Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Problem Statement:**
Calculate the mass, in grams, of **potassium iodide** that must be added to a **125-mL** volumetric flask in order to prepare **125 mL** of a **0.143 M** aqueous solution of the salt.
**Input Box:**
[_____] grams
---
**Explanation:**
This question aims to apply concepts from chemistry, specifically molarity and solution preparation. You are tasked to determine the mass of potassium iodide (KI) needed to create a specific molar concentration in a given volume of solution.
**Key Points:**
- **Molarity (M)** is defined as the number of moles of solute per liter of solution.
- The volume needed is 125 mL, which is equivalent to 0.125 L.
- The desired molarity of the potassium iodide solution is 0.143 M.
**Steps for Solution:**
1. Use the formula for molarity:
\[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}
\]
2. Calculate the number of moles of potassium iodide required:
\[
\text{moles of KI} = \text{Molarity} \times \text{Volume in liters}
\]
3. Convert moles to grams using the molar mass of potassium iodide (approximately 166 g/mol).
**Note:**
This exercise reinforces calculation skills in chemistry, specifically focusing on solution preparation and understanding molarity.](https://content.bartleby.com/qna-images/question/7b5abf62-aefa-4d0f-b576-4023d749f637/7be79a39-2433-43c6-9355-39e148e4bcb5/zrriit_processed.png)
Transcribed Image Text:**Problem Statement:**
Calculate the mass, in grams, of **potassium iodide** that must be added to a **125-mL** volumetric flask in order to prepare **125 mL** of a **0.143 M** aqueous solution of the salt.
**Input Box:**
[_____] grams
---
**Explanation:**
This question aims to apply concepts from chemistry, specifically molarity and solution preparation. You are tasked to determine the mass of potassium iodide (KI) needed to create a specific molar concentration in a given volume of solution.
**Key Points:**
- **Molarity (M)** is defined as the number of moles of solute per liter of solution.
- The volume needed is 125 mL, which is equivalent to 0.125 L.
- The desired molarity of the potassium iodide solution is 0.143 M.
**Steps for Solution:**
1. Use the formula for molarity:
\[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}
\]
2. Calculate the number of moles of potassium iodide required:
\[
\text{moles of KI} = \text{Molarity} \times \text{Volume in liters}
\]
3. Convert moles to grams using the molar mass of potassium iodide (approximately 166 g/mol).
**Note:**
This exercise reinforces calculation skills in chemistry, specifically focusing on solution preparation and understanding molarity.
![In the laboratory, a student adds 14.2 g of copper(II) iodide to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of copper(II) iodide, the copper(II) ion, and the iodide ion in the solution.
\[[\text{CuI}_2] = \_\_\_\_\ M\]
\[[\text{Cu}^{2+}] = \_\_\_\_\ M\]
\[[\text{I}^-] = \_\_\_\_\ M\]](https://content.bartleby.com/qna-images/question/7b5abf62-aefa-4d0f-b576-4023d749f637/7be79a39-2433-43c6-9355-39e148e4bcb5/mm3k94_processed.png)
Transcribed Image Text:In the laboratory, a student adds 14.2 g of copper(II) iodide to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of copper(II) iodide, the copper(II) ion, and the iodide ion in the solution.
\[[\text{CuI}_2] = \_\_\_\_\ M\]
\[[\text{Cu}^{2+}] = \_\_\_\_\ M\]
\[[\text{I}^-] = \_\_\_\_\ M\]
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