**Problem Statement:**An aqueous solution is 30.0% by mass ammonia, \( \text{NH}_3 \), and has a density of 0.892 g/mL.The molarity of ammonia in the solution is \(\underline{\hspace{3cm}}\) M.**Analysis:**This problem involves finding the molarity of an ammonia solution given its percentage by mass and density. Molarity is a measure of concentration equivalent to the number of moles of solute per liter of solution. Given the data, you can calculate the molarity using the following steps:1. **Calculate the Mass of Solution:** - Assume 100 g of solution (this simplifies calculations using the percentage by mass). - 30% by mass ammonia means 30 g of \( \text{NH}_3 \).2. **Volume of Solution:** - Use the density to calculate the volume of 100 g of solution. - Density = Mass/Volume, so Volume = Mass/Density. - Volume = 100 g / 0.892 g/mL = 112.13 mL - Convert volume to liters: 112.13 mL = 0.11213 L.3. **Calculate Moles of Ammonia:** - Use the molar mass of \( \text{NH}_3 \) (17.03 g/mol) to find the number of moles. - Moles of \( \text{NH}_3 \) = 30 g / 17.03 g/mol = 1.76 mol.4. **Calculate Molarity:** - Molarity = Moles of solute / Volume of solution in liters. - Molarity = 1.76 mol / 0.11213 L = 15.69 M.Therefore, the molarity of ammonia in the solution is approximately 15.69 M.

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An aqueous solution is 30.0% by mass ammonia, NH3, and has a density of 0.892 g/mL. The molarity of ammonia in the solution is M.

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

**Problem Statement:**

An aqueous solution is 30.0% by mass ammonia, \( \text{NH}_3 \), and has a density of 0.892 g/mL.

The molarity of ammonia in the solution is \(\underline{\hspace{3cm}}\) M.

**Analysis:**

This problem involves finding the molarity of an ammonia solution given its percentage by mass and density. Molarity is a measure of concentration equivalent to the number of moles of solute per liter of solution. Given the data, you can calculate the molarity using the following steps:

1. **Calculate the Mass of Solution:**
- Assume 100 g of solution (this simplifies calculations using the percentage by mass).
- 30% by mass ammonia means 30 g of \( \text{NH}_3 \).

2. **Volume of Solution:**
- Use the density to calculate the volume of 100 g of solution.
- Density = Mass/Volume, so Volume = Mass/Density.
- Volume = 100 g / 0.892 g/mL = 112.13 mL
- Convert volume to liters: 112.13 mL = 0.11213 L.

3. **Calculate Moles of Ammonia:**
- Use the molar mass of \( \text{NH}_3 \) (17.03 g/mol) to find the number of moles.
- Moles of \( \text{NH}_3 \) = 30 g / 17.03 g/mol = 1.76 mol.

4. **Calculate Molarity:**
- Molarity = Moles of solute / Volume of solution in liters.
- Molarity = 1.76 mol / 0.11213 L = 15.69 M.

Therefore, the molarity of ammonia in the solution is approximately 15.69 M.

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