**Topic: Precipitation and Complex Ion Formation in Silver (I) Reactions****4. Silver (I) Behavior in Aqueous Solutions**Silver (I) ions can form either a precipitate or a complex ion when mixed with sodium chloride. The outcome depends on the concentration of chloride ions present in the solution. Below are key questions and exercises to understand this chemical behavior:a. **Complex Ion and Precipitate Formation** - Write the chemical equations that illustrate the formation of a complex ion and a precipitate when silver (I) ions react with chloride ions.b. **Chloride Ion Concentration for Precipitate Formation** - Determine the necessary concentration of Cl⁻ ions to form a precipitate of AgCl (s) given [Ag⁺] = 0.1 M and [NaCl] = 1 M. Provide your answer in molar concentration.c. **Chloride Ion Concentration for Complex Ion Formation** - Calculate the concentration of Cl⁻ ions required to form a complex ion of [AgCl₂]⁻ (aq) with a 0.2 M complex concentration. Assume [Ag⁺] = 0.1 M. Your answer should also be in molar concentration.d. **Application in Qualitative Analysis** - Discuss how the knowledge of silver ion reactions with chloride can be applied to develop a qualitative analysis separation scheme.e. **Other Ion-Pair Scenarios** - Utilize the K_sp and K_f values from your lab manual to provide two additional examples where both a precipitate and a complex ion might simultaneously form.This exercise will help in understanding concepts of solubility product (K_sp), formation constant (K_f), and their applications in predicting the behavior of ions in solution.

Note - Since you have asked a question with multiple sub-parts, we will solve the first three sub-parts for you. To get the rest of the sub-parts solved, please repost the complete question specifying the sub-parts to be solved.4 a. The reaction for the formation of the precipitate is given below : Ag-(aq) + Cl-(aq) → AgCl(s) (white ppt.) The reaction for the formation of the complex ion is given below : Ag+(s) + 2Cl-(aq) → [AgCl2]-(aq) b. Now, given that : Ag+=0.1 MNaCl=1 M The Ksp for AgCl is 1.80 x 10-10. Now, the expression for Ksp can be given as : Ksp=Ag+Cl-1.80×10-10=0.1Cl-Thus,[Cl-]=1.80×10-9c. The Kf for [AgCl2]- is 1.80 x 105. The ICE table for the formation of [AgCl2]- is given below : Ag+ + 2Cl- → AgCl2-Initial concentration (in M) 0.1 0 0Change (in M) -x 2x +2xAt equilibrium (in M) (0.1-x) 2x 2x Now, K=Kf×KspNow, since Kf=AgCl2-Ag+Cl-2 and Ksp=Ag+Cl-Thus,K=AgCl2-Ag+Cl-2×Ag+Cl-=1.8×105×1.8×10-10So, K=AgCl2-Cl-=3.24×10-5Thus, [Cl-]=3.24×10-5M

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4. Silver (I) can form a precipitate and/or a complex ion when it is mixed with sodium chloride, depending on the concentration of chloride ion present in the solution. a. Write the reaction for the formation of the complex ion and the reaction for the formation of the precipitate b. What concentration of Cl is required to form a precipitate of AgCl (s) ([Ag*]=0.1M; [NaCl] =1M). Your answer shoould be listed as a molar concentration. c. What concentration of Cl is required to form a complex ion of [AgCl,] (aq) whose Assume the concentration of [Ag*] is 0.1 M. Your answer concentration is 0.2 M should be listed as a molar concentration.

4. Silver (I) can form a precipitate and/or a complex ion when it is mixed with sodium chloride, depending on the concentration of chloride ion present in the solution. a. Write the reaction for the formation of the complex ion and the reaction for the formation of the precipitate b. What concentration of Cl is required to form a precipitate of AgCl (s) ([Ag]=0.1M; [NaCl] =1M). Your answer shoould be listed as a molar concentration. c. What concentration of Cl is required to form a complex ion of [AgCl,] (aq) whose Assume the concentration of [Ag] is 0.1 M. Your answer concentration is 0.2 M should be listed as a molar concentration.

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...

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Question

**Topic: Precipitation and Complex Ion Formation in Silver (I) Reactions**

**4. Silver (I) Behavior in Aqueous Solutions**

Silver (I) ions can form either a precipitate or a complex ion when mixed with sodium chloride. The outcome depends on the concentration of chloride ions present in the solution. Below are key questions and exercises to understand this chemical behavior:

a. **Complex Ion and Precipitate Formation**
- Write the chemical equations that illustrate the formation of a complex ion and a precipitate when silver (I) ions react with chloride ions.

b. **Chloride Ion Concentration for Precipitate Formation**
- Determine the necessary concentration of Cl⁻ ions to form a precipitate of AgCl (s) given [Ag⁺] = 0.1 M and [NaCl] = 1 M. Provide your answer in molar concentration.

c. **Chloride Ion Concentration for Complex Ion Formation**
- Calculate the concentration of Cl⁻ ions required to form a complex ion of [AgCl₂]⁻ (aq) with a 0.2 M complex concentration. Assume [Ag⁺] = 0.1 M. Your answer should also be in molar concentration.

d. **Application in Qualitative Analysis**
- Discuss how the knowledge of silver ion reactions with chloride can be applied to develop a qualitative analysis separation scheme.

e. **Other Ion-Pair Scenarios**
- Utilize the K_sp and K_f values from your lab manual to provide two additional examples where both a precipitate and a complex ion might simultaneously form.

This exercise will help in understanding concepts of solubility product (K_sp), formation constant (K_f), and their applications in predicting the behavior of ions in solution.

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