2. Calculate the pH at each stage in the titration for the addition of 0.110 M HCL to 35.0 mL of 0.105 M NaOH. d. at the equivalence point. e. after the addition of 5.00 of acid beyond the equivalence point. f. after the addition of 10.0mL of acid beyond the equivalence point

Determine the pH at the point in the titration of 40.0 mL of 0.200 M HNNH2 with 0.100 M HNO: 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 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]

Please don't provide handwritten solution ....

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.

2. Fill in the following table to show the theoretical results for the titration of 1.0 L of 0.20 M acetic acid by adding the designated amount of solid (no volume change) potassium hydroxide, KOH. Show sample calculation of your work. Amount of NaOH added 0.0 mol 0.010 mol 0.020 mol 0.030 mol 0.040 mol Amount of acetic acid remaining pH [H+]

True or False To calculate the pH before the start of the titration of a weak acid with a strong base requires an I.C.E table.   True or False You can use the Henderson-Hasselbalch equation to calculate the pH at the equivalence point of a weak acid/strong base titration.

Question 7

25.0 ml of 0.100M NaOH is titrated with HC2H3O2  and 50.0mL of the acid is used to reach the endpoint.          e)Would the compound formed at the equivalence point be acidic, basic or neutral?  Write a hydrolysis equation for the salt formed in a) to support your answer. f) Which indicator should be used for this titration?  g)Sketch a titration curve for this reaction. Label the x and y axes.

Weak Base + Strong Acid Titration - Example Problem: Titration of 25 mL of .1 M NH3 With .1 M HCl: a. 0 mL b. 12.5 mL c. 20 mL d. 25 mL e 30 mL   I do know the corrects answers, I just don't know how to get to the answers. a. pH = 11.13 b. pH = 8.25 c. pH = 7.65 d. pH = 4.78 e. pH = 2.04