Two solutions of a substance (non-electroyte) are mixed in the following manner `480 mL` of `1.5M` of first solution with `520 mL or 1.2M` of second solution. The molarity of final solution is:

Options

A. `1.20 M`
B. `1.50 M`
C. 1.344 M
D. `2.70 M`

Explanation

To find the molarity of the final solution after mixing two solutions, we can follow these steps:

### Step 1: Calculate the number of moles in each solution.

1. **For the first solution:**
- Volume (V1) = 480 mL = 0.480 L (since 1 L = 1000 mL)
- Molarity (M1) = 1.5 M
- Number of moles (n1) = M1 × V1 = 1.5 mol/L × 0.480 L = 0.72 moles

2. **For the second solution:**
- Volume (V2) = 520 mL = 0.520 L
- Molarity (M2) = 1.2 M
- Number of moles (n2) = M2 × V2 = 1.2 mol/L × 0.520 L = 0.624 moles

### Step 2: Calculate the total number of moles in the final solution.

- Total moles (n_total) = n1 + n2 = 0.72 moles + 0.624 moles = 1.344 moles

### Step 3: Calculate the total volume of the final solution.

- Total volume (V_total) = V1 + V2 = 480 mL + 520 mL = 1000 mL = 1.0 L

### Step 4: Calculate the molarity of the final solution.

- Molarity of final solution (M_final) = Total moles / Total volume = n_total / V_total
- M_final = 1.344 moles / 1.0 L = 1.344 M

### Conclusion

The molarity of the final solution is **1.344 M**.

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