**Topic: Solubility and Complex Ion Formation**Consider the insoluble compound **silver chloride, AgCl**. The silver ion also forms a complex with **cyanide ions**. Write a net ionic equation to show why the solubility of AgCl(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References.For \( \text{Ag(CN)}_2^- \), \( K_f = 1.3 \times 10^{21} \). Be sure to specify states such as (aq) or (s).\[\boxed{} + \boxed{} \rightarrow \boxed{} + \boxed{}\]\[K = \boxed{}\]**Explanation:**In this problem, we are exploring the interaction between the insoluble compound silver chloride and cyanide ions, which lead to increased solubility of AgCl when cyanide is present. The formation of the complex ion \( \text{Ag(CN)}_2^- \) is characterized by a very high formation constant \( K_f \), indicating a strong tendency to form in solution.**Key Steps:**1. **Identify the static components:** - AgCl (s) as the insoluble compound. - \( \text{CN}^- \) as the complexing agent.2. **Write the net ionic equation:** - Separate the dissolution and complex formation reactions.3. **Calculate the equilibrium constant:** - Utilize the \( K_{sp} \) and \( K_f \) provided to determine the overall equilibrium constant for the process.Understanding these procedures is crucial for students studying chemical equilibria, as it demonstrates how solubility can be manipulated through complex ion formation.

We need to write the net ionic equation and the equilibrium constant for the given reaction. We are…

Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgCl(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ag(CN)2, Kf = 1.3x1021. Be sure to specify states such as (aq) or (s). K= + +

Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgCl(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ag(CN)2, Kf = 1.3x1021. Be sure to specify states such as (aq) or (s). K= + +

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+, K = 6.8x1012. Be sure to specify states such as (aq) or (s). K = [Review Topics] [References] Use the References to access important values if needed for this question. Submit Answer ? + Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support Previous Email Instructor Next> Save and Exit
Consider the insoluble compound zine hydroxide , Zn(OH), . The zince ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Zn(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH,)," , K= 2.9x10°. Be sure to specify states such as (aq) or (s).
The equilibrium constant, Ke, for the following reaction is 1.89×10-2 at 718 K. 2HI(g) H,(g) + I2(g) Calculate K. at this temperature for: H2(g) + I2(g) 2HI(g) Ke
please provide detailed solution and give the explanation of the concept.... A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?
Initially, 0.660 mol of A is present in a 1.50 L solution. 2 A(aq) = 2 B(aq) + C(aq) At equilibrium, 0.150 mol of C is present. Calculate K. K =
The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O O
Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×10¹5. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 2 more group attempts remaining
At 25 °C, an aqueous solution has an equilibrium concentration of 0.00217 M for a generic cation, A+(aq), and 0.00109 M for a generic anion, B2−(aq). What is the equilibrium constant, ?sp, of the generic salt A2B(s)?
A student ran the following reaction in the laboratory at 672 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student determines that an aqueous solution that contains 0.474 M potassium hypochlorite and 0.180 M hypochlorous acid, also has an H30* concentration of 1.89x10-8 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HCIO(aq) + H2O =H30*(aq) + ClO(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K
You are on a new planet and discover a substance, Z2O that undergoes autoionization just like water on Earth. Z2O + Z2O ⇌ Z3O+ + OZ– Through a series of experiments, you determine the equilibrium constant (Kx) for this autoionization reaction at various temperatures. The value of Keq at 25.1ºC is 6.6 x 10-13. What is the pZ of the pure substance at this temperature? (pZ = -log(Z3O+) Report your answer to the hundreths place.
A solution is 0.085 M potassium carbonate, K>CO.. Determine the pH of the solution and the equilibrium concentration (in mol L'') for each of the indicated ions. pH = [K°]eq = M [HCO3 leg = _M [CO,?leq = M The compound gold (III) iodide, Aul3, has Ksp=1.0 x 1046, and a molar mass of 577.67 g. Write the net ionic reaction for this compound dissolving in water. What are the molar concentrations of Au3* and of I- in a saturated solution of gold (III) iodide? What is the solubility (in g/ L) of the compound Aul3 in pure water? Reaction: [Au3*) = M M Pure water solubility_ g of Aul3 per liter.