Multiple Choice
When a solution is diluted by adding more solvent, how does this process affect the molarity of the solution?
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6. Chemical Quantities & Aqueous Reactions
Dilutions
Multiple Choice
What volume of 7.50 M HNO3 should be diluted to prepare 25.00 mL of a 2.00 M HNO3 solution?
A
25.00 mL
B
6.67 mL
C
9.33 mL
D
3.75 mL
Verified step by step guidance1
Identify the known values: the concentration of the stock solution \(C_1 = 7.50\, M\), the desired concentration of the diluted solution \(C_2 = 2.00\, M\), and the final volume of the diluted solution \(V_2 = 25.00\, mL\).
Recall the dilution equation which relates the concentrations and volumes before and after dilution: \(C_1 \times V_1 = C_2 \times V_2\), where \(V_1\) is the volume of the stock solution needed.
Rearrange the dilution equation to solve for \(V_1\): \(V_1 = \frac{C_2 \times V_2}{C_1}\).
Substitute the known values into the equation: \(V_1 = \frac{2.00\, M \times 25.00\, mL}{7.50\, M}\).
Calculate \(V_1\) to find the volume of 7.50 M HNO3 required to prepare 25.00 mL of 2.00 M HNO3 solution.
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