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
How do I calculate the [OH] with the given data? Do you start by calculating moles of HCL and then find calcium hydroxide's concentration?
![### Experiment: Determination of Solubility Product Constant (Ksp) of Ca(OH)₂
In this experiment, you will utilize the knowledge gained from previous titration experiments. By obtaining a sample of Ca(OH)₂ solution from a saturated solution, you can determine the solubility product constant, Ksp, by knowing the concentration of one of the ions present.
#### Procedure
In this case, it is easier to determine the molar concentration of the hydroxide ions by titration. Recall that at equilibrium, the dissociation of calcium hydroxide in water produces 2 hydroxide ions for every calcium ion generated, represented by the following chemical equation:
\[ \text{Ca(OH)}_2 (\text{s}) \leftrightarrows \text{Ca}^{2+} + 2 \text{OH}^{-} \]
The hydroxide ions in the saturated solution are titrated using a standard solution of HCl. At the titration endpoint, the volume of HCl delivered is used to calculate the molarity of hydroxide ions in the 25 mL sample withdrawn using a pipette.
#### Calculation
From the molar concentration of \(\text{OH}^{-}\) ions, the concentration of \(\text{Ca}^{2+}\) ions is obtained by dividing the hydroxide molar concentration by 2. The Ksp of calcium hydroxide is then calculated using the following expression:
\[ \text{Ksp} = \left[ \text{Ca}^{2+} \right] \left[ \text{OH}^{-} \right]^2 \]
This expression allows you to determine the solubility product constant of calcium hydroxide from the concentrations of the ions in the solution.
By following this method, you can accurately calculate Ksp, thus understanding the solubility properties of calcium hydroxide in water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6aff1de3-5b31-4aa8-8b8b-26a60a52c3ab%2F3bd46a90-4bfe-439d-8925-0e01c481975b%2F9qx5gc.png&w=3840&q=75)
Transcribed Image Text:### Experiment: Determination of Solubility Product Constant (Ksp) of Ca(OH)₂
In this experiment, you will utilize the knowledge gained from previous titration experiments. By obtaining a sample of Ca(OH)₂ solution from a saturated solution, you can determine the solubility product constant, Ksp, by knowing the concentration of one of the ions present.
#### Procedure
In this case, it is easier to determine the molar concentration of the hydroxide ions by titration. Recall that at equilibrium, the dissociation of calcium hydroxide in water produces 2 hydroxide ions for every calcium ion generated, represented by the following chemical equation:
\[ \text{Ca(OH)}_2 (\text{s}) \leftrightarrows \text{Ca}^{2+} + 2 \text{OH}^{-} \]
The hydroxide ions in the saturated solution are titrated using a standard solution of HCl. At the titration endpoint, the volume of HCl delivered is used to calculate the molarity of hydroxide ions in the 25 mL sample withdrawn using a pipette.
#### Calculation
From the molar concentration of \(\text{OH}^{-}\) ions, the concentration of \(\text{Ca}^{2+}\) ions is obtained by dividing the hydroxide molar concentration by 2. The Ksp of calcium hydroxide is then calculated using the following expression:
\[ \text{Ksp} = \left[ \text{Ca}^{2+} \right] \left[ \text{OH}^{-} \right]^2 \]
This expression allows you to determine the solubility product constant of calcium hydroxide from the concentrations of the ions in the solution.
By following this method, you can accurately calculate Ksp, thus understanding the solubility properties of calcium hydroxide in water.
![### Experiment 1 Data
The following table presents the data collected during Experiment 1, including the volume of calcium hydroxide (Ca(OH)₂) pipetted, the concentration of the hydrochloric acid (HCl) standard, and the volume of HCl used.
| Parameter | Experiment 1 |
|-----------------------------------------|--------------|
| Volume of Ca(OH)₂ Pipetted (mL) | 25.0 |
| [HCl] Standard (M) | 0.1081 |
| Volume of HCl Used (mL) | 10.40 |
#### Explanation and Usage
- **Volume of Ca(OH)₂ Pipetted (mL):** The measurement of calcium hydroxide solution that was dispensed for the titration process, recorded at 25.0 mL.
- **[HCl] Standard (M):** The molarity or concentration of the hydrochloric acid standard used in the experiment, noted to be 0.1081 M.
- **Volume of HCl Used (mL):** The volume of HCl required to reach the endpoint of the titration, measured to be 10.40 mL.
These values are critical for calculating the concentration of the unknown solution and for understanding the stoichiometry of the reaction between Ca(OH)₂ and HCl.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6aff1de3-5b31-4aa8-8b8b-26a60a52c3ab%2F3bd46a90-4bfe-439d-8925-0e01c481975b%2F8pfbksm.png&w=3840&q=75)
Transcribed Image Text:### Experiment 1 Data
The following table presents the data collected during Experiment 1, including the volume of calcium hydroxide (Ca(OH)₂) pipetted, the concentration of the hydrochloric acid (HCl) standard, and the volume of HCl used.
| Parameter | Experiment 1 |
|-----------------------------------------|--------------|
| Volume of Ca(OH)₂ Pipetted (mL) | 25.0 |
| [HCl] Standard (M) | 0.1081 |
| Volume of HCl Used (mL) | 10.40 |
#### Explanation and Usage
- **Volume of Ca(OH)₂ Pipetted (mL):** The measurement of calcium hydroxide solution that was dispensed for the titration process, recorded at 25.0 mL.
- **[HCl] Standard (M):** The molarity or concentration of the hydrochloric acid standard used in the experiment, noted to be 0.1081 M.
- **Volume of HCl Used (mL):** The volume of HCl required to reach the endpoint of the titration, measured to be 10.40 mL.
These values are critical for calculating the concentration of the unknown solution and for understanding the stoichiometry of the reaction between Ca(OH)₂ and HCl.
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