Activity3. True or False! Directions: Write T if the statement is correct and F if otherwise. Write your answer before the number. 1. If the buffer is made with à base and its conjugate acid, the pH can be adjusted using a weak acid like HCI. 2. A buffer's pH changes greatly when a small amount of strong acid or base is added to it. 3. A good buffer mixture should have about equal concentrations of both of its components. 4. The strength of a weak acid (buffer) is usually represented as an equilibrium constant. 5.The Henderson-Hasselbalch equation connects the measurable value of the pH of a solution with the theoretical value pKa.

Activity3. True or False! Directions: Write T if the statement is correct and F if otherwise. Write your answer before the number. 1. If the buffer is made with à base and its conjugate acid, the pH can be adjusted using a weak acid like HCI. 2. A buffer's pH changes greatly when a small amount of strong acid or base is added to it. 3. A good buffer mixture should have about equal concentrations of both of its components. 4. The strength of a weak acid (buffer) is usually represented as an equilibrium constant. 5.The Henderson-Hasselbalch equation connects the measurable value of the pH of a solution with the theoretical value pKa.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 103AP

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A professor prepares a buffer solution that they need for the purification of protein from human cell lysates. They did mix weak acid and conjugate base and obtained the initial solution, which is characterised by these parameters. Final volume: 200mltotal buffer compound concentration: 150mMIntitial concentration weak acid: 0.03MInitial concentration conjugate base: 0.12MInitial pH 6.9buffer compound pka 6.3
A buffer system works to keep pH within a narrow range. Buffer systemsare critical in all living cells/tissues. If pH were to measurably shift in a cell,what category of biological molecules would be most impacted, andwhat term refers to the resulting loss of their functional shapes? A buffer is a substance that, when it ionizes in water, creates a buffersystem. The substance and one of its ions represent a weak acid and aweak base. These form a pH-controlled equilibrium. Based on thedefinitions of acid and base, if [H+] increases, which would combine withthe H+, preventing a pH shift? If [H+] decreases, whichwould release H+ to counter a pH change? Check the one characteristic below that is important in a buffer system. maintains a neutral pH prevents pH from dropping prevents pH from rising minimizes change in p
In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
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You are to prepare 100. mL of an acetate buffer of pH 5.00 using 1.0 M acetic acid (CH3CO2H, also written as HC2H3O2) and solid sodium acetate (NaC2H3O2). To prepare for the investigation, complete the following calculations. The pKa for HC2H3O2 is 4.74. The Henderson-Hasselbach equation is pH = pKa + log ([conjugate base]/[acid]) (a) What ratio of [NaC2H3O2] to [CH3CO2H] is required for a pH = 5.00? (b) You will want the concentrations relatively dilute, so use an acid concentration of 0.10 M. What volume of 1.0 M CH3CO2H would be needed to prepare 100. mL of buffer with the desired concentration of 0.10 M? Use M1V1 = M2V2 (c) Use the ratio from (a) and the concentration desired (discussed in (b)) to calculate how many grams of NaC2H3O2 · 3 H2O would be needed to prepare 100. mL of buffer if the acid concentration is 0.10 M?
Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.