Multiple Choice
What is the molar concentration of the chloride ion (Cl⁻) in a solution prepared by diluting 25.0 mL of a 0.100 M CaCl₂ solution to a final volume of 250 mL?
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6. Chemical Quantities & Aqueous Reactions
Dilutions
Multiple Choice
What volume of 13 M HCl is needed to prepare 350 mL of 4.0 M HCl solution?
A
50.0 mL
B
140.0 mL
C
350.0 mL
D
107.7 mL
Verified step by step guidance1
Start by using the dilution formula, which is \( C_1V_1 = C_2V_2 \), where \( C_1 \) and \( V_1 \) are the concentration and volume of the stock solution, and \( C_2 \) and \( V_2 \) are the concentration and volume of the diluted solution.
Identify the known values: \( C_1 = 13 \) M, \( C_2 = 4.0 \) M, and \( V_2 = 350 \) mL. You need to find \( V_1 \), the volume of the stock solution.
Rearrange the dilution formula to solve for \( V_1 \): \( V_1 = \frac{C_2V_2}{C_1} \).
Substitute the known values into the rearranged formula: \( V_1 = \frac{4.0 \times 350}{13} \).
Calculate \( V_1 \) to find the volume of 13 M HCl needed to prepare the desired solution. Ensure units are consistent and convert if necessary.
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