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

The velocity function of a moving object at time is given by

Which command would capitalize all the letters in the file info.txt?