### How to Calculate Dilution of a Solution**Question:**If 21 mL of 1.0 M NH₄Cl is used, what volume does it need to be diluted to in order to make a 0.12 M solution? (Give your answer in mL to zero decimal places)**Solution:**To solve this problem, we will use the concept of dilution, which can be calculated using the formula:\[ C_1 \times V_1 = C_2 \times V_2 \]Where:- \( C_1 \) is the concentration of the initial solution (1.0 M)- \( V_1 \) is the volume of the initial solution (21 mL)- \( C_2 \) is the desired concentration of the final solution (0.12 M)- \( V_2 \) is the volume of the final solution we need to findRearranging the equation to solve for \( V_2 \):\[ V_2 = \frac{C_1 \times V_1}{C_2} \]Now plug in the values:\[ V_2 = \frac{1.0 \text{ M} \times 21 \text{ mL}}{0.12 \text{ M}} \]\[ V_2 = \frac{21}{0.12} \]\[ V_2 = 175 \text{ mL} \]Therefore, you need to dilute the 21 mL of 1.0 M NH₄Cl to a final volume of **175 mL** to obtain a 0.12 M solution.

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If 21 mL of 1.0 M NH4Cl is used what volume does it need to be diluted to in order to make a 0.12 M solution? (give your answer in mL to zero decimal places)

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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