In a solution containing `0.01M HCl` and `0.1M H_(2)CO_(3)` ratio of `[H^(+)]` produced from strong acid & weak acid respectively is :- Report your answer as `x//500`.Given :`K_(a_(1))&K_(a_(2))` of `H_(2)CO_(3)` are `4xx10^(-7)&(4xx10^(-11))` respectively.

If K_(a_(1))gtK_(a_(2)) of H_(2)SO_(4) are 10^(-2) and 10^(-6) respectively then:

Approximate p.H,0.1M aqueous H_(2)S solution when K_(1) and K_(2) for H_(2)S at 25^(@)C are 1xx10^(-7) and 1.3xx10^(-13) respectively:-

A solution contains 0.1MH_(2)S and 0.3MHCl .Calculate the conc.of S^(2-) and HS^(-) ions is solutions.Given K_(a_(1)) and K_(a_(2)) are 10^(-7) and 1.3xx10^(-13) respectively.

A solution containing a weak acid and its conjugate base acts as an acidic buffer. In a buffer the dissociation of the weak acid is suppressed by its conjugate base. (K_(1),K_(2), and K_(3) of H_(3)PO_(4) , are 10^(-4), 10^(-8), 10^(-13) respectively What is the pH of a solution obtained by mixing 100ml of 0.1 MH_(3) PO_(4) , and 150ml of 0.IM NaOH

For a 0.072 M NaSO_(4) solution,select the correct option(s): (K_(a_(1)) and K_(a_(2)) of H_(2)SO_(4)=oo & 1.2xx10^(-2))

In a solution containing 0.1M HCl & 0.1M H_(3)PO_(4) (having dissociation constants K_(a_(1)),K_(a_(2)),K_(a_(3))) assuming alphaltlt1 for H_(3)PO_(4) ,

Calculate the equilibrium constants for the reactions with water of H_(2)PO_(4)^(Theta), HPO_(4)^(2-) , and PO_(4)^(3-) as ase. Comparing the relative values of two equilibrium constants of H_(2)PO_(4)^(Theta) with water, deduce whether solutions of this ion in water are acidic or base, Deduce whether solutions of HPO_(4)^(2-) are acidic or bases. Given K_(1),K_(2) ,and K_(3) for H_(3)PO_(4) are 7.1 xx 10^(-3), 6.3 xx 10^(-8) , and 4.5 xx 10^(-13) respectively.

In a solution of 0.1M H_(3)PO_(4) acid (Given K_(a_(1))=10^(-3),K_(a_(2))=10^(-7),K_(a_(3))=10^(-12)) pH of solution is

A solution contains 0.10 M H_2S and 0.3 HCl Calculate the concentration of S^(2-) and HS^(-) ions in the solution . For H_2S , K_(a_1) = 1 xx 10^(-7) and K_(a_2) = 1.3 xx 10^(-13)

The pH of a solution containing 0.4 M HCO_(3)^(-) and 0.2 M CO_(3)^(2-) is : [K_(a1)(H_(2)CO_(3))=4xx10^(-7) , K_(a2)(HCO_(3)^(-))=4xx10^(-11)]