Question

9.& 10.) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution at each addition of the HNO3. The Kb of NH3 is 1.8 x 10-5 (Yes, you may use the back or attach sheets to show your work.) Addition of HNO3 pH 150 200 Then sketch the titration curve for this titration. Make sure to label your axes (including numerically!), to indicate the equivalence point (and whether it is acidic, basic or neutral), and to box the buffer region. (Yes, you may use graph paper. Yes, you may calculate as many additional points as you like to flesh out the shape Yes, you may use a computer, but if you do, be very careful of shope!)

Answer 1

July '09 When addition of HNO3 a 100 mL. pH = 7- bpkb - I Log C 7- 4.79 ļ loglo.05) - 5.28 -When addition of HiNaz 150 m .: pH = -log( 50 X61) when addition of HNO is 200 pH = -log (100x 0.1 2 1.97

July of Thursday We 29 . 16 when Addition of hinog 20 ml [NHz] -0.1 (M) NH3 pOH = 1/2 pkb - 1 loge }{-log(i-9x16 5) – Slag16 = 1 £ 4.74 + 2 } - 2.62 ². PH = 14-POH = 11:38 When addition of HNO3 = 50m2 : 50 mL NH3 reacts with 50mL 3 so excess NH3 concentration a 50% 0-1 = 0.033 It's a buffer So ENHANO] soln pH = pky + Log In 2.4.74 4889601033) (NH37 2 4.74 + leq 0.03 JULY M T W T F S S M T W T F S S 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 24.44