`pK_(a)` and `K_(a)` of an acid are connected by the relation.......

The pK_(a1) and pK_(a2) of an amino acid are 2.3 and 9.7 respectively. The isoelectric point of the amino acid is:

pK_(a) of a weak acid is defined as :

If K_(a) and K_(b) are the dissociation constants of weak acid and its conjugate base , pK_(a) + pK_(b)

Prove that the dergee of dissociation of weak acid is given by: alpha = (1)/(1+10^(pK_(a)-pH)) where K_(a) is its dissociation constant of the weak acid.

Greater the pK_(a) value on an acid …………… is the acid .

If pK_(a) of acetic acid and pK_(b) of ammonium hydroxide are 4.76 each. Find the pH of ammonium acetate.

Select the correct set of the statements for an acid type indicator used in a titration : (i) In general, pH range of an indicator is (pK_(a)-1) to (pK_(a)+1) and indicator shows its characteristic colours in this range. (ii) In general pH range of an indicator is (pK_(a)-1) to (pK_(a)-1) and indicator does not show its characteristic colours in this range (iii) In this relation : pH=pK_(In) +log_(10)((["In"^(-)])/(["HIn"])),pH value representes pH of indicator solution. (iv) In this relation : pH=pK_(In) +log_(10)((["In"^(-)])/(["HIn"])),pH value represents pH of resulting solution containing indiactor .

The pK_(a) of a weak acid is 4.8 . What should be the ratio of [Acid]/[Salt] of a buffer if pH = 5 .8 is required

The pK_(a_1), pK_(a_2) and pK_(a_3) value for the amino acid cysteine (HS-CH_2-undersetunderset(NH_2)(|)CH-COOH) are respectively 1.8, 8.3, 10.8. What is isoelectric point of cysteine amino acid ?

When a salt reacts with water to form acidic or basic solution , the process is called hydrolysis . The pH of salt solution can be calculated using the following relations : pH = 1/2 [pK_(w) +pK_(a) + logc] (for salt of weak acid and strong base .) pH = 1/2 [pK_(w) - pK_(b) - logc] (for salt of weak base and strong acid ) . pH = 1/2 [ pK_(w)+pK_(a)-pK_(b)] (for weak acid and weak base ). where 'c' represents the concentration of salt . When a weak acid or a weak base not completely neutralized by strong base or strong acid respectively , then formation of buffer takes place . The pH of buffer solution can be calculated using the following relation : pH = pK_(a) + log . (["Salt"])/(["Acid"]) , pOH = pK_(b) + log . (["Salt"])/([ "Base"]) Answer the following questions using the following data : pK_(a) = 4.7447 , pK_(b) = 4.7447 ,pK_(w) = 14 When 100 mL of 0.1 M NH_(4)OH is added to 50 mL of 0.1M HCl solution , the pH is