Multiple Choice
How many milliliters of 0.0500 M AgNO_3 solution are required to prepare 15.0 mL of a 0.0100 M AgNO_3 solution?
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6. Chemical Quantities & Aqueous Reactions
Dilutions
Multiple Choice
To what final volume would 100 mL of 5.0 M KCl have to be diluted in order to make a solution that is 0.54 M KCl?
A
72 mL
B
289 mL
C
330 mL
D
930 mL
E
1400 mL
Verified step by step guidance1
Start by understanding the concept of dilution, which involves adding solvent to a solution to decrease its concentration. The number of moles of solute remains constant before and after dilution.
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.
Substitute the known values into the formula: \( C_1 = 5.0 \text{ M} \), \( V_1 = 100 \text{ mL} \), and \( C_2 = 0.54 \text{ M} \). The equation becomes \( 5.0 \times 100 = 0.54 \times V_2 \).
Solve for \( V_2 \) by dividing both sides of the equation by \( 0.54 \): \( V_2 = \frac{5.0 \times 100}{0.54} \).
Calculate \( V_2 \) to find the final volume required to achieve the desired concentration of 0.54 M KCl.
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