Buffer Question 3: You have a 1.00L acetic acid buffer solution of pH 4.2. If the concentration of potassium acetate is 0.50 mol/L potassium acetate, what is the concentration 1.8 × 10-5) of the acetic acid? (Ka =

Buffer Question 3: You have a 1.00L acetic acid buffer solution of pH 4.2. If the concentration of potassium acetate is 0.50 mol/L potassium acetate, what is the concentration 1.8 × 10-5) of the acetic acid? (Ka =

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 15PS: A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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you have found the pKa to be 10.3. “Acid-free” paper should have a pH between 8.7 and 10.2. What is the pH of the buffer in your paper pulp if you add 0.581 mM calcium carbonate to pulp that started with 0.452 mM acid (pH=3.37)?
40. If you add 8.0 mL of 0.10 M HCl to 25 mL lactic acid/lactate buffer that is 0.10 M lactic acid and 0.12 M sodium lactate, what is the pH? (Ka=1.4x10-4) a. 3.5 b. 3.9 c. 3.7 d. 4.1
Please use 3 significant figures or 3 decimal places. What is the pH of a buffer is prepared, 1.00 M acetic acid and 1.00 M sodium acetate. (Acetic acid's Ka: 77 x 10-5) What is the pH of a buffer, prepared with 0.800 molar acetic acid and 1.00 molar sodium?
A theoretical weak acid has a Ka of 2.62x10-5. Find the pH of this acid when its concentration is 0.45 M. Prepare a pH 4.9, 2.5 L, 0.65 M acetate buffer. Starting materials: 1 M HOAc, 1.5 M NaOH. Find the amount of starting material needed. Prepare a pH 6.5, 1.0 L, 0.25 M phosphate buffer using 1.5 M H3PO4 and solid NaOH pellets.
5.) 1.0 L of acetate buffer is made by combining 0.50 M CH3COOH with 0.50 M CH3COONa. The Ka of CH3COOH is 1.8 X 10 ^-5. (Assume any additions cause a negligible change in volume). a. Calculate the pH of the buffer solution. b. Calculate the pH of the buffer solution after 0.010 mol of solid NaOH is added. c. Calculate the pH of the buffer solution if, instead, 0.010 mol of HCL is added.
The next 9 questions are related to the titration of 40.00 mL of a 0.0900 M acetic acid solution with 0.0900 M KOH. What is the volume of the solution at the equivalence point (in mL)? What is the molar concentration of the salt at the equivalence point? (ANALYTICAL CONCENTRATION, NOT EQUILIBRIUM CONCENTRATION) What is the pOH at the equivalence point?
4. What is the pH of a buffer made from 0.42 M H3BO3 and 0.22 M H2BO3-, if the Ka for H3BO3 is 7.3 x 10-10 ? (use 2 decimal places for pH)
When a strong base is added to a buffer it will react to become neutralized. Determine the pH after0.15 mol of OHis added to a buffer consisting of 2.0 mol of HA and 1.0 mol of A-. (Ka = 5.8 x 10-10)HA + OH- → A- + H2O
Question 4 A buffer solution includes a weak acid and its conjugate base. Include states of matter. Write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing NH3 and NH4Cl. Write the equation so that its equilibrium constant is equivalent to Ka.
Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25 from 0.10 M HFor solution and a 0.10 M NaFor solution. How many mL of the NaFor solution should you add to 20 mL of the 0.10 M HFor solution to make your buffer?
A student wants to make a pH 4.0 buffer solution. She decides to use a buffer made from formic acid and sodium formate (HCOONa). She adds 50.0 grams of sodium formate to a 1 L volumetric flask. The Ka of formic acid is 1.77×10-4. How many mL of 3.0 M formic acid should she add to the 1 L volumetric flask so that when the flask is diluted to the mark the pH will be 4.00?
A buffer is made with sodium acetate (CH3COONa)and acetic acid (CH3COOH); the Ka for acetic acid is 1.80 * 10-5. The pH of the buffer is 3.98. What is the ratio of the equilibrium concentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informa-tion is given to answer this question.