What volumes of 0.200 M `HNO_2` and 0.200 M `NaNO_2` are required to make 500 mL of a buffer solution with pH =3.00 ? [`K_a` for `HNO_2=4.00xx10^(-4)`]

What volume of 0.10 M sodium formate solution should be added to 50 mL of 0.05 M formic acid to produce a buffer solution of pH = 4.0 ? pK_a for formic acid = 3.80?

The volume of 10.50 M solution required to prepare 1.0 L of 0.25 M solution of HNO_(3) is :

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) .

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) .

Find the amount of (NH_(4))_(2)SO_(4) required to be added to 500 mL 0.2 (M) NH_(3) to prepare a buffer solution of pH=9.35. [Given: K_(b)(NH_(3))=1.78xx10^(-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 )

The volume of 0.1 M Na_(2)SO_(4) needed to be added to 10 mL of 0.1 M HCI to change the pH from 1.00 to 1.50 is : (K_(2) =1.26 xx10^(-2) " for " H_(2)SO_(4))

How much volume of 0.2 M solution of acetic acid shouls be added to 100 ml of 0.2 M solution of sodium acetate to prepare a buffer solution of pH 5.00 ? pK_(a) for acid is 4.74

How much volume of 0.2 M solution of acetic acid shouls be added to 100 ml of 0.2 M solution of sodium acetate to prepare a buffer solution of pH 5.00 ? pK_(a) for acid is 4.74