16. What is the Ke expression for the dissolution of nickel (II) phosphate in water? [N][PO] a [NI"][PO] [Ni, (PO);] b. [N][PO] [Ni, (PO₂).] C. d. [N][PO]' [N₁,(PO₂):1/

Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia. AgCl(s)+2NH3(aq)Ag(NH3)2+(aq)+Cl(aq) a What is the equilibrium constant for this dissolving process? b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH3 is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH3)2+, and the number of moles of NH3 added to the original solution.

The solubility product of CaSO42H2O is 2.4105. What mass of this salt will dissolve in 1.0 L of 0.010 M SO42-?

Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H2S ( H2S[H2S]=0.10M). What concentrations of Pb2+ and Fe2+ remain in the solution? For a saturated solution of H2S we can use the equilibrium: H2S(aq)+2H2O(l)2H3O+(aq)+S2(aq)K=1.01026 (Hint: The [H3O+] changes as metal sulfides precipitate.)

A 0.64 g sample of the white crystalline dimer (4) is dissolved in 25.0 mL of benzene at 20 C. Use the equilibrium constant to calculate the concentrations of monomer (2) and dimer (4) in this solution.

Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions. b. Lets study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S=[H+]3Ksp/Kw3+KKw/[H+] where S = solubility = [Al3+] + [Al(OH)4] and K is the equilibrium constant for Al(OH)3(s)+OH(aq)Al(OH)4(aq) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 1032. Plot the solubility of Al(OH)3 in the pH range 412.

34. A 0.1% sodium arsenite solution is used as an adsorbent solution…a. CO2b. NO2c. HCld. O3 35. In neutral or slightly alkaline solutions, silver ions react quantitatively with chloride ions, the titration ends with the formation of silver chromate which is red in color as a result of the reaction of excess silver ions with chromate ions. Here is the principle of measurement…a. Cl- ions by argentometric methodb. Ion PO¬42- by argentometric methodc. Ion F- argentometric methodd. SO42- ion by complexometric method

10. The solubility product equilibrium constant, Ksp, of silver bromide is 5.4 x 10-13 at 298 K. AgBr(s) Ag*(aq) + Br (aq) What is A,G°? (R=8.314 J/K-mol) a. ,-3.0 x 10' kJ/mol b. -5.87 kJ/mol %3D c. 5.87 kJ/mol d. 3.0 x 10' kJ/mol e. 7.0 x 10' kJ/mol

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2. Calcium Benzoate (CaBz2): a. A saturated CaBz2 sample solution is at equilibrium and the initially ion concentrations are [Ca²+]ia and [Bz];=b, CaBz₂(s) Ca²+ (aq) + 2Bz¯(aq). This sample is allowed to saturate, and the remaining solids will be filtered out. The final benzoate ion concentration in solution is [BZ];= c as determined from titration. What is the solubility product of CaBz2 in terms of a, b and c? b. The lab experiment uses the saturated CaBz2 solution at equilibrium before titration. Why must the CaBz2 solution be saturated?