For the aqueous [HgC14] complex K = 1.17x10¹³ at 25 °C. 2+ Suppose equal volumes of 0.0082MHg(NO3), solution and 0.60MKCl solution are mixed. Calculate the equilibrium molarity of aqueous Hg** ion. Round your answer to 2 significant digits. M 10

In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)

Calculate the solubility of copper(II) iodate, Cu(IO3)2 (Ksp = 7.4 108), in (a) water. (b) a 0.10 M copper(II) nitrate solution.

A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions. (a) Which acid has the larger equilibrium constant for ionization HA[HA(aq)A(aq)+H+(aq)] or HB[HB(aq)H+(aq)+B(aq)]? (b) What are the equilibrium constants for the ionization of these acids? (Hint: Remember that each solution contains three dissolved species: the weak acid (HA or HB). the conjugate base (A- or B- and the hydrogen ion (H+). Remember that osmotic pressure (like all colligative properties) is related to the total number of solute particles. Specifically for osmotic pressure, those concentrations are described by molarities.)

Sometimes equilibria fur complex ions are described in terms of dissociation constants. Kd . For the complex ion AlF63- the dissociation reaction is: AlF63Al3++6F and Kd=[Al3+][F]6[AlF63]=21024 Calculate the value of the formation constant, Kf, for AlF63-.

Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.

. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.

. Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for K for each process. a. AgIO3(s) c. Zn3(PO4)2(s) b. Sn(OH)2(s) d. BaF2(s)

A 0.250-M sodium sulfate solution is added to a 0.200-M barium nitrate solution and 0.700 g barium sulfate precipitates. Write the balanced equation for this reaction. Calculate the minimum volume of barium nitrate solution that was used. Calculate the minimum volume of sodium sulfate needed to precipitate 0.700 g barium sulfate. Assume 100% yield.

The active ingredient of Pepto-Bismol is the compound bismuth subsalicylate, which undergoes the following dissociation when added to water: C7H5BiO4(s)+H2O(l)C7H4O32(aq)+Bi3+(aq)+OH(aq)K=? If the maximum amount of bismuth subsalicylate that reacts by this reaction is 3.2 1019 mol/L, calculate the equilibrium constant for the preceding reaction.