6D.3 7th

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6D.3 7th

Postby Jordan_Wesson_2J » Thu Jan 24, 2019 9:37 pm

Why must we subtract the calculated concentrations of H+ and OH- from the initial concentration when plugging it into the Kc equation?

Vy Lu 2B
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Re: 6D.3 7th

Postby Vy Lu 2B » Thu Jan 24, 2019 11:59 pm

When using the equilibrium constant expression, we look at the equilibrium reaction in terms of reactants or products decreasing to increase reactants or products; subtract what will dissociate and add what will be formed. Whether or not the concentrations of H+ or OH- is subtracted depends on the context of the problem; rather often times those concentrations are increases in the reaction, not subtracted.

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