What is the final concentration of HCl when 5.4 mL of 1.0 M HCl is diluted with 60.0 mL of water?

• A. 0.090 M
• B. 0.100 M
• C. 0.082 M
• D. 0.009 M

Answer: (C)

Verified step by step guidance

1. Identify the initial concentration (\(C_1\)) and volume (\(V_1\)) of the HCl solution before dilution. Here, \(C_1 = 1.0\,M\) and \(V_1 = 5.4\,mL\).
2. Determine the final volume (\(V_2\)) after dilution by adding the volume of water to the initial volume of HCl solution. So, \(V_2 = 5.4\,mL + 60.0\,mL\).
3. Use the dilution formula which relates initial and final concentrations and volumes: \(C_1 \times V_1 = C_2 \times V_2\), where \(C_2\) is the final concentration after dilution.
4. Rearrange the dilution formula to solve for the final concentration \(C_2\): \(C_2 = \frac{C_1 \times V_1}{V_2}\).
5. Substitute the known values into the equation and calculate \(C_2\) to find the final concentration of HCl after dilution.