Which of the compounds is more soluble in an acidic solution than in pure water? Zn(OH)2 Ag₂S KCIO4 Pbl₂ AIPO4

Calculate the molar solubility of CdCO3 in a buffer solution containing 0.115 M Na2CO3 and 0.120 M NaHCO3

Calculate K for the reactions in Question 4.

The weak base ethanolamine. HOCH2CH2NH2, can be titrated with HCl. HOCH2CH2NH2(aq)+H3O+(aq)HOCH2CH2NH3+(aq)+H2O(l) Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 107.) (a) What is the pH of the ethanolamine solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 would be the best choice to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.

A buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.

Refer to Appendix J for solubility products for calcium salts. Determine which of the calcium salts listed is most soluble in moles per liter and which is most soluble in grams per liter.

A solution contains CO32– at a concentration of 0.0023 M and Cl– at a concentration of 0.00076 M. If AgNO3(aq) is added drop by drop to the solution, which ion, CO32– or Cl–, will precipitate first? Give the minimum concentration of Ag+ needed to precipitate each of the

How much salt must be added to PbCl2 to avoid any precipitation of solid PbSO4

An aqueous solution contains 0.27 M hydrocyanic acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.28 mol KCN O 0.27 mol KCIO4 0.134 mol KOH U 0.13 mol HNO3 O 0.28 mol HNO3

A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?