Find the pH of the solution formed when: 50ml of 0.0100M HCl acid is added to 50mL of 0.0200M nitric acid?

Question

Find the pH of the solution formed when: 50ml of 0.0100M HCl acid is added to 50mL of 0.0200M nitric acid?

Answer 1

Use the same reasoning as for your last question.

Answer 2

(50 mL)(0.01M ) = 0.5 mmoles of H+

(50 mL)(0.02M ) = 1 mmole  total 1.5 mmol of H+

( since the acids are 100% ionized )  in 100 mL of solution.

so M ( H+ ) = 1.5 mmol/100 mL = 0.015 M in H+

pH = -log ( 0.015 ) = 2 - log 1.5 = 1.82  

proof

0.01 M HCl = pH 2 ( -log 10^-2)

0.02 M HNO3 = pH 1.7 ( -log 2X 10^-2 )  so pH will be NEAR 1.85