9 Question 10 - Ch 19 HW - Conne X b Answered: Find the pH of the equ b Success Confirmation of Questio G (a) 0.10 M CH3NH2(Kb = 4.4 x 1 X + -> i ezto.mheducation.com/ext/map/index.html?_con=con&external_browser=0&launchUrl=https%253A%252F%252Fnewconnect.mheduc. * Paused Be sure to answer all parts. Find the pH of the two equivalence points and the volume (mL) of 0.0888 M KOH needed to reach them in the titration of 17.3 mL of 0.130 M H2CO3. First equivalent point Second equivalent point mL KOH mL KOH pH pH = 70°F 2:20 PM Sunny 4/24/2022

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:

Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C₁H₁N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH = pH = pH = 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrect

Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300 M NaOH. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Use a BCA table to detrmine the moles of reactant and product after the reaction of the acid and base. Ignore the amount of liquid water. Then, set up an ICE table to identify the unknown. Then figure the pH.

19) What is the solution pH when 0.10 mol of H+ is added to a 2.0-liter buffered solution created from 0.31 M NH3 (Kb = 1.8 × 10–5) and 0.26 M NH4F.

Calculate the equivalence point volume in the titration of 15.00 mL of 0.2654 M HBr with 0.5678 M Ba(OH)2.

Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl.  The Ka of HN3 is 2.2 x 10–5.   What is the pH at the equivalence point?

Calculate the pH at the equivalence point for the titration of 0.230 M methylamine (CH 3 NH 2 ) with 0.230 M HCI. The Kb of methylamine is 5.0 * 10 ^ - 4

Consider the titration of 25.0 mL of 0.766 M KOH with 1.25 M HBr. Calculate the pH after the addition of 17.64mL of HBr