For an aqueous solution formed by mixing 4.50mL of 0.15M LİOH with 25.0mL of 0.100M C2H5CO2H (propanoic acid), a) determine whether this forms a buffer solution. b) determine the pH of this combined solution. c) state whether the addition of 6.75mL of 0.100M HCI to the solution will have a large or small effect on the pH of the solution. Explain your reasoning (using 1-2 sentences).

For an aqueous solution formed by mixing 4.50mL of 0.15M LİOH with 25.0mL of 0.100M C2H5CO2H (propanoic acid), a) determine whether this forms a buffer solution. b) determine the pH of this combined solution. c) state whether the addition of 6.75mL of 0.100M HCI to the solution will have a large or small effect on the pH of the solution. Explain your reasoning (using 1-2 sentences).

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

For each of the salts (assume at this point completely soluble), write the equation for dissociation and label the ions as acidic, basic or neutral.Each salt listed will 100% dissociate NH4C2H3O2 Al2(CO3)3 Na2HPO4 NaI For each of the following salts, determine the pH of a 2.50M solution of the salt.You will need the Ka and Kb tables to complete this problem. NaBrO CH3NH3Cl NaClO2 C6H5OK CsNO3 C6H5NH3Br
Which of the following incorrectly describes buffer solutions? Buffers can be prepared using strong acids and its conjugate base. Buffers are solutions that resist drastic changes in pH with the addition of a strong acid or base. Buffers are composed of a weak acid and its conjugate base. Buffers are solutions important in maintaining homeostasis in organisms.
You add 18.00 mL of 0.800 M NaOH to 50.00 mL of pure water, and to this mixture you then add 2.00 mL of 0.300 M HCl. What will be the pH of the resulting solution?
You make 0.1 L of a buffered solution (pH=9.1) by mixing acetic acid and sodium acetate. You have 1.00 M solutions of each component of the buffered solution. What volume of each solution do you mix to make such a buffered solution? Note that the total ion concentration must be 0.170M.
When 25.0 mL of 0.200 M hydroiodic acid and 25.0 mL of 0.200 M ammonia are combined, the pH of the resulting solution will be : ..... fill in the blank 1A. Less than 7B. Equal to 7C. Greater than 7
I mix 100 mL of 0.100 M HCl in 250 mL of 0.150 M NH3. I add 50.0 mL of 0.0500 M NaOH. What is the pH of the resulting mixture?
A chemist titrates 200.0 mL of a 0.7110M dimethylamine ((CH, NH) solution with 0.3310M HNO, solution at 25 °C. Calculate the pH at equivalence. The '2 pk, of dimethylamine is 3.27. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO, solution added. alo pH %3D Ar
An analytical chemist is titrating 119.2 mL of a 0.1800M solution of ammonia (NH,) with a 0.4500M solution of HNO2. The p Kb of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 53.9 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. 3 Round your answer to 2 decimal places. pH ?
An analytical chemist is titrating 204.9 ml of a 0.2200M solution of cyanic acid (HCNO) with a 0.7300.M solution of KOH. The pK, of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 50.06 ml, 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. DH-0
1) You are given a solution wherein [OH^-] is 1/4th of the concentration of [H^+]. What is the pH of this solution? 2)What is the change in pH when a few drops of strong base containing 3.0 x 10^-3moles of [OH^-] is added to a liter of either of the following two buffered solutions at pH6.4 (you can assume the volume remains approximately constant) i) a 250 mM solution of buffer A (pKa = 5.0) ii) a 250 mM solution of buffer B (pKa = 7.2) 3. Which solution is the more effective buffer at pH 6.40(provide a rationale for your answer)?
Calculate the pH of a mixture that contains 0.15 M of HCl and 0.27 M of HC6H5O.
A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa? Ka=1.80x10-4. The total volume is 1.00L. What is the pH of this solution?