Formation Constant. In general, chemical equilibrium is reached when the forward reaction rate is equal to the reverse reaction rate and can be described using an equilibrium constant, K K. xM(aq) + yL(aq) ↽−−⇀ MxLy(aq) x M ( aq) + y L ( aq) ↽ − − ⇀ M x L y ( a q) Complex ion equilibria are no exception to this and have their
The equilibrium constant, K, describes the relative amounts of reaction species at equilibrium. The expression for K is equal to the concentrations (or partial pressures) of the products raised to their stoichiometric coefficients divided by the concentrations (or partial pressures) of the reactants raised to their stoichiometric coefficients. Example 13.4.3: Calculation of a Missing Equilibrium Concentration. Nitrogen oxides are air pollutants produced by the reaction of nitrogen and oxygen at high temperatures. At 2000 °C, the value of the equilibrium constant for the reaction, N 2(g) + O 2(g) ⇌ 2NO(g), is 4.1 × 10 −4. The ionization constant for the acid (K a) or base (K b) is a measure of how readily the acid donates protons or how readily a base accepts protons. Because you are calculating pH, you must solve for the unknown concentration of hydronium ions in solution at equilibrium. If the equilibrium constant is 1 or nearly 1, it indicates that the molarities of the reactants and products are about the same. If the equilibrium constant value was a large number, like 100, or a very large number, like \(1 \times 10^{15}\), it indicates that the products (numerator) are a great deal larger than the reactants. XHUt.