Dilute NaOH is introduced into a solution that is 0.060 M in Cu2+ and 0.010 M in Mn2+. (Ksp (Cu(OH)2) = 4.8 × 10-20, Ksp (Mn(OH)2) = 2 × 10-13) a. Which hydroxide precipitates first? b. What OH concentration is needed to initiate precipitation of the first hydroxide? begins to precipitate when [OH-] = M c. What is the concentration of the cation forming the less soluble hydroxide when the more soluble hydroxide begins to form? begins to precipitate when Drag and drop your selection from the following list to complete the answer: [Cu2+] [Mn²+] Mn(OH)2 Cu(OH)2 Cu2+ Mn2+ M

Which of the following compounds, when dissolved in a 0.01-M solution of HClO4, has a solubility greater than in pure water: CuCl, CaCO3, MnS, PbBr2, CaF2? Explain your answer.

The salt MX has a solubility of 3.17 108 mol/L in a solution with pH = 0.000. If K4 for HX is 1.00 1015, calculate the Ksp value for MX.

A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2. What volume of 0.10 M NaOH must be added to change the pH of the original buffer solution by 2.5%?

What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases it may be necessary to control the pH. (Hint: Consider the KSP values given in Appendix J.) (a) Hg22+ and Cu2+. (b) SO42- and Cl-. (c) Hg2+ and CO2+. (d) Zn2+ and Sr2+. (e) Ba2+ and Mg2+. (f) CO32- and OH-

A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?

The Ksp for lead iodide (PbI2) is 1.4 108. Calculate the solubility of lead iodide in each of the following. a. water b. 0.10 M Pb(NO3)2 c. 0.010 M NaI

You place 1.234 g of solid Ca(OH)2 in 1.00 L of pure water at 25 C. The pH of the solution is found to be 12.68. Estimate the value of Ksp for Ca(OH)2.

Consider the following pH curves for 100.0 mL of two different acids with the same initial concentration each titrated by 0.10 M NaOH. a. Which plot represents a pH curve of a weak acid, and which plot is for a strong acid? How can you tell? Cite three differences between the plots that help you decide. b. In both cases the pH is relatively constant before the pH changes greatly. Does this mean that at some point in each titration each solution was a buffered solution? c. True or false? The equivalence point volume for each titration is the same. Explain your answer. d. True or false? The pH at the equivalence point for each titration is the same. Explain your answer.

When 5 M ammonia is added to a solution containing Cu(OH)2(s), the precipitate will eventually dissolve in solution. Why? If 5 M HNO3 is then added, the Cu(OH)2 precipitate re-forms. Why? In general, what effect does the ability of a cation to form a complex ion have on the solubility of salts containing that cation?