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^-8, and the concentration of A+ at equilibrium is 1.0 x 10^-3 M, the concentration of B- at equilibrium is:

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 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.

Access Lecture 11 Part II & Lecture 12 here. Lecture 11 – Depreciation Lecture 12 TVOM Tables If it doesn’t let you access the links, please contact Honorlock Support in the chat on your screen and they should be able to fix it for you immediately. MACRS-GDS Tables are given below.