A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 0 mL, 10 mL, 20 mL, equivalence point, one-half equivalence point, 40 mL, 50 mL. Sketch the titration curve.

Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.

(i) Which acid solution is more concentrated?

Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.

(ii) Which acid has the larger Ka?

Consider the titration curves (labeled a and b) for two weak bases, both titrated with 0.100 M HCl. (a)

(b)

(ii) Which base has the larger Kb?

A 0.229-g sample of an unknown monoprotic acid is titrated with 0.112 M NaOH. The resulting titration curve is shown here. Determine the molar mass and pKa of the acid.

A 20.0-mL sample of 0.115 M sulfurous acid (H₂SO₃) solution is titrated with 0.1014 M KOH. At what added volume of base solution does each equivalence point occur?

Methyl red has a pKa of 5.0 and is red in its acid form and yellow in its basic form. If several drops of this indicator are placed in a 25.0-mL sample of 0.100 M HCl, what color will the solution appear? If 0.100 M NaOH is slowly added to the HCl sample, in what pH range will the indicator change color?

Referring to Table 18.1, pick an indicator for use in the titration of each acid with a strong base. a. HF

Referring to Table 17.1, pick an indicator for use in the titration of each base with a strong acid. a. CH3NH2

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. BaSO₄

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. b. PbBr₂

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. c. Ag₂CrO₄

Refer to the Ksp values in Table 18.2 to calculate the molar solubility of each compound in pure water. a. AgBr

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10^-11 M

Use the given molar solubilities in pure water to calculate K_sp for each compound. b. PbF₂; molar solubility = 5.63⨉10^-3 M c. MgF₂; molar solubility = 2.65⨉10^-4 M

Use the given molar solubilities in pure water to calculate K_sp for each compound. a. BaCrO₄; molar solubility = 1.08⨉10^-5 M

Use the given molar solubilities in pure water to calculate K_sp for each compound. b. Ag₂SO₃; molar solubility = 1.55⨉10^-5 M c. Pd(SCN)₂; molar solubility = 2.22⨉10^-8 M

Two compounds with general formulas AX and AX₂ have Ksp = 1.5⨉10^-5. Which of the two compounds has the higher molar solubility?

Consider the compounds with the generic formulas listed and their corresponding molar solubilities in pure water. Which compound has the smallest value of Ksp? a. AX; molar solubility = 1.35⨉10^-4 M b. AX₂; molar solubility = 2.25⨉10^-4 M c. A₂X; molar solubility = 1.75⨉10^-4 M

The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.

Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water

Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO₃)₂

Calculate the molar solubility of barium fluoride in each liquid or solution. c. 0.15 M NaF

Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. b. 0.25 M MCl₂

Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. c. 0.20 M Na₂X

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. b. pH = 7

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. c. pH = 9