The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated. (a) CuCN (b) CaCO3 (c) Ag₂CO3 (d) PbBr₂ (e) Y(OH)3 [Cu] = 1.9x10-10 M, [CN] = 1.9x10-10 M [Ca2+] = 5.2x10 -4. 4 M, [CO32-] = 6.5x 10-6 M [Ag+] = 1.8x10-5M, [CO32-] = 2.7×10-2 M [Pb2+] = 1.2x 10-2 M, [Br] =2.4x 10-² M [Y³+] = 3.5x 10-16 M, [OH-] = 6.6x 10-³ M

Can you answer all parts please

A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?

What would happen to the color of the solution in part (b) as shown if a small amount of NaOH were added and Fe(OH)3 precipitated? Explain your answer.