Using the following equilibria, what are the total concentration of dissolved ZINC, and the concentration of...
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
27. Suppose sodium hydroxide is added to a 0.0026 M solution of zinc nitrate such that the pH of the solutionn is 12.99. What is the equilibrium concentration of Zn27 Zn2 (aq)+40H (aq) Zn(OH)(aq), K- 2.8x 1015 a. 1.0x 10-14 M b. 1.1 x 10-17 AM c. 2.4 x 102 M d. 2.6 x 10-3 M e. 9.5 x 10 18 M
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U Caroline Alemany ANDEGI Activities and Due Dates Ch 6c ent Score: 681/3200 Resources Hint Check Answe on 12 of 32 > Determine the concentrations of each zinc-containing species in a solution saturated with solid Zn(OH), and having a fixed OH concentration of 4.3 x 10- M. The equilibrium constants for the equilibria that occur in the solution are given in the table. Zn(OH),(s) Zn(OH)(aq) Zn(OH)(aq) Zn(OH)-(aq) K -3.0 x 10-16 B = 2.5 x 104 = 7.2...
Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of the solution is buffered to pH=12.00 (so that the hydroxide ion concentration is 0.010 M). 1. Zn(OH)2(s) A. [Zn2] 3.0x10-12 M B. [Zn2 3.7x10- M C. [Zn23.0x10-10 M D. [Zn2] 9.1x10-3 M E. [Zn2] 1.5x10-13 M Zn2 (aq) + 20H (aq) Ksp 3.0x10-16 2. When silver carbonate, Ag,COs, is mixed with water, it dissolves to some extent to form a saturated solution where the...
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
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...
please answer both questions
QUESTION 26 Given the two equilibria below, Ag(NH3)2 (aq) = Ag (aq) + 2 NH3(aq) Kd-5.9x 10-8 Agl(s) Ag (aq)+I (aq) what is Ke for the following equilibrium? 10-17 Agl(s)+2NH3(aq) Ag(NH3)2"(aq)+ I (aq) а. 7.1 x 108 b. 1.4x 10-9 2.0 x 10-18 d. 4.9x 10-24 2.7 x 100 QUESTION 27 One liter of saturated zinc hydroxide solution contains 0.000222 g of dissolved Zn(OH)2. Use this information to estimate the Ksp for Zn(OH)2 1 pol a...
± Solubility of Zinc Hydroxide in Basic Solution A solubility-product constant, Ksp, corresponds to a reaction with the following general format: salt(s)⇌cation(aq)+anion(aq) A formation constant, Kf, corresponds to a reaction with the following general format: metal ion(aq)+Lewis base(aq)⇌complex ion(aq) Part A When Zn(OH)2(s) was added to 1.00 L of a basic solution, 1.18×10−2 mol of the solid dissolved. What is the concentration of OH− in the final solution? Express your answer with the appropriate units [OH−] =???
Consider a saturated solution of zinc arsenate, Zn3(AsO4)2 (Ksp = 1.0 × 10-27). If the pH of this solution is fixed at 6.00, what are the concentrations of the following species? Assume that these are the only species present in solution that contain Zn or As. Assume ionic strength is 0. [Zn 2+] = [ZnOH +] = [AsO4 3-] = [HAsO4 2-] = [H2AsO4 -] = [H3AsO4(aq)] =
6. Given a total dissolved lead concentration of
2.0x10-5 M, a total dissolved NTA concentration of
2.0x10-2 M, and a pH of 12.3 (note extreme pH)
a. Under these conditions, what is the dominant form of NTA?
b. Write an equation for total dissolved NTA and for total
dissolved Pb. What assumptions can you make?
c. Calculate the predicted [Pb2+], considering NTA
complexation only?
d. What is the [Pb2+] as predicted by the solubility
of Pb(OH)2(s) at pH 12.3?
e....