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
Ch.17 - Aqueous Ionic Equilibrium
Chapter 17, Problem 11
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?
Verified step by step guidance1
Determine the initial moles of AgNO3 by using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Convert the volume from mL to L before calculation.
Determine the initial moles of NaCN using the same formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Again, convert the volume from mL to L.
Write the balanced chemical equation for the reaction between AgNO3 and NaCN. The reaction is: \( \text{Ag}^+ + 2\text{CN}^- \rightleftharpoons [\text{Ag(CN)}_2]^- \).
Calculate the limiting reactant by comparing the mole ratio from the balanced equation with the initial moles of reactants.
Use the stoichiometry of the reaction to determine the change in moles of \( \text{Ag}^+ \) at equilibrium, and then calculate the concentration of \( \text{Ag}^+ \) by dividing the remaining moles by the total volume of the solution in liters.
Related Practice
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
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?
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.
Textbook Question
In which of these solutions will HNO2 ionize less than it does in pure water? a. 0.10 M NaCl b. 0.10 M KNO3 c. 0.10 M NaOH d. 0.10 M NaNO2
2308
views