Piperazine can be used as an anthelmintic (a drug that expels parasitic worms from the body).  It is a dibasic compound and has 2 pKb’s as shown below: Consider the titration of 50.00 mL of 0.05000 M piperazine is titrated with 0.1250 M HCl.  What is the pH after 40.00 mL of HCl have been added?

A student performs the titration of 88.0 mL of 1.1 M HCI (in flask) with 13.0 mL of 0.20 M NaOH (in burette). What is the pH at this point in the titration? (Hint: Use a barf table.) Your Answer: Answer

A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.

The acid HX has a pKa of 5.00.  If 25.00 mL of a 0.106 M solution of HX are titrated with 0.100 M NaOH solution, what's the pH after 11.28 mL ofbase solution is added?

100.7 mL of 0.51 M HNO3 titrated with 0.26 M NaOH. What is the pH at the halfway point?

How many moles of sodium hydroxide would have to be added to 225 mL of a 0.349 M nitrous acid solution, in order to prepare a buffer with a pH of 3.570? moles

A 25.0-mL sample of 0.10 M HCI is titrated with 0.10 M NaOH. What is the pH of the solution after 13.3 mL of NAOH have been added to the acid? Please report with 1 decimal place.

A biochemist prepares two stocks of sodium phosphate buffer by titrating phosphoric acid with sodium hydroxide. She prepares a 0.10 M solution of sodium phosphate buffer at pH 2.15, and she prepares a 0.10 M solution of sodium phosphate buffer at pH 7.20. If she mixes 48 mL of the pH 2.15 buffer with 29 mL of the pH 7.20 buffer, what will be the pH of the resulting solution? Recall that the pKas of phosphoric acid are 2.15, 7.20, and 12.35. Enter your answer to the nearest hundredth.

A 50.00-mL sample of 0.250 M HC2H3O2 was titrated with 0.125 M NaOH. What is the pH of the resulting solution after 45.0 mL of NaOH were added at 25°C?  Ka for HC2H3O2 is 1.8x10–5 at 25°C

A buffer solution is prepared by combining 0.795 moles of formic acid and 0.898 moles of sodium formate. What will the solution pH be if 0.120 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places)