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The opposite will occur if the reaction quotient is too tiny. If you just have acid, then you have to do a pure K problem and should you just have base (such as whenever the titration is complete) then you have to do a K issue. They can then be combined to give an overall equation for any redox reaction.

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To keep equilibrium temperature must be constant. Assume that the temperature of the reaction is currently altered, and it’s now T2. Substituting that which we know more about the system at equilibrium into the Ka expression provides the next equation.

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