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For a weak acid HA with Ka = 1.0 x 10^-5, if the initial concentration of HA is 0.1 M and the equilibrium concentration of A- is 0.02 M, what is the pH of the solution?

In the balanced half-reaction: 2 Fe3+ + 2 e- → 2 Fe2+, the iron species is:

If the Ka value for a weak acid HA is 1.0 x 10^-4, and the pH of a 0.2 M solution of HA is 3.6, the value of [A-] at equilibrium is approximately:

If the Ksp value for a slightly soluble salt AB is 1.0 x 10^-8, and the concentration of A+ at equilibrium is 1.0 x 10^-3 M, the concentration of B- at equilibrium is:

For a weak base BOH, the Henderson-Hasselbalch equation is:

If the Ksp value for a slightly soluble salt AB2 is 1.0 x 10^-10, and the concentration of A2+ at equilibrium is 1.0 x 10^-4 M, the concentration of B- at equilibrium is:

The equilibrium constant (Kc) for a reaction is:

For the slightly soluble salt Ag2CrO4, the equilibrium reaction is:

For the reaction: 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g), the value of Kc at a certain temperature is 4.0. If the initial concentrations are [SO2] = 0.5 M, [O2] = 0.2 M, and [SO3] = 0 M, the direction of the net reaction at equilibrium is:

If a reaction has a very small equilibrium constant (Kc