Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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**Molarity Calculations (Fill-in All the Boxes)**

This table displays calculations of molarity involving different solutes, given their amounts in moles, grams, and the volume of their solutions.

| **Solute** | **Moles of Solute** | **Grams of Solute** | **Volume of Solution (L)** | **Concentration (Molarity, M = mole/L)** |
|------------|---------------------|---------------------|----------------------------|------------------------------------------|
| NaCl       | 3.00 moles          | **175 g**           | 0.500 L                    | **6.00 M**                               |
| NaCl       | 0.231 moles         | 13.5 g              | 0.150 L                    | **1.54 M**                               |
| NaCl       | 0.375 moles         | **21.9 g**          | 0.375 L                    | **1.00 M**                               |
| NaCl       | **0.0010 moles**    | 0.059 g             | 0.0033 L                   | **0.30 M**                               |
| KNO₃       | 1.57 moles          | **159 g**           | 2.04 L                     | **0.770 M**                              |
| KNO₃       | **0.0196 moles**    | 1.98 g              | 0.00980 L                  | **2.00 M**                               |
| KNO₃       | **0.0567 moles**    | 5.73 g              | 0.288 L                    | **0.197 M**                              |

**Note:** 

- The bold entries represent the information that is given, and the other entries denote the calculated values.
- Molarity is calculated using the formula: \( \text{Molarity} (M) = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \).
- This table serves as a practice for understanding and computing molarity in solution chemistry.
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Transcribed Image Text:**Molarity Calculations (Fill-in All the Boxes)** This table displays calculations of molarity involving different solutes, given their amounts in moles, grams, and the volume of their solutions. | **Solute** | **Moles of Solute** | **Grams of Solute** | **Volume of Solution (L)** | **Concentration (Molarity, M = mole/L)** | |------------|---------------------|---------------------|----------------------------|------------------------------------------| | NaCl | 3.00 moles | **175 g** | 0.500 L | **6.00 M** | | NaCl | 0.231 moles | 13.5 g | 0.150 L | **1.54 M** | | NaCl | 0.375 moles | **21.9 g** | 0.375 L | **1.00 M** | | NaCl | **0.0010 moles** | 0.059 g | 0.0033 L | **0.30 M** | | KNO₃ | 1.57 moles | **159 g** | 2.04 L | **0.770 M** | | KNO₃ | **0.0196 moles** | 1.98 g | 0.00980 L | **2.00 M** | | KNO₃ | **0.0567 moles** | 5.73 g | 0.288 L | **0.197 M** | **Note:** - The bold entries represent the information that is given, and the other entries denote the calculated values. - Molarity is calculated using the formula: \( \text{Molarity} (M) = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \). - This table serves as a practice for understanding and computing molarity in solution chemistry.
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molarity = mole of solutevolume of solution in L 

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