A titration is performed on a 25 mL sample of 0.15 M HCN (Ka = 4.9 x 10–10) with 0.30 M NaOH. Which of the following is the pH of the solution after 15 mL of NaOH is added?
first to calculate the moles of each.
then to calculate the excess moles of base.
then to calculate Molarity and then pH.
A titration is performed on a 25 mL sample of 0.15 M HCN (Ka = 4.9...
Answer the following for a titration of 25.0 mL of 0.87 M HCN Ka = 4.9 x 10-10) with 0.39 M KOH. a.) The pH when 10.0 mL of KOH has been added. (6pts) b.) The pH at the equivalence point. (9pts)
Acid-Base Titration: A 0.15 M solution of NaOH is used to titrate 200.0 mL of 0.15 M HCN. What is the pH at the equivalence point? Ka = 4.9 x 10-10. Please include steps/work so I can see and understand how this problem is solved.
A chemist performs a titration experiment on a 35 mL sample of 0.10 M CH3NH3+ (Ka = 2.27 x 10−11) with 0.10 M NaOH. Determine the pH of solution after 25 mL of NaOH is added to the solution.
A 50.0-mL sample of 0.15 M butanoic acid, CH3CH2CH2COOH, is titrated with 0.30 M NaOH(aq). Ka for butanoic acid is 1.52 x 10-5 a) How many mL of NaOH(aq) are required to reach the equivalence point? b)What is the pH of the solution after 27.0 mL of NaOH(aq) have been added?
Consider the titration of a 25.0 mL sample of 0.125 M HCN (Ka= 6.17x10^-10) with a 0.160M KOH. What is the pH after 19.53mL of KOH? What is pH after 21.5mL of KOH?
Consider the titration of a 25.0mL sample of 0.125M HCN (Ka = 6.17x10^-10) with 0.160 M KOH. 1. What is the initial pH? 2. What is the pH at 6.00 mL base added? 3. What is the pH when 19.53 mL of KOH is added? 4. What is the PH if 21.5 mL of KOH is titrated with the solution?
A titration is performed on 50mL of a 0.10 M solution of HN3 (Ka+1.9x10-5) with 0.10 M NaOH as the titrant. (a) What is the initial pH of the HN3 solution? (b) Calculate the pH of the solution after 25 ml of NaOH have been added (c) How many mL of NaOH are required to reach the equivalence point and what is the pH of the solution at the equivalence point.
IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10) solution is titrated with 0.200 M NaOH. Find the pH before titration and after 25 mL, 50 mL, and 60 mL of NaOH has been added.
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
A titration of a 75.0 mL aqueous solution of 0.12 M acetic acid, a weak, monoprotic acid with a Ka of 1.76 × 10–5, with 0.30 M NaOH is performed. What is the pH of the solution after 10.0 mL of NaOH has been added (at 25oC)? Group of answer choices 5.24 3.98 8.21 6.17 4.45