A weak acid HA after teratment with 12 mL of `0.1M` strong base BOH has a pH of 5. At the end point, the volume of same base required is `26.6mL.K_(a)` of acid 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. A weak acid HA after treatment with 12 mL of 0.1M strong base BOH has a pH=5 . At end point, the volume of same base required is 26.6mL K_(a) of acid is:

A weak acid (HA) after treatment with 12 mL of 0.1 M strong base (BOH) has a pH of 5 . At the end point , the volume of same base required is 27 mL . K_(a) of acid is (log 2=0.3)

A weak base BOH is titrated with strong acid HA . When 10mL of HA is added, the pH is 9.0 and when 25mL is added, pH is 8.0 . The volume of acid required to reach the equivalence point is

A solution of 0 .1 weak base (B )is titrated with 0.1 M of a strong acid ( HA) . The variation of pH of the solution will be the volume of HA added is shown in the figure below. What is the pK_b of the base ? The neutralization reaction is given by B+HA rarrHA rarrBH^(+)+A^(-)

A weak acid has a strong conjugate base and a strong acid has a weak conjugate base.

A weak base (BOH) with K_(b) = 10^(-5) is titrated with a strong acid (HCl) , At 3//4 th of the equivalence point, pH of the solution is:

A strong acid is titrated with weak base. At equivalence point, pH will be :