14. Consider this titration curve and answer questions a-h. (2 pts each) 14 12 10 4. 2. 10 15 20 25 30 35 40 ml base added a) This is a (strong/weak) acid titrated with a strong base. b) Place a dot () on the curve at the equivalence point. c) The pH at the equivalence point is d) What volume of base was used to titrate the acid solution to the equivalence point? e) Place a box () on the curve at the half-equivalence point. ) What is the pH at this point?

14. Consider this titration curve and answer questions a-h. (2 pts each) 14 12 10 4. 2. 10 15 20 25 30 35 40 ml base added a) This is a (strong/weak) acid titrated with a strong base. b) Place a dot () on the curve at the equivalence point. c) The pH at the equivalence point is d) What volume of base was used to titrate the acid solution to the equivalence point? e) Place a box () on the curve at the half-equivalence point. ) What is the pH at this point?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

See similar textbooks

Similar questions

Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?
A best buffer has about equal quantities of weak acid and conjugate base present as well as having a large concentration of each species present. Explain.
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
Calculate the pH during the titration of 50.00 mL of 0.100 M Sr(OH)2 with 0.100 M HNO3 after 0, 50.00, 100.00, and 150.00 mL nitric acid have been added. Graph the titration curve and compare with the titration curve obtained in Exercise 16.22.