Multiple Choice
A laboratory has concentrated HNO3 solution with a molarity of 6.00 M. How many milliliters of this concentrated solution are required to prepare 1.15 L of 0.115 M HNO3 by dilution with water?
71
views
6. Chemical Quantities & Aqueous Reactions
Dilutions
Multiple Choice
What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution?
A
250.0 mL
B
100.0 mL
C
50.0 mL
D
25.0 mL
Verified step by step guidance1
Identify the known values: the concentration of the stock solution \(C_1 = 2.00\,M\), the desired concentration of the diluted solution \(C_2 = 0.100\,M\), and the volume of the diluted solution \(V_2 = 500.\,mL\).
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: \(V_1 = \frac{0.100\,M \times 500.\,mL}{2.00\,M}\).
Calculate \(V_1\) to find the volume of the 2.00 M KCl stock solution required to prepare 500 mL of 0.100 M KCl solution.
Related Videos
Related Practice
