If the pH of a 0.1 M solution of a weak acid HA is 4.2, the value of Ka for HA is approximately:

For a weak acid HA, the Henderson-Hasselbalch equation 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 = 0.5 M, = 0.2 M, and = 0 M, the direction of the net reaction at equilibrium is:

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

If the pH of a solution is 3.7, what is the hydronium ion concentration?

If the Ksp value for a slightly soluble salt AB is 1.0 x 10^-6, and the equilibrium concentration of both A+ and B- is 1.0 x 10^-3 M, the value of the ion product Q is:

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:

If the pH of a solution is 11.2, what is the hydronium ion concentration?

If the hydronium ion concentration of a solution is 1.0 x 10^-8 M, what is the pOH of the solution?

Attach a PDF of your work (as to how you calculated the solutions to each problem) to the assignment named ‘Quiz 8 Attachment’ within 15 minutes of submitting this quiz for full credit, else points would be deducted.