Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb= 5.2 x 10^-4), with 0.1000 M HCl solution after each of the following additions of titrant: a) 20.00mL

Find the pH of the equivalence point(s) and the volume(mL) of 0.0588 M KOH needed to reach it in titrations of(a) 23.4 mL of 0.0390 M HNO₂(b) 17.3 mL of 0.130 M H₂CO₃(two equivalence points

Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N, with 0.1000 M HCl solution after the following additions of titrant. 10.00 mL: 21.00 mL: 28.00 mL:

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The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic acid with a 0.10 M solution of a strong monoprotic base. Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the titration? (c) What is the pH at the equivalence point? (d) What is the value of K₂ for the weak acid? 14.0- 12.0 10.0 € 8.0 6.0 4.0 2.0 0.0 + 0.0 10.0 20.0 ÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄKAAAAA 30.0 Volume of titrant (mL) 40.0 50.0

Consider the titration of 25.00mL of 0.200M methylamine (CH3NH2). The titrant is 0.120M HCl. (Calculate each below using ICE and ICF tables.) Note you should NOT use M1V1=M2V2 (a) the initial pH of base? (b) the pH at 5.00mL added? (c) the pH at 1/2 the HCl needed to reach the equivalence point. (d) the volume of added acid required to reach the equivalence point? (e) the pH at equivalence point.

la) A 26.9 mL sample of 0.261M dimethylamine, (CH3)2NH, is titrated with 0.216 M hydrobromic acid. After adding 51.4 mL of hydrobromic acid, the pH is 1b) A 22.3 mL sample of 0.207 M diethylamine, (C2H5)2NH, is titrated with 0.377 M hydrobromic acid. At the titration midpoint, the pH is

Determine the pH during the titration of 60.4 mL of 0.442 M formic acid (Ka = 1.8×10-4) by 0.442 M KOH at the following points.   At the equivalence point (e) After the addition of 90.6 mL of KOH