2. Consider the titration of 100.0 mL of 0.200 M HONH2 by 0.100 M HCl (K for HONH2 = 1.1 x 10-8)? a. Calculate the pH after 0.0 mL of HCl has been added. b. Calculate the pH after 25.0 mL of HCl has been added. c. Calculate the pH at the equivalence point. d. Calculate the pH after 300.0 mL of HCl has been added. e. Using the table of color indicators in the lecture slides, indicate one color indicator which would suit this titration.

Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. PREV 1 2 4 NEXT Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. 3.0 x 10-6 %3D 5 RESET [0] [0.200] [0.0200] [0.100] [0.140] [0.175] [x] [2x] [0.200 + x] [0.200 - x] [0.0200 + x] [0.0200 - x] [0.100 + x] [0.100 - x] [0.140 + x] [0.140 - x] [0.175 + x] [0.175 - x] II

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH,NH2, are titrated with 0.100 M HI. a. What is the volume of added acid at the equivalence point for each titration? b. Is the pH at the equivalence point for each titration acidic, basic, or neutral? c. Which titration curve has the lower initial pH? d. Sketch each titration curve.

Moving to another question will save this response. uestion 5 In the titration of 0.100 M HNO3 with the titrant 0.100 M KOH, what species are present at any point after KOH has been added but before the equivalence point? a. KOH only b. KNOJ only c. HNOJ and KNO d. HNO3 only e. HNO3 and KOH

A solution of 25.0 mL 0.200 M CH3COOH solution is titrated with 0.200 M KOHsolution.a. Calculate the pH when 10.0 mL of KOH is added.b. Calculate the pH of the solution at the equivalence point.Ka for CH3COOH = 1.8x10-5; Kb for CH3COO- = 5.6x10-10.

Please don't provide handwritten solution ....

25.00 mL sample of 0.08000 M HNO2 (Ka = 4.0 × 10-4) is being titrated with 0.1000 M NaOH. a. Calculate the initial pH of the acid. b. Calculate the pH at 5.00 mL before the equivalence point. c. Calculate the pH at the equivalence point. d. Calculate the pH at 5.00 mL after the equivalence point.

Strong acid-strong base titration 6) A 100.0 mL sample of 0.18 M HCIO4 is titrated with 0.27 M LIOH. Determine the pH of the solution a) before the addition of any b) after the addition of 30.0 mL of LİOH. c) after the addition of 50.0 mL of LIOH. d) after the addition of 66.67 mL of LiOH (this is the equivalence point). e) after the addition of 75.0 mL of LIOH. LIOH.

Question 7

23.Determine the pH ranges of the equivalence points in the titration curve below.