Textbook Question
Use the given molar solubilities in pure water to calculate Ksp for each compound. b. Ag2SO3; molar solubility = 1.55⨉10-5 M c. Pd(SCN)2; molar solubility = 2.22⨉10-8 M
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Ch.17 - Aqueous Ionic Equilibrium
Chapter 17, Problem 8
A 20.0-mL sample of a 0.125 M diprotic acid (H2A) solution is titrated with 0.1019 M KOH. The acid ionization constants for the acid are Ka1 = 5.2 * 10^-5 and Ka2 = 3.4 * 10^-10. At what added volume of base does each equivalence point occur?
Verified step by step guidance1
Calculate the moles of the diprotic acid (H2A) using the initial concentration and volume: \( \text{moles of } H_2A = 0.125 \text{ M} \times 0.0200 \text{ L} \).
Determine the moles of KOH needed to reach the first equivalence point, where all \( H_2A \) is converted to \( HA^- \). This is equal to the initial moles of \( H_2A \).
Calculate the volume of KOH solution required to reach the first equivalence point using the moles of KOH and its concentration: \( \text{Volume of KOH} = \frac{\text{moles of KOH}}{0.1019 \text{ M}} \).
Determine the moles of KOH needed to reach the second equivalence point, where all \( HA^- \) is converted to \( A^{2-} \). This is twice the initial moles of \( H_2A \).
Calculate the total volume of KOH solution required to reach the second equivalence point using the moles of KOH and its concentration: \( \text{Total Volume of KOH} = \frac{\text{moles of KOH for second equivalence point}}{0.1019 \text{ M}} \).
Related Practice
Textbook Question
Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. b. Mg(OH)2 c. CaF2
Open Question
A 15.0-mL sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCl. Calculate the pH for at least five different points throughout the titration curve and sketch the curve. Indicate the volume at the equivalence point on your graph.
Open Question
After a 120.0-mL sample of a solution that is 2.8 * 10^-3 M in AgNO3 is mixed with a 225.0-mL sample of a solution that is 0.10 M in NaCN and the solution reaches equilibrium, what concentration of Ag+(aq) remains?
Open Question
A 0.5224-g sample of an unknown monoprotic acid was titrated with 0.0998 M NaOH. The equivalence point of the titration occurred at 23.82 mL. Determine the molar mass of the unknown acid.
Open Question
Aniline, abbreviated fNH2, where f is C6H5, is an important organic base used in the manufacture of dyes. It has a Kb of 4.3 * 10^(-10). In a certain manufacturing process, it is necessary to keep the concentration of fNH3+ (aniline’s conjugate acid, the anilinium ion) below 1.0 * 10^(-9) M in a solution that is 0.10 M in aniline. Find the concentration of NaOH required for this process.