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You would use the Ka or Kb value and use an ice table to solve for x. If you're given the final concentration of any of the products you can work backwards, since the change in product concentration is equal to the final concentration.
You have to solve for the value of x most of the time, using K values (including Ka or Kb) set equal to the equilibrium expression. From there you can add x to the products and subtract it from reactants to find final concentrations.
What everyone else said above is correct. Something to keep in mind is that if you are calculating for a weak acid/base, the change in molarity at equilibrium can be considered negligible because they do not 100% dissociate in solution. So, even though you have a change in X, the change is still close to 0 and can be considered 0.
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