6. Calculate the pH of a solution during a titration of 2.5M HCI with 35mL of 1.25M NaOH A. 12mL of HCI? B. 30mL of HCI? C. How many mL of HCl are needed to reach the equivalence point?

71. Consider the titration of a 20.0-mL sample of 0.105 M HC,H;O2 with 0.125 M NaOH. Determine each quantity. a. the initial pH b. the volume of added base required to reach the equivalence point c. the pH at 5.0 mL of added base d. the pH at one-half of the equivalence point e. the pH at the equivalence point f. the pH after adding 5.0 mL of base beyond the equivalence point

A 5.36–g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L. a. What is the pH of this buffer solution? b. Is the solution acidic or basic? c. What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?

Pls help me !! A 150.0 mL sample of 0.21 M HF is titrated with 0.50 M NaOH. Determine the pH at these points:   a.At the beginning (before base is added) b.After adding 40.0 mL of NaOH After adding c.63.0 mL of NaOH 9

4. Calculate the pH at each point of a titration where 30.0 ml of 0.25M HNO3 are titrated with the following volumes of 0.15M LiOH. a. 15.0ml b. 25.0ml c. 50.0ml d. 60.0ml

HF is being titrated with NaOH. The equivalence point of this titration would be а. acidic b. basic C. neutral

What is the pH of a buffer made by combining 45 ml of 0.15M nitrous acid and 20 ml of 0.175 M sodium nitrite a. 3.43 b. 3.64 c. 3.28 d. 3.06

A 25.31 ml solution of a weak acid, 0.211M, is titrated with 0.338M. The ka of the acid is 1.3 x 10^-7. Calculate the pH after these volumes of NaOH have been added. Round all answers to two decimal places a. 0.00ml added (a) b. 3.16ml added c. at the equivalence point d. 15.96ml

A student is titrating a 100 mL of 0.50 M solution of hydrofluoric acid (HF) with 1.0 M strong base (NaOH). a) at the equivalence point, what ions/compounds will be present in the solution? A complete answer will also be specific as to what ions/compounds are not present in solution. b) calculate the pH at the equivalence point.

Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid, Ka = 4.9 x 10-5, with 0.100 M NaOH at the following points: a. Before any NaOH is added.      b. After 18.7 mL of NaOH are added.   c. After 25.00 mL of NaOH are added.   d. After 50.00 mL of NaOH are added.   e. After 53.00 mL of NaOH are added.   C) What is the pKa of the acid (show calculation)? please solve sub-parts a,b, and c.