What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH)2 with 50.00 mL of 0.300 mol L-1 NaOH? Assume that the volumes are additive.

A) 13.05 B) 13.10 C) 13.28 D) 13.58 A) 13.05 B) 13.10 C) 13.28 D) 13.58

Ten milliliters of 0.10 M NH3(aq)(Kb = 1.8 × 10-5)is mixed with 10 mL of 0.10 M NH4Cl(aq).Neglecting the differences between activities and concentrations,the resulting solution:

A) has a pH = 4.74 B) has a [H+] of approximately 10-3 M C) has a [NH4+] greater than that of the NH4Cl(aq) D) has an [OH-] of 1.8 × 10-5 M E) is acidic A) has a pH = 4.74 B) has a [H+] of approximately 10-3 M C) has a [NH4+] greater than that of the NH4Cl(aq) D) has an [OH-] of 1.8 × 10-5 M E) is acidic

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L-1 CH3COOH with 25.00 mL of 0.010 mol L-1 CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3COOH.

A) 2.87 B) 3.74 C) 4.75 D) 5.74 A) 2.87 B) 3.74 C) 4.75 D) 5.74

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L-1 HCl with 40.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

A) 0.64 B) 1.64 C) 12.36 D) 13.36 A) 0.64 B) 1.64 C) 12.36 D) 13.36

Exam 17: Additional Aspects of Acidbase Equilibria

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is

(Multiple Choice)

4.9/5

(33)

Question 21

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH)₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

(Multiple Choice)

4.9/5

(31)

Question 22

A buffer is 0.282 M C₆H₅COOH(aq)and 0.282 M C₆H₅COONa(aq).Calculate the pH after the addition of 0.150 moles of nitric acid to 1.0 L of the buffer.For C₆H₅COOH,pK_a = 4.20.

(Multiple Choice)

4.9/5

(41)

Question 23

Ten milliliters of 0.10 M NH₃(aq)(K_b = 1.8 × 10^-5)is mixed with 10 mL of 0.10 M NH₄Cl(aq).Neglecting the differences between activities and concentrations,the resulting solution:

(Multiple Choice)

4.7/5

(45)

Question 24

What is the pH at the equivalence point for the titration of 0.20 M aqueous nitrous acid by 0.20 M aqueous sodium hydroxide? K_a for nitrous acid is 4.5 × 10^-4

(Multiple Choice)

4.8/5

(37)

Question 25

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

(Multiple Choice)

4.8/5

(40)

Question 26

A 25.0 mL sample of 0.150 mol L^-1 aqueous butanoic acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10^-5.

(Multiple Choice)

4.8/5

(44)

Question 27

A weak acid has K_a = 1.00 × 10^-3.If [HA] = 1.00 M what must be [A^-] for the pH to be 2.7?

(Multiple Choice)

4.9/5

(30)

Question 28

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl(aq)to reach the equivalence point?

(Multiple Choice)

4.9/5

(29)

Question 29

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.10 M HC₂H₃O₂(aq).

(Multiple Choice)

4.9/5

(34)

Question 30

Which of the following mixtures would you dismiss as a potential buffer in a laboratory?

(Multiple Choice)

4.8/5

(39)

Question 31

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L^-¹ HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

(Multiple Choice)

4.8/5

(40)

Question 32

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[HCl] = 1.045 M K_a for HF is 6.6 × 10^-4

(Multiple Choice)

4.7/5

(39)

Question 33

What is the concentration of the acetate ion of an aqueous solution measured to be 0.20 M acetic acid in 0.20 M hydrochloric acid? (K_a for acetic acid = 1.8 × 10^-5)

(Multiple Choice)

4.7/5

(35)

Question 34

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.1 M NaCl(aq).

(Multiple Choice)

4.9/5

(32)

Question 35

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 aqueous acetic acid with 10.00 mL of 0.10 mol L^-1 KOH(aq)? Assume that the volumes of the solutions are additive.K_a = For CH₃COOH.

(Multiple Choice)

4.7/5

(41)

Question 36

The color change range of most acid-base indicators is 1 pH unit.

(True/False)

4.9/5

(44)

Question 37

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.10 M NaCN(aq).

(Multiple Choice)

4.9/5

(30)

Question 38

For the following titration,determine whether the solution at the equivalence point is acidic,basic,or neutral and why: NaHCO₃(aq)titrated with NaOH(aq)

(Multiple Choice)

4.9/5

(38)

Question 39

Choose the correct statement.

(Multiple Choice)

4.9/5

(40)

Question 40

Showing 21 - 40 of 130

Exam 17: Additional Aspects of Acidbase Equilibria

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L-1 in nitrous acid.The acid dissociation constant of nitrous acid is

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH)2 with 50.00 mL of 0.300 mol L-1 NaOH? Assume that the volumes are additive.

A buffer is 0.282 M C6H5COOH(aq)and 0.282 M C6H5COONa(aq).Calculate the pH after the addition of 0.150 moles of nitric acid to 1.0 L of the buffer.For C6H5COOH,pKa = 4.20.

Ten milliliters of 0.10 M NH3(aq)(Kb = 1.8 × 10-5)is mixed with 10 mL of 0.10 M NH4Cl(aq).Neglecting the differences between activities and concentrations,the resulting solution:

What is the pH at the equivalence point for the titration of 0.20 M aqueous nitrous acid by 0.20 M aqueous sodium hydroxide? Ka for nitrous acid is 4.5 × 10-4

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L-1 CH3COOH with 25.00 mL of 0.010 mol L-1 CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3COOH.

A 25.0 mL sample of 0.150 mol L-1 aqueous butanoic acid is titrated with a 0.150 mol L-1 NaOH(aq)solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10-5.

A weak acid has Ka = 1.00 × 10-3.If [HA] = 1.00 M what must be [A-] for the pH to be 2.7?

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L-1 HCl(aq)to reach the equivalence point?

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.10 M HC2H3O2(aq).

Which of the following mixtures would you dismiss as a potential buffer in a laboratory?

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L-1 HCl with 40.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[HCl] = 1.045 M Ka for HF is 6.6 × 10-4

What is the concentration of the acetate ion of an aqueous solution measured to be 0.20 M acetic acid in 0.20 M hydrochloric acid? (Ka for acetic acid = 1.8 × 10-5)

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.1 M NaCl(aq).

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L-1 aqueous acetic acid with 10.00 mL of 0.10 mol L-1 KOH(aq)? Assume that the volumes of the solutions are additive.Ka = For CH3COOH.

The color change range of most acid-base indicators is 1 pH unit.

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.10 M NaCN(aq).

For the following titration,determine whether the solution at the equivalence point is acidic,basic,or neutral and why: NaHCO3(aq)titrated with NaOH(aq)

Choose the correct statement.

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH)₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

A buffer is 0.282 M C₆H₅COOH(aq)and 0.282 M C₆H₅COONa(aq).Calculate the pH after the addition of 0.150 moles of nitric acid to 1.0 L of the buffer.For C₆H₅COOH,pK_a = 4.20.

Ten milliliters of 0.10 M NH₃(aq)(K_b = 1.8 × 10^-5)is mixed with 10 mL of 0.10 M NH₄Cl(aq).Neglecting the differences between activities and concentrations,the resulting solution:

What is the pH at the equivalence point for the titration of 0.20 M aqueous nitrous acid by 0.20 M aqueous sodium hydroxide? K_a for nitrous acid is 4.5 × 10^-4

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

A 25.0 mL sample of 0.150 mol L^-1 aqueous butanoic acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10^-5.

A weak acid has K_a = 1.00 × 10^-3.If [HA] = 1.00 M what must be [A^-] for the pH to be 2.7?

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl(aq)to reach the equivalence point?

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.10 M HC₂H₃O₂(aq).

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L^-¹ HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[HCl] = 1.045 M K_a for HF is 6.6 × 10^-4

What is the concentration of the acetate ion of an aqueous solution measured to be 0.20 M acetic acid in 0.20 M hydrochloric acid? (K_a for acetic acid = 1.8 × 10^-5)

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 aqueous acetic acid with 10.00 mL of 0.10 mol L^-1 KOH(aq)? Assume that the volumes of the solutions are additive.K_a = For CH₃COOH.

For the following titration,determine whether the solution at the equivalence point is acidic,basic,or neutral and why: NaHCO₃(aq)titrated with NaOH(aq)