A solution contains 1.22x10-2 M zinc acetate and 9.43x10 M silver nitrate. Solid sodium phosphate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of phosphate ion when this precipitation first begins? [PO,]= M %3D
A solution contains 1.22x10-2 M zinc acetate and 9.43x10 M silver nitrate. Solid sodium phosphate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of phosphate ion when this precipitation first begins? [PO,]= M %3D
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
![**Title: Understanding Precipitation Reactions in Aqueous Solutions**
**Introduction:**
In this exercise, we explore the concept of precipitation reactions by working with an aqueous solution containing different dissolved salts. We'll be determining the compound that precipitates first when a new reagent is added and calculating the concentration at which this precipitation begins.
**Problem Statement:**
A solution contains \(1.22 \times 10^{-2}\) M zinc acetate and \(9.43 \times 10^{-3}\) M silver nitrate. Solid sodium phosphate is added slowly to this mixture.
**Questions and Analysis:**
**A. What is the formula of the substance that precipitates first?**
* Formula = ______________
**B. What is the concentration of the phosphate ion when this precipitation first begins?**
* \([ \text{PO}_4^{3-} ]\) = ______________ M
**Explanation and Approach:**
1. **Identify Possible Precipitates:**
- Given the ions in solution (\(\text{Zn}^{2+}\) from zinc acetate and \(\text{Ag}^+\) from silver nitrate), and the added \(\text{PO}_4^{3-}\) from sodium phosphate, we need to look at the solubility product constants (\(K_{sp}\)) for potential precipitation reactions:
- For \(\text{Zn}_3(\text{PO}_4)_2\): \(K_{sp}\)
- For \(\text{Ag}_3\text{PO}_4\): \(K_{sp}\)
- The compound with the lower \(K_{sp}\) will precipitate first.
2. **Calculate the Concentration of \(\text{PO}_4^{3-}\):**
- Use the \(K_{sp}\) values and the given concentrations to find out at what concentration the first compound will begin to precipitate.
- The formula needed to solve for \(\text{PO}_4^{3-}\) concentration when a compound starts to precipitate is derived from the equilibrium \(K_{sp}\) expressions.
**Conclusion:**
Fill in the blanks with the correct formula for the precipitate and the corresponding phosphate ion concentration using the above approach and data provided.
**Learning Objectives:**
- Understand the concept of solubility product constants (\(K_{sp}\)).
- Determine which compound precipitates first based on \(K_{sp](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77bfbc94-404c-40d5-8c71-b661b10ff379%2F4e1b68b4-80fd-44c5-b288-d95d342bc5a9%2Fv1bz6kc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Understanding Precipitation Reactions in Aqueous Solutions**
**Introduction:**
In this exercise, we explore the concept of precipitation reactions by working with an aqueous solution containing different dissolved salts. We'll be determining the compound that precipitates first when a new reagent is added and calculating the concentration at which this precipitation begins.
**Problem Statement:**
A solution contains \(1.22 \times 10^{-2}\) M zinc acetate and \(9.43 \times 10^{-3}\) M silver nitrate. Solid sodium phosphate is added slowly to this mixture.
**Questions and Analysis:**
**A. What is the formula of the substance that precipitates first?**
* Formula = ______________
**B. What is the concentration of the phosphate ion when this precipitation first begins?**
* \([ \text{PO}_4^{3-} ]\) = ______________ M
**Explanation and Approach:**
1. **Identify Possible Precipitates:**
- Given the ions in solution (\(\text{Zn}^{2+}\) from zinc acetate and \(\text{Ag}^+\) from silver nitrate), and the added \(\text{PO}_4^{3-}\) from sodium phosphate, we need to look at the solubility product constants (\(K_{sp}\)) for potential precipitation reactions:
- For \(\text{Zn}_3(\text{PO}_4)_2\): \(K_{sp}\)
- For \(\text{Ag}_3\text{PO}_4\): \(K_{sp}\)
- The compound with the lower \(K_{sp}\) will precipitate first.
2. **Calculate the Concentration of \(\text{PO}_4^{3-}\):**
- Use the \(K_{sp}\) values and the given concentrations to find out at what concentration the first compound will begin to precipitate.
- The formula needed to solve for \(\text{PO}_4^{3-}\) concentration when a compound starts to precipitate is derived from the equilibrium \(K_{sp}\) expressions.
**Conclusion:**
Fill in the blanks with the correct formula for the precipitate and the corresponding phosphate ion concentration using the above approach and data provided.
**Learning Objectives:**
- Understand the concept of solubility product constants (\(K_{sp}\)).
- Determine which compound precipitates first based on \(K_{sp
Transcribed Image Text:**Calculation of Calcium Ion Concentration in Solution**
*Solid sodium fluoride is slowly added to 175 mL of a calcium iodide solution until the concentration of fluoride ion is 0.0251 M. The maximum amount of calcium ion remaining in solution is _______ M.*
In this educational example, students are required to calculate the concentration of calcium ions remaining in a solution after sodium fluoride is added to a calcium iodide solution.
To solve for the concentration of calcium ions:
1. **Initial Information Given:**
- Volume of calcium iodide solution: 175 mL
- Concentration of fluoride ion: 0.0251 M
2. **Approach:**
- Utilize the solubility product constant (Ksp) for calcium fluoride to find the solubility equilibrium.
- Employ stoichiometry to relate the concentration of calcium ions to that of fluoride ions.
This exercise aids in understanding chemical equilibrium, particularly the solubility product constant concept. Students should have access to values like the Ksp of calcium fluoride to proceed with calculations. The objective is to determine the blank value for the calcium ion concentration at equilibrium.
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