equilibrium

What is the pH of a buffer solution that is 0.295 mol L^-1 in hypochlorous acid (HClO) and 0.373 mol L^-1 in sodium hypochlorite (NaClO) ? The $K _ { a }$ of hypochlorous acid is 3.8 × $10 ^ { - 8 }$ .

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of the base.The K_a for HF is 3.5 × 10^-4.

A 1.00 L buffer solution is 0.150 mol L^-1 in C₆H₅COOH and 0.250 mol L^-1 in C₆H₅COOLi.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl.The K_a for HC₇H₅O₂ is 6.5 × 10^-5.

A buffer solution is 0.100 mol L^-1 in both C₆H₅COOH and C₆H₅COOLi and has a pH of 4.19.Which of the following pH values would you expect after the addition of a small amount of a strong base?

What is the molar solubility of calcium hydroxide (Ca(OH) ₂) in water? The solubility-product constant for CaOH₂ is 4.5 × 10^-6 at $25 ^ { \circ } \mathrm { C }$

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH.Determine the pH of the solution after the addition of 300.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH) ₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.

A sample contains Ba₃(PO₄) ₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the precipitate formed upon the addition of 6 mol L^-1 HCl.

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 mol L^-1 in AgNO₃ and 0.075 mol L^-1 in NaCl.What will happen once these solutions are mixed? K_sp (AgCl) = 1.77 × 10^-10.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 mol L^-1 HCl for complete neutralization? K_a = 3.0 × 10^-8 for HOCl.

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 mol L^-1 KOH solution.What is the concentration of the H₃PO₄ solution (in mol L^-1) ?

Calculate the pH of a solution that is 0.445 mol L^-1 in sodium formate (HCOONa) and 0.265 $\text { mol L-1 }$ in formic acid (HCOOH) .The $K _ { a }$ of formic acid is 1.77 × $10 ^ { - 4 }$ .

For a strong acid titrated with a strong base,is the equivalence point acidic,basic,or neutral?

Consider the K_sp values for two compounds: MZ,K_sp = 1.5 × 10^-20 and MZ₂,K_sp = 1.5 × 10^-20.Why don't these compounds have the same molar solubility?

What is the molar solubility of silver iodide (AgI) in water? The solubility-product constant for AgI is 8.5 × 10^-17 at 25 °C.

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl.The K_a for HF is 3.5 × 10^-4.

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 mol L^-1 HClO with 200.0 mL of 0.30 mol L^-1 KClO.The K_a for HClO is 2.9 × 10^-8.

Which of the following compounds' solubility will not be affected by a low pH in solution?

Exam 16: Aqueous Ionic Equilibrium

What is the pH of a buffer solution that is 0.295 mol L-1 in hypochlorous acid (HClO) and 0.373 mol L-1 in sodium hypochlorite (NaClO) ? The KaK _ { a }Ka​ of hypochlorous acid is 3.8 × 10−810 ^ { - 8 }10−8 .

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of the base.The Ka for HF is 3.5 × 10-4.

A 1.00 L buffer solution is 0.150 mol L-1 in C6H5COOH and 0.250 mol L-1 in C6H5COOLi.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl.The Ka for HC7H5O2 is 6.5 × 10-5.

A buffer solution is 0.100 mol L-1 in both C6H5COOH and C6H5COOLi and has a pH of 4.19.Which of the following pH values would you expect after the addition of a small amount of a strong base?

What is the molar solubility of calcium hydroxide (Ca(OH) 2) in water? The solubility-product constant for CaOH2 is 4.5 × 10-6 at 25∘C25 ^ { \circ } \mathrm { C }25∘C

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH.Determine the pH of the solution after the addition of 300.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

A 100.0 mL sample of 0.10 mol L-1 Ca(OH) 2 is titrated with 0.10 mol L-1 HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.

A sample contains Ba3(PO4) 2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate formed upon the addition of 6 mol L-1 HCl.

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 mol L-1 in AgNO3 and 0.075 mol L-1 in NaCl.What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10-10.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 mol L-1 HCl for complete neutralization? Ka = 3.0 × 10-8 for HOCl.

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 mol L-1 KOH solution.What is the concentration of the H3PO4 solution (in mol L-1) ?

Calculate the pH of a solution that is 0.445 mol L-1 in sodium formate (HCOONa) and 0.265 mol L-1 \text { mol L-1 } mol L-1 in formic acid (HCOOH) .The KaK _ { a }Ka​ of formic acid is 1.77 × 10−410 ^ { - 4 }10−4 .

For a strong acid titrated with a strong base,is the equivalence point acidic,basic,or neutral?

Consider the Ksp values for two compounds: MZ,Ksp = 1.5 × 10-20 and MZ2,Ksp = 1.5 × 10-20.Why don't these compounds have the same molar solubility?

What is the molar solubility of silver iodide (AgI ) in water? The solubility-product constant for AgI is 8.5 × 10-17 at 25 °C.

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl.The Ka for HF is 3.5 × 10-4.

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 mol L-1 HClO with 200.0 mL of 0.30 mol L-1 KClO.The Ka for HClO is 2.9 × 10-8.

Which of the following compounds' solubility will not be affected by a low pH in solution?

What is the pH of a buffer solution that is 0.295 mol L^-1 in hypochlorous acid (HClO) and 0.373 mol L^-1 in sodium hypochlorite (NaClO) ? The $K _ { a }$ of hypochlorous acid is 3.8 × $10 ^ { - 8 }$ .

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of the base.The K_a for HF is 3.5 × 10^-4.

A 1.00 L buffer solution is 0.150 mol L^-1 in C₆H₅COOH and 0.250 mol L^-1 in C₆H₅COOLi.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl.The K_a for HC₇H₅O₂ is 6.5 × 10^-5.

A buffer solution is 0.100 mol L^-1 in both C₆H₅COOH and C₆H₅COOLi and has a pH of 4.19.Which of the following pH values would you expect after the addition of a small amount of a strong base?

What is the molar solubility of calcium hydroxide (Ca(OH) ₂) in water? The solubility-product constant for CaOH₂ is 4.5 × 10^-6 at $25 ^ { \circ } \mathrm { C }$

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH.Determine the pH of the solution after the addition of 300.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH) ₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.

A sample contains Ba₃(PO₄) ₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the precipitate formed upon the addition of 6 mol L^-1 HCl.

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 mol L^-1 in AgNO₃ and 0.075 mol L^-1 in NaCl.What will happen once these solutions are mixed? K_sp (AgCl) = 1.77 × 10^-10.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 mol L^-1 HCl for complete neutralization? K_a = 3.0 × 10^-8 for HOCl.

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 mol L^-1 KOH solution.What is the concentration of the H₃PO₄ solution (in mol L^-1) ?

Calculate the pH of a solution that is 0.445 mol L^-1 in sodium formate (HCOONa) and 0.265 $\text { mol L-1 }$ in formic acid (HCOOH) .The $K _ { a }$ of formic acid is 1.77 × $10 ^ { - 4 }$ .

Consider the K_sp values for two compounds: MZ,K_sp = 1.5 × 10^-20 and MZ₂,K_sp = 1.5 × 10^-20.Why don't these compounds have the same molar solubility?

What is the molar solubility of silver iodide (AgI) in water? The solubility-product constant for AgI is 8.5 × 10^-17 at 25 °C.

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl.The K_a for HF is 3.5 × 10^-4.

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 mol L^-1 HClO with 200.0 mL of 0.30 mol L^-1 KClO.The K_a for HClO is 2.9 × 10^-8.