18. Aqueous Equilibrium
Complex Ions: Formation Constant
02:20
Practice this topic
- Multiple Choice
If your equilibrium constant K is equal to the product of Ksp and Kf, find the solubility of AgCl in 2.0 M NH3. Ksp of AgCl = 1.77 × 10−10; Kf of Ag(NH3)2+ = 1.7 × 107.
1031views3rank1comments - Multiple Choice
A solution is composed of 3.20 × 10−4 M Co(NO3)3 mixed with 0.200 M NH3. Determine the [Co3+] that remains once the solution reaches equilibrium in the formation of Co(NH3)63+.
1023views1rank - Textbook QuestionWhat is the molar solubility of AgI in 0.20 M NaCN? (a) 6.2 x 10^-4 M(b) 1.0 x 10^-1 M(c) 7.6 x 10^-2 M(d) 2.1 x 10^-3 M932views
- Textbook Question
The solubility product for Zn1OH22 is 3.0 * 10-16. The formation constant for the hydroxo complex, Zn1OH242 - , is 4.6 * 1017. What concentration of OH- is required to dissolve 0.015 mol of Zn1OH22 in a liter of solution?
288views - Textbook Question
The value of Ksp for Cd(OH)2 is 2.5 × 10–14. (b) The solubility of Cd(OH)2 can be increased through formation of the complex ion CdBr42- (Kf = 5 × 103). If solid Cd(OH)2 is added to a NaBr solution, what is the initial concentration of NaBr needed to increase the molar solubility of Cd(OH)2 to 1.0 × 10-3 mol/L?
405views - Textbook Question
Use the appropriate values of Ksp and Kf to find the equilibrium constant for the reaction. FeS(s) + 6 CN-(aq) ⇌ Fe(CN)64-(aq) + S2-(aq)
1568views - Multiple ChoiceA solution contains 2.2 × 10^-3 M in Cu2+ and 0.33 M in LiCN. If the formation constant (Kf) for the complex ion Cu(CN)4^2- is 1.0 × 10^25, how much copper ion (Cu2+) remains at equilibrium?668views
- Multiple ChoiceWhat concentration of Cu2+ is needed to have a concentration of Cu(CN)4^2- equal to 2.0 x 10^-5 M in a solution with a [CN^-] of 9.3 x 10^-4 M? Kf of Cu(CN)4^2- = 1.0 x 10^25708views