A solution is prepared by mixing `25.0` mL of `6.0` M HCI with `45.0` mL of `3.0` M `HNO_(3)`. What is `[H^(+)]` in the resulting solution?

What is the concentration of H^(+) in a solution that is prepared by mixing 50.0 mL of 0.50 M HCl with 200.0 mL of 0.25 M HCl ? Fill your Answer of the multiplying it with 10.

The pH of a solution formed by mixing 40 mL of 0.10 M HCl and 10 mL of 0.45 M NaOH is:

250mL of 0.2M H_(2)SO_(4) is mixed with 100mL of 0.5M H_(2)SO_(4) . What is the molarity of the resulting solution?

60ml of 0.1M HCl is mixed with 40ml of 0.05M H_(2)SO_(4) .The "pH" value of the resulting solution is

50 mL of 0.1 M HCl and 50 mL of 2.0 M NaOH are mixed. The pH of the resulting solution is

50.0 mL of 0.10 M ammonia solution is treated with 25.0 mL of 0.10M HCI . If K_(b)(NH_(3))=1.77xx10^(-5) , the pH of the resulting solution will be

50.0 mL of 0.10 M ammonia solution is treated with 25.0 mL of 0.10M HCI . If K_(b)(NH_(3))=1.77xx10^(-5) , the pH of the resulting solution will be