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What is the cell potential (Ecell) for the following balanced redox reaction: 2 Fe3+(aq) + Sn(s) → 2 Fe2+(aq) + Sn2+(aq), given that E°(Fe3+/Fe2+) = 0.77 V and E°(Sn2+/Sn) = -0.14 V?

For a weak acid HA with Ka = 1.0 x 10^-6, if the pH of the solution is 5.0, what is the ratio of [A-]/[HA] at equilibrium?

If the Ka value for a weak acid HA is 1.0 x 10^-5, and the initial concentration of HA is 0.2 M, the hydronium ion concentration at equilibrium is approximately:

The relationship between ΔG, ΔH, and ΔS at constant temperature is given by:

For the weak acid H3PO4 (phosphoric acid), the first dissociation step is:

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: