Multiple Choice
What is the molarity (M) of a solution prepared by diluting 125 mL of 0.500 M H₂SO₄ to 375 mL?
6. Chemical Quantities & Aqueous Reactions
Dilutions
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During a serial dilution, you use 15.0 mL of a standard solution and dilute it to 1.35 L twice. What is the final concentration if the standard solution had an initial concentration of 0.500 M?
A
0.0185 M
B
0.250 M
C
0.00278 M
D
0.0370 M
Verified step by step guidance1
Start by understanding the concept of serial dilution. In a serial dilution, a solution is diluted multiple times, and each dilution step reduces the concentration of the solute in the solution.
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 after dilution.
For the first dilution, substitute the values: \( C_1 = 0.500 \text{ M} \), \( V_1 = 15.0 \text{ mL} \), and \( V_2 = 1.35 \text{ L} \). Convert \( V_1 \) to liters by dividing by 1000, so \( V_1 = 0.015 \text{ L} \). Solve for \( C_2 \) using the formula.
After finding \( C_2 \) from the first dilution, use this concentration as \( C_1 \) for the second dilution. Again, apply the dilution formula with \( V_1 = 1.35 \text{ L} \) and \( V_2 = 1.35 \text{ L} \) for the second dilution.
Calculate the final concentration \( C_2 \) after the second dilution using the values obtained from the first dilution step. This will give you the final concentration of the solution after both dilutions.
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