A 50.0-mL sample of 0.15 M acetic acid, CH3COOH (Ka = 1.82 x 10-5 ), is titrated with 0.15 M NaOH solution. Calculate the pH after the following volumes of base have been added: (a) 0 mL (b) 50.0 mL

What is the pH of the following buffer mixtures? (a) 100 mL 1 M acetic acid plus 100 ml 0.5 M sodium acetate (b) 250 ml 0.3 M phosphoric acid plus 250 mL 0.8 M KH;PO,

Determine the pH during the titration of 58.9 mL of 0.341 M formic acid (Ka = 1.8×10-4) by 0.341 M NaOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any NaOH (b) After the addition of 14.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint)  (d) At the equivalence point  (e) After the addition of 88.4 mL of NaOH

A buffer solution contains 0.50 M acetic acid (CH3COOH; Ka = 1.8 x 10–5) and 0.35 M sodium acetate, NaCH3CO2. What is the pH of the solution?           (A) 4.59          (B) 4.90          (C) 2.29          (D) 2.52

A 21.0 mL sample of 0.308 M methylamine, CH3NH2, is titrated with 0.245 M hydrobromic acid.At the titration midpoint, the pH is

t ent Determine the pH during the titration of 64.4 mL of 0.443 M acetic acid (K₂ = 1.8x10-5) by 0.443 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 96.6 mL of KOH

You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?

Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, Kp = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4

The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic base with a 0.10 M solution of a strong monoprotic acid. (a) What is the pH before any titrant has been added? (b) Wh Data points at 1 mL increments. the pH the midpoint the titration? (c) What is the pH at the equivalence point? (d) What is the value of K, for the weak base? 12.0 10.0 8.0 2 6.0 4.0 2.0 0.0 0.0 10.0 20.0 PODAAAAAAAÀÀÀÀÀÀÀÀÀOOOOOOO 30.0 Volume of titrant (mL) 40.0 50.0

Consider the titration of 25.00mL of 0.200M Methylene (CH3NH2). The titrant is 0.120M HCL. Calculate each of the following. (a) the initial pH of base? (b) the pH of 5.00mL added? (c) the pH at 1/2 the HCl needed to reach equivalence point? (d) the volume of added acid required to reach equilibrium? (e) the pH at equivalence point?