7. A buffer solution is 0.25M CH,COOH-0.15M NaCH,COO, saturated in H₂S (0.10M), and with [Mn¹2] = 0.15M a. show that Mns will not precipitate from this solution (for MnS, Ksp = 3 x 10'). b. Which buffer component would you increase in concentration, and to what minimum value, to ensure that precipitation of MnS begins? Assume that the concentration of the other buffer component is held constant.

From the solubility data given for the following compounds, calculate their solubility product constants. a. Cu Br, copper (1) bromide, 1.0 × 10-³ g/L Ksp b. Ag I, silver iodide, 2.8 × 10-8 g/10 mL Ksp = =

You are given a solution of 0.20M CoCl3, 0.15M SnCl2, 0.35M CuCl2, and 0.25M AgCl.Giventhe following table, calculatethe hydroxide concentration needed to precipitate each metal individually so they can be recovered. You do not want more than one metal to precipitate at one time or when you filter the precipitate you will get a mixture.(Optional; calculate the volume of a 0.25M NaOH solution needed to cause this precipitation) b.) Hydroxide needed to precipitate Sn(OH)2 c.) Hydroxide needed to precipitate Cu(OH)2 d.) Hydroxide needed to precipitate AgOH

Write the balanced equation for the reaction of aqueous Pb(CIO,), with aqueous Nal. Include phases. chemical equation: Ph(CIO, ), + 2Nal(aq) 2NACIO, + Pbl,(s) Incarect What mass of precipitate will form if 1.50 L of highly concentrated Ph(CIO, ), is mixed with 0.400 L. 0.200 M Nal? Assume the reaction goes to completion. mass of precipitate: 87.78 Incorect