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 (S) of Zn(CN)2 in a solution with a pH=5.06. Ignore activities. The...
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.
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), 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) =
what is the molar solubility of Zn^2+ in a solution that is buffered at a pH of 3.00? The Ksp for Zn(OH)2 is 3x10^-17.
Determine the molar solubility of copper(1) azide (CuN,) in a solution with a pH of 8.59. Ignore activities. The Ksp for CuN, is 4.9 x 10-9. The K, for HN, is 2.2 x 10-5 molar solubility:
Determine the molar solubility of copper(I) azide (CuN3) in a solution with a pH of 12.50. Ignore activities. The ?sp for CuN3 is 4.9×10−9. The Ka for HN3 is 2.2×10−5
The Ksp value for Zn(OH)2 is 5.0 times 10-6. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.