Determine [Zn2+], [CN−], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of 2.340. The Ksp for Zn(CN)2 is 3.0×10−16. The Ka for HCN is 6.2×10−10.
Determine [Zn2+], [CN−], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of...
Determine (Zn2+], [CN-), and (HCN) in a saturated solution of Zn(CN), with a fixed pH of 2.080. The Ksp for Zn(CN), is 3.0 x 10-16. The K, for HCN is 6.2 x 10-10. (Zn2+] = [HCN] = CNC] =
Determine [Zn2+], [CN-], and [HCN) in a saturated solution of Zn(CN), with a fixed pH of 1.250. The Ksp for Zn(CN), is 3.0 x 10-16. The K, for HCN is 6.2 x 10-10. [Zn²+] = M [HN] = | M [CN-] = M
Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of 2.160. The Ksp for Zn(CN)2 is 3.0 × 10–16. The Ka for HCN is 6.2 × 10–10. Hint: Use the systematic treatment of equilibrium to solve this problem. 1. Write the pertinent reactions. 2. Write the charge balance equation. 3. Write the mass balance equations. 4. Write the equilibrium constant expressions for each reaction. 5. Count the equations and unknowns. 6. Solve for...
LL Determine [Zn2+1, (CN"), and [HCN) in a saturated solution of Zn(CN), with a fixed pH of 2.180. The K, for Zn(CN), is 3.0 x 10-16. The K, for HCN is 6.2 x 10-10. [Zn2+] = [HCN] = | [CN) =
Determine the molar solubility (S) of Zn(CN)2 in a solution with a pH=5.06. Ignore activities. The Ksp for Zn(CN)2 is 3.0×10−16 TheKa for HCN is 6.2×10−10
Determine the molar solubility ( ? ) of Zn(CN)2 in a solution with a pH=5.89 . Ignore activities. The ?sp for Zn(CN)2 is 3.0×10−16 . The ?a for HCN is 6.2×10−10.
Problem 2: Find the concentrations of Agt. CN. and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: AgCN() ► Ag+ + CN- CN + H20 HCN(aq) + OH Ksp = 2.2 x 10-16 Kb = 1.6 x 105
Problem 2: Find the concentrations of Ag, CN, and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: Ksp = 2.2 x 10-16 AgCN(s) CN + H20 Ag+ + CN- HCN(aq) + OH- Kb = 1.6 x 10-5
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...
ksp= 8x10-12 A 350.0 mL sample of a saturated solution of Zn(CN)2 is at equilibrium at 25C. At equilibrium, the [CN-1) is 2.52 x 10-4 M. What is the molar solubility of Zn(CN)2? Enter your answer with units. If no units are required, write no units after your number.