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To do this, we complete a second concentration table, using as initial concentrations those calculated for the first equilibrium Reaction Initial concentration (M) 0 Change in concentration (M) Equilibrium concentration (M) x Substitute equilibrium concentrations into the equilibrium constant expression and solve for x, making the approximation that This value is too small to cause a measurable change in the concentrations already calculated, but it does tell us the concentration of carbonate anions in the solution One more ion remains, , generated from the water equilibrium. ovid.
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