30 ml of 0.2 M NaOH is added with 50 ml `"0.2 M "CH_(3)COOH` solution. The extra volume of 0.2 M NaOH required to make the pH of the solution 5.00 is `(10)/(x).` The value of x is. The ionisation constant of `CH_(3)COOH=2xx10^(-5)`.

20 mL of 0.2M sodium hydroxide is added to 50 mL of 0.2 M acetic acid to give 70 mL of the solution. What is the pH of this solution. Calculate the additional volume of 0.2M NaOh required to make the pH of the solution 4.74 . (Ionisation constant of CH_(3)COOh is 1.8 xx 10^(-5))

20 mL of 0.2M sodium hydroxide is added to 50 mL of 0.2 M acetic acid to give 70 mL of the solution. What is the pH of this solution. Calculate the additional volume of 0.2M NaOh required to make the pH of the solution 4.74 . (Ionisation constant of CH_(3)COOh is 1.8 xx 10^(-5))

0.2 M NaOH are added to 50 ml of 0.2 M acetic acid ( K_(a) = 1.8 xx 10^(-5)) . The volume of 0.2 M NaOH required to make the pH of solution 4.74 ( -log 1.8 xx 10^(-5) = 4.74 )

If 50 ml 0.2 (M) CH_3COOH is mixed with 20 ml 0.2 (M) NaOH solution, then what will be the pH of the mixed solution?

50 ml of 0.1 M HCl and 50 ml of 0.2 M NaOH are mixed. The pH of the resulting solution is :

20ml of 0.2 M NaOH is added to 50 ml , of 0.2 M CH_(3)COOH to give 70 ml , of the solution. What is the pH of the solution? The ionization constant of acetic acid is 2xx10^(-5)

If 20 mL of 0.1 M NaOH is added to 30 mL of 0.2 M CH_(3)COOH (pK_(a)=4.74) , the pH of the resulting solution is :

100 ml of 0.1 M CH_(3)COOH are mixed with 100ml of 0.1 M NaOH , the pH of the resulting solution would be

If 20 mL of 0.1 M NaOH is added to 30 mL of 0.2 M CH_(3)COOH (pK_(a)=4.74), the pH of the resulting solution is :