To prepare a buffer solution of pH=4.04, amount of Barium acetate to be added to 100 mL of 0.1 M acetic acid solution `[pK_b(CH_(3)COO^(-))=9.26]` is:

To prepare a buffer solution of pH=4.04, amount of Barium acetate to be added to 100mL of 0.1 M acetic acid solution [ pkb (CH3COO-)=9.26] is:

To prepare a buffer of pH 8.26 , amount of (NH_(4))_(2)SO_(4) to be added into 500mL of 0.01M NH_(4)OH solution [pK_(a)(NH_(4)^(+))=9.26] is:

To prepare a buffer of pH 8.26 , amount of (NH_(4))_(2)SO_(4) to be added into 500mL of 0.01M NH_(4)OH solution [pK_(a)(NH_(4)^(+))=9.26] is:

A buffer solution of pH value 4 is to be prepared, using CH_(3)COOH and CH_(3)COONa .How much amount of sodium acetate is to be added to 1.0L of M//10 acetic acid? (K_(a) = 2.0 xx 10^(-5))

A buffer solution of pH value 4 is to be prepared, using CH_(3)COOH and CH_(3)COONa .How much amount of sodium acetate is to be added to 1.0L of M//10 acetic acid? (K_(a) = 2.0 xx 10^(-5))

In order to prepare a buffer solution of pH 5.74, sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is _______ M, the concentration of sodium acetate in the buffer is M. (Round off to the Nearest Integer). [Given : p^(Ka) (acetic acid) = 4.74]

The Ph of basic buffer mixtures is given by : Ph=Pk_(a)+ log (["Base"])/(["Salt"]) whereas Ph of acidic buffer mixtures is given by : Ph = pK_(a)+"log"(["Salt"])/(["Acid"]) . Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. The volume of 0.2 m NaOH needed to prepare a buffer of pH 4.74 with 50 mL of 0.2 m acetic acid pH_(b) of CH_(3)COO^(-)=9.26 is :

The pH of basic buffer mixtures is given by : pH=pK_(a)+log((["Base"])/(["Salt"])) , whereas pH of acidic buffer mixtures is given by: pH= pK_(a)+log((["Salt"])/(["Acid"])) . Addition of little acid or base although shows no appreciable change for all practical purpose, but since the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) change, a slight decrease or increase in pH results in. The volume of 0.2M NaOH needed to prepare a buffer of pH 4.74 with 50 mL of 0.2M acetic acid is: (pK_(a) of CH_(3)COO^(-)= 9.26)

A buffer solution contains 0.1 M each of acetic acid and sodium acetate. The pH of the buffer solution is (pK_(a)(CH_(3)COOH)=4.75) :