If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11,which of the following is TRUE?

A) [HCHO2] 2] B) [HCHO2] = [NaCHO2] C) [HCHO2] 2] D) [HCHO2] > [NaCHO2] E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2. A) [HCHO2] 2] B) [HCHO2] = [NaCHO2] C) [HCHO2] 2] D) [HCHO2] > [NaCHO2] E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

Determine the molar solubility for Zn(OH)2 in pure water.Ksp for Zn(OH)2 is 3.00 × 10-17.

A) 3.0 × 10-17 M B) 7.5 × 10-18 M C) 3.11 × 10-6 M D) 1.96 × 10-6 M E) 5.5 × 10-19 M A) 3.0 × 10-17 M B) 7.5 × 10-18 M C) 3.11 × 10-6 M D) 1.96 × 10-6 M E) 5.5 × 10-19 M

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 40.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

A) 5.00 mL B) 20.0 mL C) 40.0 mL D) 80.0 mL A) 5.00 mL B) 20.0 mL C) 40.0 mL D) 80.0 mL

Calculate the pH of a solution formed by mixing 525 mL of 0.50 M H2CO3 with 355 mL of 0.87 M NaHCO3.The Ka for H2CO3 is 4.3× 10-7.

A) 4.63 B) 10.31 C) 6.44 D) 6.30 E) 4.18 A) 4.63 B) 10.31 C) 6.44 D) 6.30 E) 4.18

Match between columns Premises: pH = pKS1U1B1aS1U1B0 pH = 7 pH = pKS1U1B1a2S1U1B0 pH > 7 pH < 7

The Answer of 3/4 of the way to second equivalence is...

Exam 18: Aqueous Ionic Equilibrium

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 61

Gives what happens at low pH for aluminum hydroxide.

(Multiple Choice)

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Question 62

You have a 0.850 M solution of Na₂CrO₄ at a given temperature.At what concentration will silver ions need to be added in order for a participate to form? The K_sp for Ag₂CrO₄ at this temperature is 2.00 × 10^-12.

(Multiple Choice)

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Question 63

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

(Multiple Choice)

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Question 64

Gives what happens at high pH for aluminum hydroxide.

(Multiple Choice)

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Question 65

If the pKa of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.11,which of the following is TRUE?

(Multiple Choice)

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Question 66

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution before the addition of any KOH.The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 67

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 50.0 mL of LiOH.

(Multiple Choice)

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Question 68

Sketch the titration curve for a diprotic acid.Make sure to label the equivalence point(s)and the relative amounts of base that were added to reach them.

(Short Answer)

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Question 69

A sample contains Ba₃(PO₄)₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the precipitate after the addition of 6 M HCl; H₂S and 0.2 M HCl; OH^-to a pH of 8; and (NH₄)₂HPO₄ with NH₃.

(Multiple Choice)

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Question 70

Determine the molar solubility for Zn(OH)₂ in pure water.K_sp for Zn(OH)₂ is 3.00 × 10^-17.

(Multiple Choice)

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Question 71

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 40.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

(Multiple Choice)

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Question 72

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

(Multiple Choice)

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Question 73

Calculate the pH of a solution formed by mixing 525 mL of 0.50 M H₂CO₃ with 355 mL of 0.87 M NaHCO₃.The K_a for H₂CO₃ is 4.3× 10^-7.

(Multiple Choice)

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Question 74

Identify the compound that is acid-insoluble.

(Multiple Choice)

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Question 75

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of NaCN? Assume that the volumes of the solutions are additive and that K_a =

(Multiple Choice)

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Question 76

Animals will lick up ethylene glycol (antifreeze)due to its sweet taste.The antidote for ethylene glycol poisoning is the administration of

(Multiple Choice)

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Question 77

Which of the following solutions is a good buffer system?

(Multiple Choice)

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Question 78

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

(Multiple Choice)

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Question 79

Match the following.

pH = pK_a

3/4 of the way to second equivalence point of a diprotic acid/strong base titration

pH = 7

half-way to equivalence point of a weak acid/strong base titration

pH = pK_a2

equivalence point of a weak acid/strong base titration

Correct Answer:

Verified

pH = pK_a

pH = 7

pH = pK_a2

pH > 7

pH < 7

(Matching)

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Question 80

Exam 18: Aqueous Ionic Equilibrium

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

Gives what happens at low pH for aluminum hydroxide.

You have a 0.850 M solution of Na2CrO4 at a given temperature.At what concentration will silver ions need to be added in order for a participate to form? The Ksp for Ag2CrO4 at this temperature is 2.00 × 10-12.

The molar solubility of CuI is 2.26 × 10-6 M in pure water.Calculate the Ksp for CuI.

Gives what happens at high pH for aluminum hydroxide.

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11,which of the following is TRUE?

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution before the addition of any KOH.The Ka of HF is 3.5 × 10-4.

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 50.0 mL of LiOH.

Sketch the titration curve for a diprotic acid.Make sure to label the equivalence point(s)and the relative amounts of base that were added to reach them.

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3.

Determine the molar solubility for Zn(OH)2 in pure water.Ksp for Zn(OH)2 is 3.00 × 10-17.

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 40.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

Calculate the pH of a solution formed by mixing 525 mL of 0.50 M H2CO3 with 355 mL of 0.87 M NaHCO3.The Ka for H2CO3 is 4.3× 10-7.

Identify the compound that is acid-insoluble.

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of NaCN? Assume that the volumes of the solutions are additive and that Ka =

Animals will lick up ethylene glycol (antifreeze)due to its sweet taste.The antidote for ethylene glycol poisoning is the administration of

Which of the following solutions is a good buffer system?

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

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A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

You have a 0.850 M solution of Na₂CrO₄ at a given temperature.At what concentration will silver ions need to be added in order for a participate to form? The K_sp for Ag₂CrO₄ at this temperature is 2.00 × 10^-12.

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

If the pKa of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.11,which of the following is TRUE?

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution before the addition of any KOH.The K_a of HF is 3.5 × 10^-4.

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 50.0 mL of LiOH.

A sample contains Ba₃(PO₄)₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the precipitate after the addition of 6 M HCl; H₂S and 0.2 M HCl; OH^-to a pH of 8; and (NH₄)₂HPO₄ with NH₃.

Determine the molar solubility for Zn(OH)₂ in pure water.K_sp for Zn(OH)₂ is 3.00 × 10^-17.

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 40.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

Calculate the pH of a solution formed by mixing 525 mL of 0.50 M H₂CO₃ with 355 mL of 0.87 M NaHCO₃.The K_a for H₂CO₃ is 4.3× 10^-7.

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of NaCN? Assume that the volumes of the solutions are additive and that K_a =

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