What is the pH of a buffer that is 0.185 M in a weak acid and 0.227 M in the acid's conjugate base? The acid's ionization constant is 5.7×10-4 pH =

A 2.00 L solution contains 0.545 M NH3 and 0.641 M NH4A.  (The Kb of NH3 is 1.86⋅10−51.86⋅10-5). What is the pH of this solution?   What is the pH of this solution after 0.121 mol of HCl are added to the solution?   What is the pH of this solution after 0.242 mol of HCl are added to the solution?

An aqueous solution contains 0.302 M ammonia (NH3). How many mL of 0.393 M perchloric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 9.240? mL

a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…

Near the equivalence point in the titration of a strong acid with a strong base, one drop of base can cause the pH of the solution in the flask to change from 6.0 to 8.0. What is the relationship between the hydrogen ion concentrations at the two pH values? (A) The [H+] would be 100 times higher at pH 8.0 than 6.0. (B) The [H+] would be 200 times higher at pH 6.0 than 8.0. (C) The [H+] would be 2 times higher at pH 6.0 than 8.0. (D) The [H+] would be 2 times higher at pH 8.0 than 6.0. (E) The [H+] would be 100 times higher at pH 6.0 than 8.0.

A 0.581 M solution of a weak base has a pH of 11.86. What is the base hydrolysis constant, Kp, for the weak base? Kh =

Calculate the pH for each of the cases in the titration of 35.0 mL of 0.240 M KOH(aq) with 0.240 M HCl(aq). Note: Enter your answers with two decimal places. before addition of any HCl: after addition of 13.5 mL HCl: after addition of 21.5 mL HCl: after addition of 35.0 mL HCl: after addition of 41.5 mL HCl: after addition of 50.0 mL HCl:

From the options below, select the three (3) methods that could be used to form a buffer solution: Select 3 correct answer(s) Adding a strong base to a weak acid solution Adding a strong base to a weak base solution Adding a strong acid to a weak acid solution Adding a weak acid (or weak base) to a solution of a salt of that weak acid (or weak base) Adding a weak acid (or weak base) to any salt solution Adding a strong acid to a weak base solution

If a buffer solution is 0.180 M in a weak base (Kb=7.5×10−5) and 0.400 M in its conjugate acid, what is the pH?

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?