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If 120 mL of a 1.2 M glucose solution is diluted to 550.0 mL, what is the molarity of the diluted solution? Express your answer using two significant figures.

If 120 mL of a 1.2 M glucose solution is diluted to 550.0 mL, what is the molarity of the diluted solution? Express your answer using two significant figures.

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
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:** If 120 mL of a 1.2 M glucose solution is diluted to 550.0 mL, what is the molarity of the diluted solution? Express your answer using two significant figures. **Hints Available**: There is an option to view hints, which may be provided in an online setting to aid student comprehension. **Input and Submission:** - There is a textbox for entering the final answer, accompanied by a submit button for evaluation. --- **Explanation for Students:** To solve this problem, use the dilution formula: \[ C_1V_1 = C_2V_2 \] Where: - \( C_1 \) is the initial concentration (1.2 M) - \( V_1 \) is the initial volume (120 mL) - \( C_2 \) is the final concentration (unknown) - \( V_2 \) is the final volume (550.0 mL) Rearrange the equation to solve for \( C_2 \): \[ C_2 = \frac{C_1V_1}{V_2} \] Substitute the known values to find the molarity of the diluted solution.
Transcribed Image Text:**Question:** If 120 mL of a 1.2 M glucose solution is diluted to 550.0 mL, what is the molarity of the diluted solution? Express your answer using two significant figures. **Hints Available**: There is an option to view hints, which may be provided in an online setting to aid student comprehension. **Input and Submission:** - There is a textbox for entering the final answer, accompanied by a submit button for evaluation. --- **Explanation for Students:** To solve this problem, use the dilution formula: \[ C_1V_1 = C_2V_2 \] Where: - \( C_1 \) is the initial concentration (1.2 M) - \( V_1 \) is the initial volume (120 mL) - \( C_2 \) is the final concentration (unknown) - \( V_2 \) is the final volume (550.0 mL) Rearrange the equation to solve for \( C_2 \): \[ C_2 = \frac{C_1V_1}{V_2} \] Substitute the known values to find the molarity of the diluted solution.
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