Consider the titration of a 25.0mL sample of 0.125M HCN (ka=6.17x10^-10) with a 0.160 M KOH.
What is the initial pH?
What is the pH after adding 6 mL of KOH?
Consider the titration of a 25.0mL sample of 0.125M HCN (ka=6.17x10^-10) with a 0.160 M 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?
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?
2. Consider the titration of 25.0mL of 0.100M formic acid with 0.100 M NaOH (Ka= 1.8 x 10-4). Part IV. What is the pH after adding 25.0mL of NaOH? a)5.60 b) 8.23 c) 9.80 d)13.00 Answer is B
Calculate the pH for each case in the titration of 50.0 mL of 0.160 M HClO(aq) with 0.160 M KOH(aq). ionization constant=4.0×10^–8 What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 40.0 mL KOH? pH = What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of 60.0 mL KOH? pH...
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?
Consider the titration of a 40.0 mL sample of 0.150 M HCl with 0.200 M KOH a) What is the initial pH? b) What is the pH after the addition of 10.0 mL of the KOH? c) What is the pH at the equivalence point? d) What is the pH after 40.0 mL of KOH has been added?
Consider the titration of 25.0 mL of 0.100 M HF with 0.125 M KOH. The Ka is 6.8 x 10-4 for HF. What is the pH after 20.0 mL of base are added? Please show steps.
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)
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?
Consider the titration of a 33.0 mL sample of 0.180 M HBr with 0.210 M KOH. Determine the following: the pH after adding 5.0 mL of base beyond the equivalence point. Express your answer using two decimal places.