Consider the titration of 100.0 mL of 0.42 M H3A by 0.42 M KOH for the...

Consider the titration of 100.0 mL of 0.42 M H₃A by 0.42 M KOH for the next three questions. The triprotic acid has K_a1 = 1.0 x 10^-4, K_a2 = 1.0 x 10^-7, and an unknown value for K_a3. All answers to 3 significant digits.

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 added is 9.00. Determine the value of K_a3 for this triprotic acid. Use scientific notation to enter this answer, e.g., 1.0 x 10^-3 = 1.0E-3.

Ka₃ =

Solutions

Expert Solution

queen_honey_blossom answered 2 months ago

Next > < Previous

Related Solutions

Consider the titration of 100.0 mL of 0.43 M H3A by 0.43 M KOH for the...

Consider the titration of 100.0 mL of 0.43 M H3A by 0.43 M KOH for the next three questions. The triprotic acid has Ka1 = 1.0 x 10-4, Ka2 = 1.0 x 10-7, and an unknown value for Ka3. 1) Calculate the pH after 100.0 mL of KOH has been added. 2) Calculate the pH after 150.0 mL of KOH has been added. 3) The pH of the solution after 200.0 mL of KOH has been added is 9.00. Determine...

titration of 100.0 mL of 0.6 M H3A by 0.6 M KOH for the next three...

titration of 100.0 mL of 0.6 M H3A by 0.6 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. Calculate the pH after 150.0 mL of KOH has been added.The pH of the solution after 200.0 mL of KOH has been added is 8.00. Determine the value of Ka3 for...

Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25°C....

Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25°C. Ka for HCN = 6.2×10-10. Part 1 Calculate the pH after 0.0 mL of KOH has been added. pH = Part 2 Calculate the pH after 50.0 mL of KOH has been added. pH = Part 3 Calculate the pH after 75.0 mL of KOH has been added. pH = Part 4 Calculate the pH at the equivalence point. pH = Part 5 Calculate...

Consider the titration of 100.0 mL of 0.400 M C5H5N by 0.200 M HCl. (Kb for...

Consider the titration of 100.0 mL of 0.400 M C5H5N by 0.200 M HCl. (Kb for C5H5N = 1.7×10-9) Part 1 Calculate the pH after 0.0 mL of HCl added. pH = Part 2 Calculate the pH after 35.0 mL of HCl added. pH = Part 3 Calculate the pH after 75.0 mL of HCl added. pH = Part 4 Calculate the pH at the equivalence point. pH = Part 5 Calculate the pH after 300.0 mL of HCl added....

Consider the titration of 100.0 mL of 0.400 M C5H5N by 0.200 M HCl. (Kb for...

Consider the titration of 100.0 mL of 0.400 M C5H5N by 0.200 M HCl. (Kb for C5H5N = 1.7×10-9) Part 1 Calculate the pH after 0.0 mL of HCl added. pH = Part 2 Calculate the pH after 25.0 mL of HCl added. pH = Part 3 Calculate the pH after 75.0 mL of HCl added. pH = Part 4 Calculate the pH at the equivalence point. pH = Part 5 Calculate the pH after 300.0 mL of HCl added....

Consider the titration of 100.0 mL of 0.400 M HONH2 by 0.200 M HCl. (Kb for...

Consider the titration of 100.0 mL of 0.400 M HONH2 by 0.200 M HCl. (Kb for HONH2 = 1.1×10-8) Part 1 Calculate the pH after 0.0 mL of HCl added. pH = Part 2 Calculate the pH after 40.0 mL of HCl added. pH = Part 3 Calculate the pH after 75.0 mL of HCl added. pH = Part 4 Calculate the pH at the equivalence point. pH = Part 5 Calculate the pH after 300.0 mL of HCl added....

Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the...

Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the milliliters of base that must be added to reach the first, second, and third equivalence points.

Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the...

Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added. Va = 0 mL Va = 1.0 mL Va = 5.0 mL Va = 9.0 mL Va = 9.9 mL Va = 10.0 mL Va = 10.1 mL Va = 12.0 mL Make a graph of pH versus Va = 0, 1.0, 5.0, 9.0, 9.9, 10.0, 10.1, and 12.0 mL.

Consider the titration of 20.00 mL of 0.100 M HBr with 0.150 M KOH at 25...

Consider the titration of 20.00 mL of 0.100 M HBr with 0.150 M KOH at 25 °C. What would be the pH of the solution when 20.00 mL of KOH have been added?

Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.200 M KOH....

Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.200 M KOH. Determine each of the following: 1. initial pH 2. the volume of added base required to reach the equivalence point 3. pH at 10.4 mL of added base 4. pH at the equivalence point

Subjects