Chapter 6: QJ-E (page 141)

Question: Histidine is a triprotic amino acid:
Find the value of the equilibrium constant for the reaction

Short Answer

Expert verified

The equilibrium constant for the reaction is 1.17×10^-8

Step by step solution

Given data

Histidine is one type of amino acid. It follows the following equilibrium constant values for protonation

$K_{1} = 3 \times 10^{- 2} K_{2} = 8.5 \times 10^{- 7} K_{3} = 4.6 \times 10^{- 10}$

We need to determine equilibrium constant for the following reaction

Determine the equilibrium constant

be denoted by A and the equilibrium constant for the reaction be K.

The equilibrium constant for the reaction will be

$\begin{array}{rcl} [H^{+}] [O H^{-}] & = & K_{w} \\ K_{w} & = & 10^{- 14} \\ \frac{[A H^{+}] [O H^{-}]}{[A H]} & = & K \\ \frac{[A H]}{[A]} & = & K_{2} \\ \frac{[H^{+}] [A] [O H^{-}]}{[A H]} & = & \frac{K_{w}}{K_{2}} \\ \frac{[A H^{+}] [O H^{-}]}{[A H]} & = & \frac{K_{w}}{K_{2}} \\ K & = & \frac{K_{w}}{K_{2}} \\ = & \frac{10^{- 14}}{8.5 \times 10^{- 7}} \\ = & 1.17 \times 10^{- 8} \end{array}$

Therefore, the equilibrium constant for the reaction is 1.17×10^-8

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Question: Histidine is a triprotic amino acid:
Find the value of the equilibrium constant for the reaction

Short Answer

Step by step solution

Given data

Determine the equilibrium constant

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Question: Histidine is a triprotic amino acid:Find the value of the equilibrium constant for the reaction

Short Answer

Step by step solution

Given data

Determine the equilibrium constant

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Making Measurements

Ionic and Molecular Compounds

Chemistry Branches

Organic Chemistry

Chemical Reactions

Kinetics

Study anywhere. Anytime. Across all devices.

Question: Histidine is a triprotic amino acid:
Find the value of the equilibrium constant for the reaction