34. At 25 C, only 1.9 g CaSO4 will dissolve in 2.00 L of water. What is the equilibrium constant for the reaction below? CaSO4(s) Ca²+(aq) + SO4²-(aq) a. b. C. d. e. 4.9 x 10-5 1.9 x 104 1.4 x 10-² 7.0 x 10-3 0.90 Letter answer to question #34:
34. At 25 C, only 1.9 g CaSO4 will dissolve in 2.00 L of water. What is the equilibrium constant for the reaction below? CaSO4(s) Ca²+(aq) + SO4²-(aq) a. b. C. d. e. 4.9 x 10-5 1.9 x 104 1.4 x 10-² 7.0 x 10-3 0.90 Letter answer to question #34:
Chemistry
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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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![### Solubility and Equilibrium Constants
**Question 34:** At 25°C, only 1.9 g of CaSO₄ (calcium sulfate) will dissolve in 2.00 L of water. What is the equilibrium constant for the reaction below?
\[ \text{CaSO}_4(s) \leftrightarrow \text{Ca}^{2+}(aq) + \text{SO}_4^{2-}(aq) \]
**Options:**
a. \( 4.9 \times 10^{-5} \)
b. \( 1.9 \times 10^{-4} \)
c. \( 1.4 \times 10^{-2} \)
d. \( 7.0 \times 10^{-3} \)
e. 0.90
**Answer Box:**
Letter answer to question #34: __________
---
**Explanation:**
This question involves calculating the equilibrium constant (also known as the solubility product or \( K_{sp} \)) for the dissolution reaction of calcium sulfate (\( \text{CaSO}_4 \)).
**Steps to Solve:**
1. Determine the molar mass of CaSO₄.
2. Convert 1.9 g of CaSO₄ into moles.
3. Calculate the molar concentration of \( \text{Ca}^{2+} \) and \( \text{SO}_4^{2-} \) when the 1.9 g of CaSO₄ is dissolved in 2.00 L of water.
4. Use the calculated concentrations to determine the equilibrium constant \( K_{sp} \).
**Chemical Equation:**
\[ \text{CaSO}_4(s) \leftrightarrow \text{Ca}^{2+}(aq) + \text{SO}_4^{2-}(aq) \]
\( K_{sp} = [ \text{Ca}^{2+} ][ \text{SO}_4^{2-} ] \)
**Given Data:**
- Mass of CaSO₄: 1.9 g
- Volume of water: 2.00 L
- Temperature: 25°C
**Calculation Considerations:**
- Molar mass of CaSO₄ is required for conversion from grams to moles.
- Concentrations of \( \text{Ca}^{2+} \) and \(](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc2b26743-f936-4d82-936f-53393b21669b%2Ff4c8cadf-b985-48ed-92bf-ec3d919004d1%2Fokgloj7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Solubility and Equilibrium Constants
**Question 34:** At 25°C, only 1.9 g of CaSO₄ (calcium sulfate) will dissolve in 2.00 L of water. What is the equilibrium constant for the reaction below?
\[ \text{CaSO}_4(s) \leftrightarrow \text{Ca}^{2+}(aq) + \text{SO}_4^{2-}(aq) \]
**Options:**
a. \( 4.9 \times 10^{-5} \)
b. \( 1.9 \times 10^{-4} \)
c. \( 1.4 \times 10^{-2} \)
d. \( 7.0 \times 10^{-3} \)
e. 0.90
**Answer Box:**
Letter answer to question #34: __________
---
**Explanation:**
This question involves calculating the equilibrium constant (also known as the solubility product or \( K_{sp} \)) for the dissolution reaction of calcium sulfate (\( \text{CaSO}_4 \)).
**Steps to Solve:**
1. Determine the molar mass of CaSO₄.
2. Convert 1.9 g of CaSO₄ into moles.
3. Calculate the molar concentration of \( \text{Ca}^{2+} \) and \( \text{SO}_4^{2-} \) when the 1.9 g of CaSO₄ is dissolved in 2.00 L of water.
4. Use the calculated concentrations to determine the equilibrium constant \( K_{sp} \).
**Chemical Equation:**
\[ \text{CaSO}_4(s) \leftrightarrow \text{Ca}^{2+}(aq) + \text{SO}_4^{2-}(aq) \]
\( K_{sp} = [ \text{Ca}^{2+} ][ \text{SO}_4^{2-} ] \)
**Given Data:**
- Mass of CaSO₄: 1.9 g
- Volume of water: 2.00 L
- Temperature: 25°C
**Calculation Considerations:**
- Molar mass of CaSO₄ is required for conversion from grams to moles.
- Concentrations of \( \text{Ca}^{2+} \) and \(
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