Multiple ChoiceIf 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 × 107.189views1rank1comments
Multiple ChoiceA 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+.202views
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 M926views
Textbook QuestionFrom the value of Kf listed in Table 17.1, calculate the concentration of Ni2 +1aq2 and Ni1NH326 2+ that are present at equilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of 0.20 M NH31aq2.878views
Textbook QuestionThe 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?284views
Textbook QuestionThe value of Ksp for Cd1OH22 is 2.5 * 10-14. (b) The solubility of Cd1OH22 can be increased through formation of the complex ion CdBr42 - 1Kf = 5 * 1032. If solid Cd1OH22 is added to a NaBr solution, what is the initial concentration of NaBr needed to increase the molar solubility of Cd1OH22 to 1.0 * 10-3 mol/L?400views
Textbook QuestionA solution is made 1.1 * 10 - 3 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2 + (aq) remains?1054views
Textbook QuestionUse the appropriate values of Ksp and Kf to find the equilibrium constant for the reaction. FeS(s) + 6 CN-(aq)ΔFe(CN)64 - (aq) + S2 - (aq)1556views
Textbook QuestionIs the solubility of Zn(OH)2 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (c) NaCN616views
Textbook QuestionDissolution of 5.0 x 10^-3 mol of Cr(OH)3 in 1.0 L of 1.0 M NaOH gives a solution of the complex ion [Cr(OH)4]- (Kf = 8 x10^29). What fraction of the chromium in such a solution is present as uncomplexed Cr3+?517views
Textbook QuestionWrite a balanced net ionic equation for each of the follow-ing dissolution reactions, and use the appropriate Ksp and Kf values in Appendix C to calculate the equilibrium constant for each. (a) AgI in aqueous NaCN to form [Ag(CN)2]-501views
Textbook QuestionWrite a balanced net ionic equation for each of the follow-ing dissolution reactions, and use the appropriate Ksp and Kf values in Appendix C to calculate the equilibrium constant for each. (b) Cu(OH)2 in aqueous NH3 to form [Cu(NH3)4]2+516views
Textbook QuestionCalculate the molar solubility of AgI in: (a) Pure Water (b) 0.10 M NaCN: Kf for [Ag(CN)2]- is 3.0 x 10^201296views
Textbook QuestionCalculate the molar solubility of Cr(OH)3 in 0.50 M NaOH; Kf for Cr(OH)4- is 8 x 10^29.873views
Textbook QuestionCitric acid (H3Cit) can be used as a household cleaning agent to dissolve rust stains. The rust, represented as Fe(OH)3, dissolves because the citrate ion forms a soluble complex with Fe3+ (a) Using the equilibrium constants in Appendix C and Kf = 6.3 x 10^11 for Fe(Cit), calculate the equilibrium constant K for the reaction. (b) Calculate the molar solubility of Fe(OH)3 in 0.500 M solution of H3Cit.465views
Textbook QuestionCalculate the solubility of silver chloride in a solution that is 0.100 M in NH3.960views
Textbook QuestionCalculate the solubility of CuX in a solution that is 0.150 M in NaCN. Ksp for CuX is 1.27 * 10 - 36.621views