5) Zinc forms a precipitate with the hydroxide ion (Zn(OH)2) as well as several complex ions....
A) Consider the insoluble compound zinc hydroxide, Zn(OH)2. The zinc ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Zn(OH)2(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH3)42+, Kf = 2.9×109. Specify states such as (aq) or (s) and provide K. K = ______ B) Consider the insoluble compound nickel(II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions....
Consider the insoluble compound zinc carbonate, ZnCO;. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO; (5) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction For Zn(OH)2-, K -2.9x1015Use the pull-down boxes to specify states such as (aq) or (s). K Submit Answer Retry Entire Group 8 more group attempts remaining sted
Using the following equilibria, what are the total concentration of dissolved ZINC, and the concentration of EACH zinc species in a solution with a pH of 9.0? (you may neglect activity coefficients here) Zn(OH)2 (s) Zn2+ (aq) + 2 OH+ (aq) Zn2+ (aq) + OH- (aq) ZnOH(aq) Zn2+ (aq) + 2 OH- (aq) Zn(OH)2 (aq) Zn2+ (aq) + 3 OH- (aq) Zn(OH)3- (aq) Zn²+ (aq) + 4 OH" (aq) Zn(OH)42-(aq) Ksp = 3 x 10-16 Ki = 1 x 104...
1- In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate the concentration of free Zn2+ ion when 1.32×10-2mol ZnSO4(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.40). For Zn(OH)42-, Kf = 4.6×1017. [Zn2+] = ------ M 2- What is the approximate concentration of free Hg2+ ion at equilibrium when 1.86×10-2 mol mercury(II) nitrate is added to 1.00 L of solution that is 1.310...
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate the concentration of free Zn2+ ion when 1.54×10-2 mol Zn(CH3COO)2(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.70). For Zn(OH)42-, Kf = 4.6×1017. [Zn2+] = M
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate the concentration of free Zn2+ ion when 1.57×10-2 mol Zn(NO3)2(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.20). For Zn(OH)42-, Kf = 4.6×1017. [Zn2+]=___M please explain
What is the molar solubility of zinc hydroxide at pH 12.34? For Zn(OH)2, Ksp = 2.1 x 10-16; for Zn(OH)42-, Ky= 2.8 x 1015 a) 1.2 x 10-25 M b) 1.3 x 10-2 M c) 3.7 x 10-6 M d) 1.4 x 10-8 M e) 2.8 x 10 4 M
7. Solid Zinc Hydroxide, Zn(OH)dissolves in water to form zinc ions, and hydroxide ions. a. Write the expression for the solubility product constant, Kyp, of zinc hydroxide. b. If the value of the K, for zinc hydroxide is 7.7 x 10-17 at 25°C, calculate the molar solubility bo zinc hydroxide at 25°C.
3. Pb(OH)2 (8) is amphoteric and forms the complex ion Pb(OH)/(aq) with excess OH in solution. Write the balanced equilibrium equation of Pb(OH)2 (s) in the presence of excess hydroxide. 4. A solution contains Pb(NO3)2 and Zn(NO3)2. Consult the solubility table and answer the following questions: a. NaOH (aq) is added to the solution. What precipitate (or precipitates) forms? b. Can you separate the two metal ions using NaOH? c. Nat (aq) is added to the solution. What precipitate (or...
A) Consider the insoluble compound cobalt(II) hydroxide , Co(OH)2. The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Co(OH)2(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH3)62+, Kf = 7.7×104. Use the pull-down boxes to specify states such as (aq) or (s). _____ + _____ = _____ + _____ K = B) Consider the insoluble compound nickel(II) carbonate ,...