$200$ mL of $1$ M $HCl$ is mixed with $300$ mL of $6$ M $HCl$ and the final solution is diluted to $1000$ mL. The molar concentration of $\left[H^{+}\right]$ ion is:

Q. 200 mL of a 1 M $HN{O}_3$ solution is mixed with 300 mL of 6 M $HN{O}_3$ and the final solution is diluted to 1000 mL. Calculate the concentration of $H^{+}$ ions.

Q. 100 mL of a 1 M $H_{2}S{O}_4$ solution is mixed with 200 mL of a 0.5 M HCl solution and diluted to a final volume of 500 mL. 200 mL of this solution is further diluted with 300 ml of water. Find the normality of $H^{+}$ ions in the final solution.

Q. 100 mL of a 0.1 M HCl solution, 200 mL of a 0.2 M HCl solution, 300 mL of a 0.3 M HCl solution, 400 mL of a 0.4 M HCl solution and 500 mL of a 0.5 M HCl solution are mixed. 200 mL of this solution is diluted with 300 mL of water. What is the molarity of HCl in the resultant solution?

Q. 100 mL of a 0.1 M HCl solution, 200 mL of a 0.2 M HCl solution, 300 mL of a 0.3 M HCl solution, 400 mL of a 0.4 M HCl solution and 500 mL of a 0.5 M HCl solution are mixed. 200 mL of this solution is diluted with 300 mL of water. What is the molarity of HCl in the resultant solution?