(b) Using the equation below, explain what happens to maintain the pH of the solution: HA (aq) (i) H+ (aq) + A (aq) when an acid is added (meaning more H+ ions added) (ii) when a base is added (meaning more OH- ions added) (iii) Give one example each of a buffer in both living and non-living systems
(b) Using the equation below, explain what happens to maintain the pH of the solution: HA (aq) (i) H+ (aq) + A (aq) when an acid is added (meaning more H+ ions added) (ii) when a base is added (meaning more OH- ions added) (iii) Give one example each of a buffer in both living and non-living systems
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section17.6: Equilibria Involving Complex Ions
Problem 2.1ACP: Phosphate ions are abundant in cells, both as the ions themselves and as important substituents on...
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![(b) Using the equation below, explain what happens to maintain the pH of the solution:
HA (aq)
(i)
H+ (aq)
+
A (aq)
when an acid is added (meaning more H+ ions added)
(ii) when a base is added (meaning more OH- ions added)
(iii) Give one example each of a buffer in both living and non-living systems](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0c7834e0-cce9-4f6a-be4a-aec6bef2b5fc%2Fa0724865-bf19-4d2e-b228-c12ea5d7a83c%2Fewqs56i_processed.png&w=3840&q=75)
Transcribed Image Text:(b) Using the equation below, explain what happens to maintain the pH of the solution:
HA (aq)
(i)
H+ (aq)
+
A (aq)
when an acid is added (meaning more H+ ions added)
(ii) when a base is added (meaning more OH- ions added)
(iii) Give one example each of a buffer in both living and non-living systems
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