Chapter 16, Problem 73AP

If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?

What mass of lead (II) iodide, Pbl, (K = 9.80 x 10°, M.M. = %3D 461.0 g/mol), will dissolve in 275 mL of 0.659 M Pb(NO3)2?

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51. In a saturated solution of NiCOs, the concentration of nickel(II) ion is 7.6 x 10 mol/L. The Ksp of nickel(II) carbonate would be which of the following? 5.8 x 107 a. b. 1.2 x 10 C. 4.4 × 10-10 a. adding some PCI(g) b. removing some PCI;(g) c. decreasing temperature d. e. 52. For the equilibrium system below, which of the following would result in an increase in the quantity of Clig)? PCI(g) + Ch(g) PCI;(g) + 45 kJ d. e. 7.6 × 10- none of the above 53. 1.2 mol of CH,OH(g) are injected into a 2.0 L. container and the following equilibrium becomes established. 2H2(g) + CO(g) CH₂OH(g) + 92 kJ If at equilibrium 1.0 mol of CH₂OH is still in the container the K must be which of the following? a. 25 12.5 b. 125 0.032 c. 0.0080 d. e. increasing the volume of the container injecting some He gas 54. If the equilibrium shown below is cooled at a constant pressure. H₂(g) + 12(g) 2HI(g) + 65 kJ What is most likely to happen? a. [Pb][Br] b. [Pb][Br] c. [Pb ][Br] d. both a and c e. both b and…

Describe how you would prepare a) 7.00L of 0.0500M potassium permanganate solution from solid potassium permanganate and water b) 500 ml of a solution that is 0.0250M in I¯ starting with solid magnesium iodide c) 4.0OL of 0.150 molar perchloric acid solution, starting with 8.00 molar solution of perchloric acid reagent.

11. You are determining the K for Al:(CO3)a. You do some careful measurements and determine that 0.0682 grams of the solid dissolved in 450. mL of water. What is K, for the solid. Molar mass of the solid is 234.01 g/mol.

Solid zinc nitrate is slowly added to 125mL of a 0.0317 M ammonium cyanide solution. The concentration of zinc ion required to just initiate precipitation is?

Jj.144.

Which of the following anions will separate Ag* from Pb** by precipitating one of them, leaving the other in solution? (A) CATIONS High Solubility (aq) Low Solubility (s) OOH™ O cr O C₂H30₂ 3- PO4³- Cl, Br, I Halides SO4²- Most Ag+, Pb²+, Tl+, Hg₂²+, Hg, Cu Solubility Table $2. Group 1, Nhì, Group 2 Most ANIONS OH Group 1, NH4*, Sr²⁰, Ba²+, Tl. Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr², Ra² CO32, C₂H3O2 NO3 PO4³-, SO3²- Group 1, NH4 Most All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Most All Ag+ None