Hey guys i only have this question left on my review and i just can't fingure it out!

Sketch a pH curve for the titration of 40.00mL of 0.100 M hydrazine, H2NNH2, having a K of 3.0x10^-6 by 0.100 M HCIO4

a) what combination of acide-base titration is this? (SA-SB; SA-WB; or SB-WA)

b)Identify and buffering regions.

c) What is the predicted apporximate pH at equivalence point?

d) What is the voliume of HCIO4 added at the equivalence point?

e) How many "quantitative" or "stoichiometric" reactions are taking place?

f) Write an equation for any hydrolysis reaction taking place.

G) suggest a suitable indicator for this titration. Explain

We can't draw pictures on the board; however, here is a site that gives graphs of titration curves. The curve you want is a weak base/strong acid curve (HClO4 is a strong acid/hydrazine is a weak base).

http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA6/MAIN/1ChemLabMenu/Measuring/Titration/titr_menu/CURVES/CURVEINDSTILLS/MENU.HTM

that is helpful, i just don't get how to get the graph right, mine went up, how do i get the numbers and plot the graph correct?

To answer these questions and sketch a pH curve for the titration, you need to understand the basics of acid-base titrations and how to calculate pH values at different points in the titration process. Here's a step-by-step guide to help you find the answers:

Step 1: Determine the type of acid-base titration:
To identify the type of titration, check the strength of the acids and bases involved. In this case, we have hydrazine (H2NNH2) as a weak base and HCIO4 (perchloric acid) as a strong acid. Therefore, it is a weak base-strong acid titration. The correct combination is SA-WB (Strong Acid-Weak Base).

Step 2: Identify buffering regions:
Buffering regions occur before and after the equivalence point. These regions have a relatively stable pH due to the presence of a weak acid and its conjugate base or a weak base and its conjugate acid. In this titration, before the equivalence point, the buffering region contains a mixture of the weak base, hydrazine, and its conjugate acid. After the equivalence point, the buffering region contains only the excess strong acid, HCIO4.

Step 3: Predict the approximate pH at the equivalence point:
The equivalence point occurs when the number of moles of acid is stoichiometrically equal to the number of moles of base. In this titration, hydrazine and HCIO4 react in a 1:1 ratio. At this point, the resulting solution will be neutral, so the predicted approximate pH at the equivalence point is 7.

Step 4: Calculate the volume of HCIO4 at the equivalence point:
To find the volume of HCIO4 at the equivalence point, you need to set up a balanced equation and use stoichiometry. The balanced equation for the reaction between hydrazine and HCIO4 is:

H2NNH2 + HCIO4 -> H2NNH3+ + CIO4-

Since the reaction occurs in a 1:1 ratio, the volume of HCIO4 added at the equivalence point is equal to the initial volume of hydrazine, which is 40.00 mL.

Step 5: Determine the number of stoichiometric reactions:
The term "quantitative" or "stoichiometric" reactions refers to reactions that occur in exact stoichiometric ratios. In this titration, as mentioned in step 4, the reaction occurs in a 1:1 ratio. Therefore, only one stoichiometric reaction is taking place.

Step 6: Write an equation for any hydrolysis reaction taking place:
Hydrolysis reactions occur when a salt or its ions react with water to produce an acidic or basic solution. In this case, no hydrolysis reaction takes place because neither hydrazine nor HCIO4 are salts.

Step 7: Suggest a suitable indicator for this titration:
To suggest an indicator, you need to consider the pH range at which the indicator changes color. Since the predicted approximate pH at the equivalence point is 7, you need an indicator that changes color around pH 7. One suitable indicator is phenolphthalein, which changes from colorless to pink around pH 8.2-10.

Remember, when sketching the pH curve, the pH will be relatively high before the equivalence point (due to the weak base) and decrease sharply near the equivalence point before rising sharply after the equivalence point (due to the strong acid).

I hope this explanation helps you tackle the remaining questions and sketch the pH curve successfully!