**Problem Statement:**An aqueous solution has a molality of (4.9300x10^-1) m. The density of the solution is (1.42x10^0) g/mL and the solute has a molar mass of (1.660x10^2) g/mol.**Question:**What is the mole fraction of solute of this solution?**Instructions:**- Enter your answer in scientific notation with 3 significant figures. Do not include any units in your answer.- Do not round any intermediate calculations.- **Note:** Your answer is assumed to be reduced to the highest power possible. This exercise aims to calculate the mole fraction of a solute in an aqueous solution given its molality, density, and molar mass. This type of problem is commonly encountered in chemistry education to deepen understanding of solution concentration measurements. **Problem Statement:**An aqueous solution has a mass percent of solute of \( (3.570 \times 10^1) \% \). The density of the solution is \( (1.3900 \times 10^0) \) g/mL and the solute has a molar mass of \( (1.53 \times 10^2) \) g/mol.What is the molality of solute of this solution?**Instructions:**Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer.**Note:** Your answer is assumed to be reduced to the highest power possible.**Additional Guidelines:**- Do not round any intermediate calculations.

To calculate mole fraction of solute, we use formula : mole fraction of solute = ( moles of solute / moles of solute + moles of solvent ) So, we first need to calculate moles of solute and solvent . The work is shown as :Note : please upload other question again to get solved.

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An aqueous solution has a molality of (4.9300x10^-1) m. The density of the solution is (1.42x10^0) g/mL and the solute has a molar mass of (1.660x10^2) g/mol. What is the mole fraction of solute of this solution?

An aqueous solution has a molality of (4.9300x10^-1) m. The density of the solution is (1.42x10^0) g/mL and the solute has a molar mass of (1.660x10^2) g/mol. What is the mole fraction of solute of this solution?

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 has a molality of (4.9300x10^-1) m. The density of the solution is (1.42x10^0) g/mL and the solute has a molar mass of (1.660x10^2) g/mol.

**Question:**

What is the mole fraction of solute of this solution?

**Instructions:**

- Enter your answer in scientific notation with 3 significant figures. Do not include any units in your answer.
- Do not round any intermediate calculations.
- **Note:** Your answer is assumed to be reduced to the highest power possible.

This exercise aims to calculate the mole fraction of a solute in an aqueous solution given its molality, density, and molar mass. This type of problem is commonly encountered in chemistry education to deepen understanding of solution concentration measurements.

**Problem Statement:**

An aqueous solution has a mass percent of solute of \( (3.570 \times 10^1) \% \). The density of the solution is \( (1.3900 \times 10^0) \) g/mL and the solute has a molar mass of \( (1.53 \times 10^2) \) g/mol.

What is the molality of solute of this solution?

**Instructions:**

Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer.

**Note:** Your answer is assumed to be reduced to the highest power possible.

**Additional Guidelines:**

- Do not round any intermediate calculations.

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