In aqueous solution the Ag ion forms a complex with two cyanide anions.Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemicalequation for the last step in the formation of the complex.K₂=☐Write the Last Step:Last Step:☑ロ→ロ For the aqueous [Ag(CN)2] complex K₁ = 1.26 × 1021 at 25 °C.+Suppose equal volumes of 0.0038M AgNO3 solution and 0.20M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Ag" ion.Round your answer to 2 significant digits.Шмx10×

Answered: In aqueous solution the Ag ion forms a…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 74QRT

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Similar questions

When 5 M ammonia is added to a solution containing Cu(OH)2(s), the precipitate will eventually dissolve in solution. Why? If 5 M HNO3 is then added, the Cu(OH)2 precipitate re-forms. Why? In general, what effect does the ability of a cation to form a complex ion have on the solubility of salts containing that cation?
Write the chemical equation for the formation of each complex ion and write its formation constant expression, (a) [Ag(CN)2] (b) [Cd(NH3)4]2+
Sufficient sodium cyanide, NaCN, was added to 0.015 M silver nitrate, AgNO3, to give a solution that was initially 0.108 M in cyanide ion, CN. What is the concentration of silver ion, Ag+, in this solution after Ag(CN)2 forms? The formation constant Kf for the complex ion Ag(CN)2 is 5.6 1018.
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+?
The solubility of Mg(OH)2 in water is approximately 9.6 mg/L at a given temperature. Calculate the Ksp of magnesium hydroxide. Calculate the hydroxide concentration needed to precipitate Mg2+ ions such that no more than 5.0 μg Mg2+ per liter remains in the solution.
The active ingredient of Pepto-Bismol is the compound bismuth subsalicylate, which undergoes the following dissociation when added to water: C7H5BiO4(s)+H2O(l)C7H4O32(aq)+Bi3+(aq)+OH(aq)K=? If the maximum amount of bismuth subsalicylate that reacts by this reaction is 3.2 1019 mol/L, calculate the equilibrium constant for the preceding reaction.
What is the Ksp expression for silver carbonate? (a) Ksp[Ag+][CO32] (b) Ksp[Ag+]2[CO32] (c) Ksp[Ag+][CO32]2
Sometimes 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-.
Suppose that solid AgCl and AgI are placed in 1.0 L water in separate beakers. Some, but not all, of each solid compound dissolves. In which beaker is the silver ion concentration, [Ag+], larger? Does the volume of water in which each compound dissolves affect the equilibrium concentration?
The average normal concentration of Ca2+ in urine is 5.33 g/L. Calculate the concentration of oxalate needed to precipitate calcium oxalate to initiate formation of a kidney stone. Ksp of calcium oxalate = 2.3 × 10−9. Calculate the minimum phosphate concentration that would precipitate a calcium phosphate kidney stone. Ksp of calcium phosphate = 2.0 × 10−29.
Write equations for the stepwise formation of each of the following complex ions. a. CoF63 b. Zn(NH3)42+
You have a solution that has a lead(II) ion concentration of 0.0012 M. If enough soluble chloride-containing salt is added so that the Cl concentration is 0.010 M, will PbCl2 precipitate?

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