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Chapter 15: Problem 167

Name one biological system in which control of \(\mathrm{pH}\) (buffering ability) is important, and name the buffer that is in control.

Short Answer

Expert verified
One biological system where pH control (buffering ability) is important is the human blood, which needs a stable pH for oxygen transport, enzyme activity, and overall homeostasis. The primary buffer in control in this system is the bicarbonate buffer system, consisting of carbonic acid (H2CO3) and its conjugate base, bicarbonate (HCO3⁻), which helps regulate blood pH by converting strong acids or bases to relatively weak ones.

Step by step solution

01

Introduction

pH control, known as buffering ability, plays a crucial role in various biological systems, as it helps in maintaining the proper functioning of proteins, enzymes and other cellular structures. Multiple buffer systems exist within an organism to maintain a stable pH and prevent detrimental effects on cellular functions.
02

Example of a biological system

One essential biological system in which control of pH is important is the human blood and the associated acid-base balance. A stable pH environment in the bloodstream is necessary for proper oxygen transport, enzyme activity, and overall homeostasis.
03

The buffer in control

In the human blood, the primary buffer that maintains the pH balance is the bicarbonate buffer system. This system consists of a weak acid, carbonic acid (H2CO3), and its conjugate base, bicarbonate (HCO3⁻). The bicarbonate buffer system helps regulate blood pH by converting strong acids or bases to relatively weak ones, thus preventing drastic changes in pH and maintaining a stable environment for cellular functions.

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Most popular questions from this chapter

Write a chemical equation for the reaction between each pair of reactants, using single or double arrows as appropriate: (a) \(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{OH}^{-}\) (b) \(\mathrm{HCl}\) and \(\mathrm{F}^{-}\) (c) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) and \(\mathrm{OH}^{-}\) (d) \(\mathrm{HCN}\) and \(\mathrm{H}_{2} \mathrm{O}\)

Two students each dissolve 1 mole of acid in enough water to get 1 L of solution. Student \(A\) uses acetic acid, and student \(B\) uses hydrochloric acid. Do the solutions have the same pH? If not, which has the lower pH? Why should the two pH values be different?

Can a buffer resist \(\mathrm{pH}\) changes for any added amount of strong acid or base? Explain.

Complete the following sentence: "The lower the \(\mathrm{p} K_{\mathrm{a}}\), the (stronger/weaker) the acid." \(^{\prime \prime}\) How does this parallel pH?

What is the \(\mathrm{pH}\) of a solution whose \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration is \(10.0 \mathrm{M}\) ? Is this solution acidic or basic?
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