Answered step by step
Verified Expert Solution
Question
1 Approved Answer
For the diprotic weak acid H_(2)A,K_(al)=3.5times 10^(-6) and K_(a2)=8.3times 10^(-9) . What is the pH of a 0.0500M solution of H_(2)A ? pH= 3.37 What
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)
Step by Step Solution
There are 3 Steps involved in it
Step: 1
Get Instant Access to Expert-Tailored Solutions
See step-by-step solutions with expert insights and AI powered tools for academic success
Step: 2
Step: 3
Ace Your Homework with AI
Get the answers you need in no time with our AI-driven, step-by-step assistance
Get Started