H(3)PO(4) is a weak triprotic acid, appr...

`H_(3)PO_(4)` is a weak triprotic acid, approximate pH 0.1 M `NaHPO_(4)`(aq.) is calculated by:

`1/2[pK_(a1)+pK_(a2)]`

`1/2[pK_(a2)+pK_(a3)]`

`1/2[pK_(a1)+pK_(a3)]`

`pK_(a1)+pK_(2)`

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pK_(a1) , pK_(a_(2)) and pK_(a_(3)) of H_(3)PO_(4) are respectively x,y and z. pH of 0.1 M Na_(2)HPO_(4) solution is

Statement-1 : Both H_(3)PO_(3) and H_(3)PO_(4) have the same number of hydrogen atoms but H_(3)PO_(4) is a tribasic acid and H_(3)PO_(3) is a dibasic acid. Statement-2 : 1 mol of H_(3)PO_(3) is neutralised by 2 mol of NaOH while 1 mol of H_(3)PO_(4) is neutralised by 3 mol of NaOH

Statement-1: Heat of neutralisation of H_(3)PO_(4) with NaOH is more than that of HCl with NaOH. Statement-2: H_(3)PO_(4) is a triprotic acid and hence release more heat on complete neutralization, while HCl is a monoprotic acid.

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STATEMENT -1 : H_(3)PO_(4) is a tribasic acid. and STATEMENT -2 : In H_(3)PO_(4) , only two H-atoms are replaceable.

A buffer solution of 0.080M Na_(2)HPO_(4) and 0.020 M Na_(3)PO_(4) is prepared. The electrolytic oxidation of 1.0 mmol RNHOH is carried out in 100mL buffer to give RNHOH + H_(2)O rarr RNO_(2) + 4H^(o+) + 4e^(-) Calculate approximate pH of the solution after oxidation is complete pK_(a_(2)), pK_(a_(2)) , and pK_(a_(3)) of H_(3)PO_(4) are 2.12,7.20 , and 12.0 , respectively.

H_(3)A is a weak triprotic acid (K_(a1)=10^(-5),K_(a2)=10^(-9),K_(a3)=10^(-13) What is the value of pX of 0.1 M H_(3)A (aq.) solution ? Where pX=-log X and X= [[A^(3-)]]/[[HA^(2-)]]

Statement -1 : H_(3)PO_(2) is a weak monobasic acid and is also strong reducing in nature. Statement -2 :

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