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Calculating the Equilibrium Constant for Reaction

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If the following data is "true":

H3PO4(aq)<--> H^+(aq) + H2PO4^-(aq) ...... .Ka1 = 7.5x10^-3
H2PO4^-(aq)<--> H+(aq) + HPO4^-2(aq) .............Ka2 = 6.2x10^-8
HPO4^-2(aq) <--> H+(aq) + HPO4^-3(aq) ............Ka3 = 4.8x10^-13

What is Ka for the reaction H3PO4(aq) <--> 3H^+(aq) + PO4^-3(aq)?

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Solution Preview

If the following data is "true":

H3PO4(aq) <--> H+(aq) + H2PO4−(aq) Ka1 = 7.5×10−3
H2PO4−(aq)<--> H+ (aq) + HPO42−(aq) Ka2 = ...

Solution Summary

This solution provides step by step for calculating the equilibrium constant for a reaction.

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Calculating the Equilibrium Constant: Change in Free Energy

Survey of physical chemistry

State all of the assumptions (e.g. ideal gas etc).

(previous reaction is 2H??2(g) + O2(g) ----> 2H2O(g))

Given the reaction in the previous question at 298 Kelvin where H2 has a partial pressure of 0.10 bar, O2 is at 0.20 bar, and H2o is at 1.5 bar:
(a) Determine the direction and quantify the change in free energy the reaction must undergo to reach equilibrium.

(b) Calculate the equilibrium constant.

(c) Illustrate the reaction on a plot of Free Energy versus % Reactants/Products (show ?GO, the approximate position of Q for the given partial pressures, and the position of Q at equilibrium).

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