For the diprotic weak acid

H_(2)A,K_(al)=3.5\\\\times 10^(-6)

and

K_(a2)=8.3\\\\times 10^(-9)

. What is the

pH

of a

0.0500M

solution of

H_(2)A

?\

pH=

3.37\ What are the equilibrium concentrations of

H_(2)A

and

A^(2-)

in this solution?\

[H_(2)(A)]=

4.9

*10^(-2)

For the diprotic weak acid H2A,Ka1=3.5106 and Ka2=8.3109. What is the pH of a 0.0500M solution of H2A ? pH= What are the equilibrium concentrations of H2A and A2 in this solution