Chemical Principles 8th Edition Steven S. Zumdahl, Donald J. DeCoste - Solutions

A solution contains 1.0 3 1026 M HOCl and an unknown concentration of KOCl. If the pH of the solution is 7.20, calculate the KOCl concentration.
Estimate the pH of a solution in which bromcresol green is blue and thymol blue is yellow.
A solution has a pH of 7.0. What would be the color of the solution if each of the following indicators were added? a. Thymol blue c. methyl redb. Bromthymol blue d. crystal viole
The Ksp for lead iodide (PbI2) is 1.4 3 1028. Calculate the solubility of lead iodide in each of the following.a. Waterb. 0.10 M Pb(NO3)2c. 0.010 M NaI
Calculate the solubility of solid Ca3(PO4)2 (Ksp = 1.3 × 10-32) in a 0.20-M Na3PO4 solution.
The solubility of Ce(IO3)3 in a 0.20 M KIO3 solution is 4.4 × 1028 mol/L. Calculate Ksp for Ce(IO3)3.
A solution is prepared by mixing 50.0 mL of 0.10 M Pb (NO3)2 with 50.0 mL of 1.0 M KCl. Calculate the concentrations of Pb21 and Cl- at equilibrium. [Ksp for PbCl2(s) = 1.6 × 1025.]
The Ksp for PbI2(s) is 1.4 × 10-8. Calculate the solubility of PbI2(s) in 0.048 M NaI.
A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the resulting solution. [Ksp for AgIO3(s) = 3.17×10-8.]
Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole barium nitrate is added. Assuming change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.
Calculate the solubility of AgCN(s) (Ksp = 2.2 × 10-12) in a solution containing 1.0 M H1. (Ka for HCN is 6.2 × 10-10.)

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