a of m-chlorobenzoic acid, HC7H4CIO2, is 1.5x 10-4.(a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC7H4CIO2 and 60.0 mL 0.1 M C7H4CIO₂ to give a final volume of100.0 mL. What is the pH of this buffer?4.0(b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC7H4ClO2 and 40.0 mL 0.1 M C7H4CIO₂ to give a final volume100.0 mL. What is the pH of this buffer?4.0(c) Why is buffer #2 more acidic than buffer #1?O It has a greater volume of base.O It has a greater final volume.O It was prepared after buffer #1.It has a higher acid concentration.-

The Henderson-Hasselbalch equation for the acidic buffer solution is: pH=pKa+logsaltacid ......(1)

of m-chlorobenzoic acid, HC7H4CIO2, is 1.5x 10-4. (a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC7H4CIO2 and 60.0 mL 0.1 M C7H4CIO2 to give a final volume of 100.0 mL. What is the pH of this buffer? 4.0 (b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC7H4CIO2 and 40.0 mL 0.1 M C7H4CIO2 to give a final volume c 100.0 mL. What is the pH of this buffer? 4.0 (c) Why is buffer #2 more acidic than buffer #1? It has a greater volume of base. O It has a greater final volume. O It was prepared after buffer #1. It has a higher acid concentration.

of m-chlorobenzoic acid, HC7H4CIO2, is 1.5x 10-4. (a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC7H4CIO2 and 60.0 mL 0.1 M C7H4CIO2 to give a final volume of 100.0 mL. What is the pH of this buffer? 4.0 (b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC7H4CIO2 and 40.0 mL 0.1 M C7H4CIO2 to give a final volume c 100.0 mL. What is the pH of this buffer? 4.0 (c) Why is buffer #2 more acidic than buffer #1? It has a greater volume of base. O It has a greater final volume. O It was prepared after buffer #1. It has a higher acid concentration.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the pH for each of the following cases in the titration of 60.0 mL of 0.250-M hydrobromic acid, HBr(aq), with 0.250 M NaOH: (HBr is a strong acid) (a) before addition of any NaOH, (b) after addition of 30.0 mL of NaOH, (c) after addition of 50.0 mL of NaOH, (d) after addition of 60.0 mL of NaOH, and (e) after addition of 80.0 mL of NaOH
A solution is prepared that contains 25.0 mL pyridine, C5H5N, d = 0.978 g/ml and 27.6 g pyridinium hydrochloride, C5H5N • HCl. The volume of the aqueous solution is 250. mL. What is the pH of this buffer solution? (K₁ C5H5N = 1.5 × 10 %) A) 4.68 B) 5.17 C) 5.29 D) 8.82 E) 8.71 ||
Determine the pH during the titration of 59.5 mL of 0.490 M hypochlorous acid (Ką = 3.5×10-8) by 0.490 M NaOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.3 mL of NaOH
We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.44. We titrate this solution with a 0.250 M NaOH solution and we need 33.3 mL of this 0.250 M NaOH solution to reach the equivalence point. The temperature is 25.0 ◦C throughout. (a) What is the molar mass of HA? (b) What is the dissociation constant, Kb, of A−(aq)? (c) What would be the pH of a 2.222 M solution of A−(aq)?
We have 500.0 mL of a buffer solution which is 0.651 M in NH3 and 0.354 M in NH4Cl. 500.0 mL of a 0.224 M HCl solution are added. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the final pH of this solution?
Determine the pH during the titration of 59.7 mL of 0.392 M hypochlorous acid (K₂ = 3.5×10-8) by 0.392 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 13.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.6 mL of KOH Submit Show Approach Show Tutor Steps
What is the pH of a solution prepared by mixing 20.0 mL of 0.50 M NaOH and 35.0 mL of 0.50 benzoic acid solution? (Benzoic acid is monoprotic with a Ka of 6.5 x 10-5.)
TUTOR Analysis of a Weak Acid-Strong Base Titration Curve Determine the pH during the titration of 63.3 mL of 0.465 M formic acid (K₂ = 1.8×10) by 0.465 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 95.0 mL of KOH
For the titration of 50.0 mL of 0.150 M ethylamine. C2H5NH2,with 0.100 M HCl, find the pH at each of the following points, and then use that information to sketch the titration curve and decide on an appropriate indicator. (a) At the beginning, before HCl is added (b) At the halfway point in the titration (c) When 75% of the required acid has been added (d) At the equivalence point (e) When 10.0 mL more HCl has been added than is required (f) Sketch the titration curve. (g) Suggest an appropriate indicator for this titration.
For the titration of 75.00 mL of 0.1000 M0.1000 M acetic acid with 0.1000 M0.1000 M NaOH, calculate the pH (a) before the addition of any NaOH solution, (b) after 25.00 mL of the base has been added, (c) after half of the HC2H3O2 has been neutralized, and (d) at the equivalence point.
Consider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d please
a) A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a solution of acetic acid. However, they forgot to document the mass of NaC2H3O2 added to the beaker. Fortunatelly, they know that the concentration of HC2H3O2 is 0.235M. Determine the mass, in grams, of NaC2H3O2 that must have been added to the solution. (Molar Mass of NaC2H3O2=82.0343 g/mol) b) 10 mL is accidentally spilled into the buffer solution from part a. Determing the new pH of the solution.