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Question 15 (2 points) Saved \( \equiv \) Listen What molarity (M) of copper sulfate is made from diluting 27.9 mL of 8.3 M copper sulfate a final volume of 225.0 mL ? (answer to 1 decimal place)

Ask by Ayala Cummings. in the United States
Feb 26,2025

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The final molarity is approximately 1.0 M.

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To calculate the molarity of copper sulfate after dilution, you can use the dilution formula: \( M_1 V_1 = M_2 V_2 \), where \( M_1 \) is the initial molarity, \( V_1 \) is the initial volume, \( M_2 \) is the final molarity, and \( V_2 \) is the final volume. Given: - \( M_1 = 8.3 \, M \) - \( V_1 = 27.9 \, mL \) - \( V_2 = 225.0 \, mL \) First, convert volumes to liters: - \( V_1 = 0.0279 \, L \) - \( V_2 = 0.2250 \, L \) Now substitute the values into the formula: \[ 8.3 \times 0.0279 = M_2 \times 0.2250 \] Calculating the left side: \[ 0.23137 = M_2 \times 0.2250 \] Now solve for \( M_2 \): \[ M_2 = \frac{0.23137}{0.2250} \approx 1.0305 \, M \] Finally, rounding to one decimal place: **The molarity of the diluted copper sulfate solution is approximately 1.0 M.**

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