Solution of an acid and it's anion (that is it's conjugate base) or of a base and it's common cation are buffered. When we add a small amount of acid or base to any one of them, the pH of solution changes very little pH of buffer solution can be compoted as , for , acidic , buffer pH = pK_(a) + "log"(["Conjugate base"])/(["Acid"]) for basuc buffer pOH = pK_(b) + "log" (["Conjugated base"])/(["base"]) it is generally accepteed that a solution has useful buffer capacity (pH change resistng power) provided that the value of [salt or conjugate base]/[acid] for acidic acid buffer lies within the range of 1:10 to 10:1. Buffer capacity is max. When [conjugate base]=[acid] Calculate the pH of the solution made by adding 0.01 mole of HCl in 100 ml. of solution which is 0.2 M in NH_(3)(pK_(b) = 4.74) and 0.3 M in NH_(4)^(+):

Solution of an acid and it's anion (that is it's conjugate base) or of

1.	Solution of an acid and it's anion (that is it's conjugate base) or of a base and it's common cation are buffered. When we add a small amount of acid or base to any one of them, the pH of solution changes very little pH of buffer solution can be compoted as , for , acidic , buffer pH = pK_(a) + "log"(["Conjugate base"])/(["Acid"]) for basuc buffer pOH = pK_(b) + "log" (["Conjugated base"])/(["base"]) it is generally accepteed that a solution has useful buffer capacity (pH change resistng power) provided that the value of [salt or conjugate base]/[acid] for acidic acid buffer lies within the range of 1:10 to 10:1. Buffer capacity is max. When [conjugate base]=[acid] Calculate the pH of the solution made by adding 0.01 mole of HCl in 100 ml. of solution which is 0.2 M in NH_(3)(pK_(b) = 4.74) and 0.3 M in NH_(4)^(+):
Answer» `5.34` `8.66` `7.46` `4.46` SOLUTION :N//A