If 880 mL of water is added to 125.0 mL of a 0.770 M HBrO₄ solution what is the resulting molarity?

• A. 0.096 M
• B. 0.136 M
• C. 0.257 M
• D. 0.892 M
• E. 1.76 M

Answer: (A)

Verified step by step guidance

1. Start by understanding the concept of dilution, which involves adding solvent to a solution, decreasing the concentration of the solute.
2. Use the dilution formula: \( C_1V_1 = C_2V_2 \), where \( C_1 \) is the initial concentration, \( V_1 \) is the initial volume, \( C_2 \) is the final concentration, and \( V_2 \) is the final volume.
3. Identify the known values: \( C_1 = 0.770 \text{ M} \), \( V_1 = 125.0 \text{ mL} \), and the final volume \( V_2 = 125.0 \text{ mL} + 880 \text{ mL} \).
4. Substitute the known values into the dilution formula to solve for \( C_2 \): \( C_2 = \frac{C_1V_1}{V_2} \).
5. Calculate \( V_2 \) and then use the formula to find \( C_2 \), which is the resulting molarity of the solution after dilution.