Consider the titration of 50.0mL of 0.10M H3A (Ka=5.0x10^-4, Ka2=1.0x10^-8 Ka3=1.0x10^-11) titrated by 0.10 M KOH...

Question

Question

Consider the titration of 50.0mL of 0.10M H3A (Ka=5.0x10^-4, Ka2=1.0x10^-8 Ka3=1.0x10^-11) titrated by 0.10 M KOH

a)Calculate the pH of the resulting solution at 125mL of KOH added

b) At what volume of KOH added does pH=3.30

c) At 75.0mL of KOH added, is the solution acidic or basic?

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Consider the titration of 100.0 mL of 0.27 M H3A by 0.27 M KOH for the...

Consider the titration of 100.0 mL of 0.27 M H3A by 0.27 M KOH for the next three questions. The triprotic acid has Ka1 = 1.0 x 10-3, Ka2 = 1.0 x 10-6, and an unknown value for Ka3. 1) Calculate the pH after 100.0 mL of KOH has been added. pH = 2) Calculate the pH after 150.0 mL of KOH has been added. pH = 3) The pH of the solution after 200.0 mL of KOH has been...
Consider the titration of 100.0 mL of 0.75 M H3A by 0.75 M KOH for the...

Consider the titration of 100.0 mL of 0.75 M H3A by 0.75 M KOH for the next three questions. The triprotic acid has Ka1 = 1.0 x 10-5, Ka2 = 1.0 x 10-8, and an unknown value for Ka3. 1) Calculate the pH after 100.0 mL of KOH has been added. pH = Tries 0/45 2) Calculate the pH after 150.0 mL of KOH has been added. pH = Tries 0/45 3) The pH of the solution after 200.0 mL...
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10...

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?

If 100mL of 0.10M CH3COOH (Ka=1.8x10-5) is titrated with 0.10 M NaOH. Calculate the pH value...

If 100mL of 0.10M CH3COOH (Ka=1.8x10-5) is titrated with 0.10 M NaOH. Calculate the pH value for the following solution. A. 75.0 mL of NaOH is added B. 100.0 mL of NaOH is added C. Suggest an indicator for this titration
24. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10-5) is titrated with a 0.10 M KOH solution. After 50.00 mL of the KOH solu...

24. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10-5) is titrated with a 0.10 M KOH solution. After 50.00 mL of the KOH solution is added, the pH in the titration flask will be A) 4.28 B) 8.72 C) 9.41 D) 11.24 E) 12.08 [Kb = 5.6 x 10-10 for acetate ion] 0.0025 - 0.25 .
25. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10") is titrated with a...

25. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10") is titrated with a 0.10 M KOH solution. After 75.00 mL of the KOH solution is added, the pH in the titration flask will be A) 9.31 B) 9.18 C) 9.52 D) 11.63 E) 12.30

Consider the titration of 45.0 ml of 0.10 MHCl with 0.10 M KOH .

This question has multiple parts. Work all the parts to get the most points. Consider the titration of 45.0 ml of 0.10 MHCl with 0.10 M KOH .What is the total solution volume at the equivalence point?Without doing detailed calculations, indicate the approximate pH at the beginning of the titration and at the equivalence point. pH at the beginning = _______ pH at the equivalence point = _______
Consider the titration of a 25.0mL sample of 0.125M HCN (Ka = 6.17x10^-10) with 0.160 M...

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 100.0 mL of 0.200M acetic acid (CH3COOH, Ka=1.8 x10-5) by 0.100M KOH....

Consider the titration of 100.0 mL of 0.200M acetic acid (CH3COOH, Ka=1.8 x10-5) by 0.100M KOH. Calculate the pH of the resulting solution after 50.0 mL 0.100M KOH is added.

Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the...

Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL pH = b. 10.0 mL pH = c. 60.0 mL pH = d. 80.0 mL pH = e. 110.0 mL pH = Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the...