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Chemistry (7th Edition)
- What is a complex ion? The stepwise formation constants for the complex ion Cu(NH3)42+ are K1 1 103, K2 1 104, K3 = 1 103, and K4 1 103. Write the reactions that refer to each of these formation constants. Given that the values of the formation constants are large, what can you deduce about the equilibrium concentration of Cu(NH3)42+ versus the equilibrium concentration of Cu2+?arrow_forwardSolid Pbl2 (Ksp = 9.8 109) is placed in a beaker of water. After a period of time, the lead(II) concentration is measured and found to be 1.1 103 M. Has the system reached equilibrium? That is, is the solution saturated? If not, will more Pbl2 dissolve?arrow_forwardIn the presence of NH3, Cu2+ forms the complex ion Cu(NH3)42+. If the equilibrium concentrations of Cu2+ and Cu(NH3)42+ are 1.8 1017 M and 1.0 103 M, respectively, in a 1.5-M NH3 solution, calculate the value for the overall formation constant of Cu(NH3)42+. Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)Koverall=?arrow_forward
- At 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.arrow_forward1. What is the equilibrium constant for the process of dissolving Agl by the addition of aqueous NaCN? Ksp for Agl is 8.5 × 10−17, and Kr for [Ag(CN)2]− is 1.3 × 1021. 6.5 × 10−4 8.7 × 104 1.1 × 105arrow_forwardAluminum hydroxide reacts with an excess of hydroxide ions to form the complex ion Al(OH)4-. (a) Write an equation for this reaction. (b) Calculate K. (c) Determine the solubility of Al(OH)3 (in mol/L) at pH 12.0.arrow_forward
- The solubility of zinc oxalate, ZnC2O4, in 0.0150 M ammonia is 3.6 104 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for zinc oxalate is 1.5 109, what must be the zinc-ion concentration in the solution? Now calculate the formation constant for the complex ion Zn(NH3)42+.arrow_forwardSometimes equilibria fur complex ions are described in terms of dissociation constants. Kd . For the complex ion AlF63- the dissociation reaction is: AlF63Al3++6F and Kd=[Al3+][F]6[AlF63]=21024 Calculate the value of the formation constant, Kf, for AlF63-.arrow_forwardThe solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.arrow_forward
- Solutions of sodium thiosulfate are used to dissolve unexposed AgBr (Ksp = 5.0 1013) in the developing process for black-and-white film. What mass of AgBr can dissolve in 1.00 L of 0.500 M Na2S2O3? Ag+ reacts with S2O32 to form a complex ion: Ag+(aq)+2S2O32(aq)Ag(S2O3)23(aq)K=2.91013arrow_forwardIn the presence of CN, Fe3+ forms the complex ion Fe(CN)63. The equilibrium concentrations of Fe3+ and Fe(CN)63 are 8.5 1040 M and 1.5 103 M, respectively, in a 0.11-M KCN solution. Calculate the value for the overall formation constant of Fe(CN)63. Fe3+(aq)+6CN(aq)Fe(CN)63(aq)Koverall=?arrow_forwardTooth enamel is composed of the mineral hydroxyapatite. The Ksp of hydroxyapatite, Ca5(PO4)3OH, is 6.8 1037. Calculate the solubility of hydroxyapatite in pure water in moles per liter. How is the solubility of hydroxyapatite affected by adding acid? When hydroxyapatite is treated with fluoride, the mineral fluorapatite, Ca5(PO4)3F, forms. The Ksp of this substance is 1 1060. Calculate the solubility of fluorapatite in water. How do these calculations provide a rationale for the fluoridation of drinking water?arrow_forward
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