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20 mL of 0.5 M HCl is mixed with 30 mL o...

20 mL of 0.5 M HCl is mixed with 30 mL of 0.3 M HCl, the molarity of the resulting solution is :

A

0.8 M

B

0.53 M

C

0.38 M

D

0.83 M

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The correct Answer is:
To find the molarity of the resulting solution when 20 mL of 0.5 M HCl is mixed with 30 mL of 0.3 M HCl, we can follow these steps: ### Step 1: Identify the given values - Molarity of the first solution (M1) = 0.5 M - Volume of the first solution (V1) = 20 mL - Molarity of the second solution (M2) = 0.3 M - Volume of the second solution (V2) = 30 mL ### Step 2: Calculate the total number of moles of HCl from each solution - Moles from the first solution: \[ \text{Moles}_1 = M1 \times V1 = 0.5 \, \text{mol/L} \times 20 \, \text{mL} = 0.5 \times 0.020 \, \text{L} = 0.01 \, \text{mol} \] - Moles from the second solution: \[ \text{Moles}_2 = M2 \times V2 = 0.3 \, \text{mol/L} \times 30 \, \text{mL} = 0.3 \times 0.030 \, \text{L} = 0.009 \, \text{mol} \] ### Step 3: Calculate the total moles of HCl in the mixture \[ \text{Total moles} = \text{Moles}_1 + \text{Moles}_2 = 0.01 \, \text{mol} + 0.009 \, \text{mol} = 0.019 \, \text{mol} \] ### Step 4: Calculate the total volume of the resulting solution \[ \text{Total volume} = V1 + V2 = 20 \, \text{mL} + 30 \, \text{mL} = 50 \, \text{mL} = 0.050 \, \text{L} \] ### Step 5: Calculate the molarity of the resulting solution \[ \text{Molarity} = \frac{\text{Total moles}}{\text{Total volume}} = \frac{0.019 \, \text{mol}}{0.050 \, \text{L}} = 0.38 \, \text{M} \] ### Final Answer The molarity of the resulting solution is **0.38 M**. ---
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