Answered: Given what we know about pH and…

Given what we know about pH and buffers, which will resist a change in pH the most: 1) water or 2) the buffered solution? Provide reasons to support your answer (3-4 sentences).

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

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.4: Acid-base Properties Of Salts

Problem 2RC

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One of the most challenging parts of solving acidbase problems is writing out the correct equation. When a strong acid or a strong base is added to solutions, they are great at what they do, and we always react them first. If a strong acid is added to a buffer, what reacts with the H+ from the strong acid and what are the products? If a strong base is added to a buffer, what reacts with the OH from the strong base and what are the products? Problems involving the reaction of a strong acid or strong base are assumed to be stoichiometry problems and not equilibrium problems. What is assumed when a strong acid or strong base reacts to make it a stoichiometry problem?
Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH3 CH;NH2 C¿H5NH2 C,H;NH2 C3H;N 1.8 × 10-5 4.38 × 10-4 5.6 × 10-4 3.8 × 10-10 Ammonia Methylamine Ethylamine Aniline Pyridine NH, CH;NH;* C¿H5NH3* C¢H;NH;* C;H;NH+ 1.7 x 10-9 314. Compute the concentration of the weak base in Molarity (round off answer to 4 decimal places).
In 3-10 sentences, explain by citing the chemical reactions involved in how buffers resist a drastic change in pH when an acid or base is added.
The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
Consider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answer
Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH,+ CH3NH3+ CH5NH3+ CH;NH3* C;H;NH+ 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 Ammonia NH3 CH;NH2 CH;NH2 CH;NH, C;H;N Methylamine Ethylamine Aniline Pyridine 1.7 x 10-9 3. Compute the concentration of the weak base in Molarity (Write your answer in 4 decimal places without the unit).
CH3CH2COOH Draw the Lewis structure of the acid and mark the acidic hydrogen with an asterisk (*). Draw a Lewis structure of the conjugate base of the acid. Suppose the acid is neutralized with a strong base. a) Which of the two structures you drew in 6 and 7 would be the predominant form of the species at a pH well above that at the equivalence point? b) Which of the two structures would be the predominant form of the species at a very low pH, well below that at the equivalence point and similar to the pH near the start of the titration? c) At what point in the titration, if any, would there be equal amounts of the two forms?
What are the factors that affect buffer capacity? Explain in 2-3 sentences.
Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 C,H;NH2 C;H;N NH,+ CH;NH3+ CH5NH3* CH;NH3* C;H;NH+ 1.8 × 10-5 4.38 × 10-4 5.6 x 10-4 3.8 × 10-10 Pyridine 1.7 x 10-9 2. Compute for pKb. (Write your answer in 2 decimal places).
A)6.85The best conjugate pair for this pH would be: If you were going to add NaOH solution as part of the buffer preparation, which component of the conjugate pair would you use in this case? B)10.80 The best conjugate pair for this pH would be: If you were going to add NaOH solution as part of the buffer preparation, which component of the conjugate pair would you use in this case?