Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of...
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
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 1.57×10-2 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
Determination of a Solubility Product and Observation of the Common lon Effect . Calculate the molar solubility in mol/L for Zn(OH): in water. Zn(OH): has a Kap value of 1.8 x 10. Also, fill in the provided ICE table in solving this problem. Zn(OH)2(s)Zn2 (ag)20H (aq) Initial concentration (M Change in concentration (M) Equilibrium concentration (M From the molar solubility in question 1, calculate the concentration of OH ions in solution, and the pH of the solution. . Two 10.0...
Find the hydronium ion concentration and pH for the following 1. 2. Calculate the hydronium ion concentration and the pH when 80.0 mL of 0.55 MNH, is mixed with 80.0 mL of 0.55 M HCl (K. = 5.6 x 10-10). Concentration M pH- Phenol (CH-OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(0) = CH.0 (aq) +H3O+ (aq) K= 1.3 x 10-10 If you dissolve 0.593 g of the acid in enough water to...
5) Zinc forms a precipitate with the hydroxide ion (Zn(OH)2) as well as several complex ions. Given the equilibria below, calculate the concentration of each zinc species in a solution saturated with Zn(OH)2 and [OH') fixed at 3.2 x 107M Zn(OH)2(8) Ksp = 3 x 10-16 Zn(OH)* K= 1 x 104 Zn(OH)2(aq) K = 2 x 1010 Zn(OH)3 K = 8 x 1013 Zn(OH)42 K= 3 x 1015
In the presence of excess OH-, the Al3+(aq) ion forms a hydroxide complex ion, Al(OH)4-. Calculate the concentration of free Al3+ ion when 1.32×10-2 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 13.00). For Al(OH)4-, Kf = 1.1×1033. [Al3+] = ?M
Which substance is the oxidizing agent in the following reaction? Ca(s) + Zn2+1 Zn2+ (aq) 2+ - Ca (aq) + Zn(s) Zn(s) Oca 2t (al O cals) None of the above Zn2+ (aq) The oxidation number for each atom in Gaz(SO4)3 is O +2, +4, -1. 0 1. +3, +4, -1. +2, +4,-2. O 1. +3, +6, -2. The molar solubility of Calcium carbonate is 4.2 x 10-6 M. What is Ksp for this compound 3.0 x 0 x 10-16...
calculate the initial pH of the solution given the following reaction. Ca(OH)2 -> Ca2+ + 2OH- with ksp= 1.3 x 10^-6 please explain how you got your answer. 15) (5 pts) Calculate the initial pH of the solution given the following reaction and equilibrium information below: Ca(OH),(s) = Ca2+ (aq) + 20H- (aq) with Ksp = 1.3 x 10-6 A) 8.2 B) 10.3 C) 11.8 D) 12.1 E) None of these are correct + Ann
What is the maximum concentration of Ni2+ in a solution of pH 10.00? Ksp (NI(OH)2) = 2.0*10-15 M