An aqueous solution has a mole fraction of solute of \( (2.840 \times 10^{-2}) \). The density of the solution is \( (1.170 \times 10^{0}) \) g/mL and the solute has a molar mass of \( (8.11 \times 10^{1}) \) g/mol.**What is the Molarity of solute of this solution?**Enter your answer in scientific notation with 3 sig figs. 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. **Calculation of Molality from Mass Percent, Density, and Molar Mass**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 the solute in 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.**Diagrams:**The image contains handwritten elements that do not contribute to the numerical or conceptual information provided about the problem, as they appear to be non-relevant scribbles or marks.

Since you have mentioned the second question as 4th one so I am going to solve that as per the…

An aqueous solution has a mass percent of solute of (3.570x10^1)%. The density of the solution is (1.3900x10^0) g/mL and the solute has a molar mass of (1.53x10^2) g/mol. What is the molality of solute of this solution?

An aqueous solution has a mass percent of solute of (3.570x10^1)%. The density of the solution is (1.3900x10^0) g/mL and the solute has a molar mass of (1.53x10^2) g/mol. What is the molality 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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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

An aqueous solution has a mole fraction of solute of \( (2.840 \times 10^{-2}) \). The density of the solution is \( (1.170 \times 10^{0}) \) g/mL and the solute has a molar mass of \( (8.11 \times 10^{1}) \) g/mol.

**What is the Molarity of solute of this solution?**

Enter your answer in scientific notation with 3 sig figs. 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.

**Calculation of Molality from Mass Percent, Density, and Molar Mass**

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 the solute in 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.

**Diagrams:**
The image contains handwritten elements that do not contribute to the numerical or conceptual information provided about the problem, as they appear to be non-relevant scribbles or marks.

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