A `50.0` mL solution of `0.150` M HCl. Is mixed with `25.0` mL of `0.400` M HCl What is the HCI concentration in the final solution? (Assume volumes are additive.)

100 mL of 0.15 M HCl is mixed with 100 mL of 0.005M HCl , what is the pH of the following solution approxmately

100 mL of 0.15 M HCl is mixed with 100 mL of 0.005M HCl , what is the pH of the following solution approxmately

100 ml of 0.15 M HCl is mixed with 100 ml of 0.05 M HCl, is the pH of the resulting solution?

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

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

If 100 mL of 0.100 M HCl solution and 100 mL of 0.100 M NaOH are mixed, what is the molarity of the salt in the resulting sollution? Assuming that the volumes are additive.

If 250 ml of 0.25 M NaCl solution is diluted with water to a volume of 500 ml, the new concentration of solution is:

25 mL of 3.0 M HCl are mixed with 75 mL of 4.0 M HCl. If the volumes are additive, the molarity of the final mixture will be :

25 mL of 3.0 HCl are mixed with 75 mL of 4.0 M HCl. If the volumes are additive, the molarity of the final mixture will be :