The diprotic acid H2A has pK1 = 4.63 and pK2 = 8.98. a) at what pH is [H2A] = [HA-]? b) at what pH is [HA-] = [A2-]? c) Which is the principal species at pH 2.00: d) Which is the principal species at pH 6.00: e) Which is the principal species at pH 10.00:
Added by Jacqueline S.
Step 1
The equilibrium expression for this step is: Ka1 = [HA-][H+]/[H2A] Since [H2A] = [HA-], we can rewrite the expression as: Ka1 = [HA-][H+]/[HA-] Now, we can cancel out [HA-] from both sides: Ka1 = [H+] Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 98 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Consider the diprotic acid H2A with K1 = 1.00 X 10-4 and K2 = 1.00 X 10-8. Find the pH and the concentrations of H2A, HA- and A2- in a) 0.1000 M H2A b) 0.1000 M NaHA c) 0.1000 M Na2A solutions.
Suman K.
For the diprotic weak acid H2A, Ka1 = 3.6 Ă— 10^(-6) and Ka2 = 7.1 Ă— 10^(-9). What is the pH of a 0.0450 M solution of H2A? pH = What are the equilibrium concentrations of H2A and A^2- in this solution? [H2A] = [A^2-] =
Supreeta N.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD