Normality of H2SO4 =0.6 N

Given:
- Volume of HCl solution = 100 ml
- Normality of HCl solution = 0.3 N
- Volume of H2SO4 solution = 200 ml
- Normality of H2SO4 solution = 0.6 N

To Find:
- Normality of H2SO4 in the final solution

Solution:
The normality of a solution can be calculated using the formula:

Normality (N) = Number of gram equivalents / Volume of solution in liters

Step 1: Calculate the number of gram equivalents of HCl solution
Number of gram equivalents of HCl solution = Normality (N) x Volume of solution in liters
= 0.3 x (100/1000)
= 0.03 gram equivalents

Step 2: Calculate the number of gram equivalents of H2SO4 solution
Number of gram equivalents of H2SO4 solution = Normality (N) x Volume of solution in liters
= 0.6 x (200/1000)
= 0.12 gram equivalents

Step 3: Calculate the total number of gram equivalents in the final solution
Total number of gram equivalents = Number of gram equivalents of HCl + Number of gram equivalents of H2SO4
= 0.03 + 0.12
= 0.15 gram equivalents

Step 4: Calculate the normality of the final solution
Normality of the final solution = Total number of gram equivalents / Volume of the final solution in liters
Volume of the final solution = 100 ml + 200 ml = 300 ml = 0.3 L
Normality of the final solution = 0.15 / 0.3
= 0.5 N

Therefore, the normality of H2SO4 in the final solution is 0.5 N.

Explanation:
When two solutions are mixed, the total number of gram equivalents in the final solution is the sum of the individual gram equivalents. The volume of the final solution is the sum of the individual volumes. Using the formula for normality, we can calculate the normality of the final solution. In this case, we added 100 ml of 0.3 N HCl solution and 200 ml of 0.6 N H2SO4 solution to get a final volume of 300 ml. We found that the total number of gram equivalents in the final solution is 0.15. Dividing this by the final volume of 0.3 L gives us a normality of 0.5 N for the final solution.