For a solution obtained by mixing equal volumes of 0.02M KOH solution &0.2M B (weak diacidic base),`(K_(b_(1))=10^(-7) & K_(b_(2))=10^(-14))` . Find the pH of solution

pOH of a 0.004M aqueous solution of diacidic weak base B (pK_(b_(1))=3.7&pK_(b_(2))=7.3) is:

pH of solution obtained by mixing equal volumes of 0.1M Triethyl amine (K_(b)=6.4xx10^(-5)) & (4)/(45)M NH_(4)OH (K_(b)=1.8xx10^(-5)) will be :

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

Calcualate pH,[H^(+)],[OH^(-)],[CH_(3)COOH],[SH^(-)],[H_(2)S],[S^(2-)] in a solution obtained by mixing equal volume of 0.2M H_(2)S &0.02M acetic acid .Given that K_(a)(CH_(3)COOH)=2xx10^(-5),K_(a_(1))(H_(2)S)=10^(-7),K_(a_(2))(H_(2)S)=10^(-14) Take log21=-1.32,(1)/(sqrt(21))=0.218

In a 0.2M aqueous solution of Ethylene diamine (H_(2)NCH_(2)CH_(2)NH_(2)): Given K_(b_(1))=8xx10^(-5) & K_(b_(2))=2.7xx10^(-8) Find the pH of Solution .

% dissociation of a 0.024M solution of a weak acid HA(K_(a)=2xx10^(-3)) is :

Calculate pOH of 0.1 M aq. Solution of weak base BOH (K_(b)=10^(-7)) at 25^(@)C.

Find the pH of a buffer solution having equal volumes of 0.2MNH_(4)OH and 0.2M NH_(4)Cl (K_(b) for base =1.0xx10^(-5) )

Calculate the pH of solution obtained by mixing 10 ml of 0.1 M HCl and 40 ml of 0.2 M H_(2)SO_(4)

What is the pH of 0.01 M glycine solution? [For glycine, K_(a_(1))=4.5xx10^(-3) and K_(a_(2))=1.7xx10^(-10) at 298 K ]