1. Make sure you show your blank sheet of paper, front and back (both sides need to be blank), clearly to the webcam before starting the exam.  2. Also, please complete a scan of your desk area. 3. Finally, please read and acknowledge the statement below.  Basically, this is a reminder to only submit your own work and do not receive or give assistance of any kind or use unauthorized materials.   Good luck!

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.3567 M NaOH? Ka =1.8 × 10-4 for formic acid.

Show all Work 50.0 mL of 0.20 M NH3 titrated with 0.25 M HCl (Kb = 1.8 x 10–5, pKb = 4.74) a) What is the pH of the solution at the start of the titration? b)after 18.0 mL of titrant have been added? c)at the equivalence point? d)at the half-equivalence point? e)after 50.0 mL of titrant have been added? Sketch the titration curve.

Consider the following reaction at equilibrium.  What will happen if the pressure increased?             4 FeS2(s) + 11 O2(g)  ⇌  2 Fe2O3(s) + 8 SO2(g)

Consider the position function of a moving object, given by

A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of hydrofluoric acid is 3.5 × 10-4.

Based on your prior understanding of equilibrium (Le Chatelier’s principle) explain why the percent ionization of a weak acid decreases as the concentration of the acid increases. Hint: think of the dissociation equilibrium of a weak acid, HA:

Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point?

A buffer can be prepared by the combination of a weak acid and its conjugate base. However, a buffer can’t be prepared from a strong acid and its conjugate base. Briefly explain why?

(a) Consider the function Find the point at which