From the following equilibrium constants, calculate the equilibrium constant for the reaction...

Question:

From the following equilibrium constants, calculate the equilibrium constant for the reaction {eq}HO_2CCO_2H 2H^+ + C_2O^2- _4. {/eq}

Chemical Equilibrium:


A chemical equilibrium represents the state of a reaction system in which the reactant and product concentrations are not expected to change significantly with time. This equilibrium has a constant "K" defined as the ratio of product concentrations over reactant concentrations. A common example of chemical equilibrium is the acid dissociation or base hydrolysis equilibria of weak acids and bases. It is possible to find "K" values for new equilibrium systems from known equilibrium systems and known "K" values if they are chemically similar.

Answer and Explanation: 1

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{eq}HO_2CCO_2H \leftrightharpoons 2H^+ + C_2O_4^{2-} {/eq}

The above equilibrium represents the double deprotonation of oxalic acid to form oxalate...

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Equilibrium: Chemical and Dynamic

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Chapter 11 / Lesson 1
23K

Learn the definition of chemical equilibrium and how it is dynamic. Discover what the equilibrium constant is and how it shows whether the reaction favors the reactants or products. Learn how chemists designate equilibrium in an equation and how they show the difference in reaction rate.


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