Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with KOH in water. If 40.00 mL of the %3D KOH solution is required to reach the equivalence point, what will the pH of the solution be after only 20.00 mL of the KOH solution has been added? 1.80 2.91 3.74 4.56

Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with KOH in water. If 40.00 mL of the %3D KOH solution is required to reach the equivalence point, what will the pH of the solution be after only 20.00 mL of the KOH solution has been added? 1.80 2.91 3.74 4.56

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

An analytical chemist is titrating 57.7mL of a 0.2900M solution of formic acid H2CO2 with a 0.9700M solution of KOH . The pKa of formic acid is 3.74 . Calculate the pH of the acid solution after the chemist has added 7.03mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
Consider the titration of 100.0 mL of 0.100 M acetic acid (Ka = 1.8 x 105). When 50.00 mL of 0.100 M NaOH is added to the acetic acid solution, calculate the pH of the resulting mixture. Use the simultaneous equations method, showing the derivation of the final equation you used to calculate pH and justify any assumptions made in your derivation.
A solution of a weak acid is titrated with a standard solution of a strong base. The progress of the titration is followed with a pH meter. Which of the following observations best describes what would occur? Initially the pH of the solution increases slowly, and then it increases much more rapidly, before increasing slowly again At the equivalence point, the pH is 7 The pH of the solution gradually decreases throughout the experiment After the equivalence point, the pH becomes constant because this is the buffer
A 200mL solution of 0.3 M weak acid is titrated with 40 mL of 1.5 M NaOH. If the Ka of the acid is 5.37 x 10-10, what is the pH at this point in the titration?
The following is a titration curve for a monoprotic weak acid. 0.200 grams of the acid was dissolved in 50.00 mls of water and titrated with a 0.150 M solution of NaOH. 14.00 13.00 12.00 11.00 10.00 9.00 8.00 pH 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 Vol. Base (mL) What is the pKa of the acid? How many moles of acid were present? What is the molecular weight of the acid? What pH range should the indicator change color to determine the endpoint of titration? Over what pH range is [HA]> [A]? 00 08 25.00 00'0 00 0 00 9 00 0
You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?
In a lab, you titrate 27.0 mL of 0.100 M acetic acid (CH3COOH, a weak acid, pKa 5.756, Ka 2.75 x 10-5), with 0.100 M NaOH. At the equivalence point, the concentration of the primary species in solution is approximately What is the pH of the solution at the equivalence point? At the equivalence point, what percentage of the analyte has been titrated?
30 mL of 0.1 M HCI is titrated with 0.1 M CH3NH₂ (Ka = 2.0 x 10-¹1) solution. Calculate the pH after adding 15 mL of CH3NH₂ to initial acid 12.01 5.81 1.48 3.49 9.57
Consider the titration of a 60.0 mL of 0.321 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH. 1. What is the pH before any base has been added? 2. After 30.0 mL of KOH have been added, identify the primary species left in the solution. 3. After 30.0 mL of KOH have been added, what would the pH of the solution be? 4. After 75.0 mL of KOH have been added, identify the primary species left in the solution. 5. After 75.0 mL of KOH have been added, what would the pH of the solution be?
a) Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic acid to prepare a buffer with a pH = 3.50. Assume there is no change in volume upon addition of the sodium formate. b) Write the predominant chemical reaction that occurs when 0.050 mol of HClO4 is added to 1.00 L of the buffer prepared in part a and calculate the pH of the solution.
10.0 mL of 0.400 M NaOH is added to 20.0 mL of 0.50 M CH3COOH. Calculate the pH of the resulting solution. Ka(CH3COOH) = 1.8 × 10-5
1.Determine the pH during the titration of 62.9 mL of 0.360 M hydrocyanic acid (Ka = 4.0×10-10) by 0.360 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 94.4 mL of KOH 2. When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?