The acid-base reaction with Kc > 1 = HNO₃ + F⁻ ⇄ NO₃⁻ + HF
The acid-base reaction with Kc < 1 = HF + NO₃⁻ ⇄ F⁻ + HNO₃
In chemistry, the equilibrium constant Kc or Keq is used to represent the ratio of the concentrations of all the chemicals involved in an equilibrium process. The law of mass action is explicitly considered in relation to it.
It is therefore also known as the mass action constant, though it is more usually referred to as the equilibrium constant. In contrast to the equilibrium position, the equilibrium constant's value is purely based on temperature and is unaffected by pressure or concentration.
Any reversible process in equilibrium will always have a ratio of reactants to products that is equal to Kc at a particular temperature.
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