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solute moles of solute 3.00 moles NaCl NaCl .231 moles NaCl NaCl .375 moles .0010 moles KNO3 1.57 moles KNO3 .0196 moles KNO3 .0567 moles grams of solute 175 g 13.5 g 21.9 g .059 g 159 g 1.98 g 5.73 g volume of solution 0.500 L .150 L .375 L .0033 L 2.04 L .00980 L .288 L Concentration (Molarity, M=mole/L) 6.00 M 1.54 M 1.00 M 0.30 M .770 M 2.00 M .197 M

solute moles of solute 3.00 moles NaCl NaCl .231 moles NaCl NaCl .375 moles .0010 moles KNO3 1.57 moles KNO3 .0196 moles KNO3 .0567 moles grams of solute 175 g 13.5 g 21.9 g .059 g 159 g 1.98 g 5.73 g volume of solution 0.500 L .150 L .375 L .0033 L 2.04 L .00980 L .288 L Concentration (Molarity, M=mole/L) 6.00 M 1.54 M 1.00 M 0.30 M .770 M 2.00 M .197 M

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help the molarity to show work with this table

**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.
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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