Question

You have 2 buffers A and B which have a pH of 7.4. Addition of 5...

You have 2 buffers A and B which have a pH of 7.4. Addition of 5 drops of 0.1N HCl changes the pH of buffer A to 6.8, whereas addition of 5 drops of 0.1 N HCl to buffer B changes its pH to 7.2.

Which is the better buffer and why?                                                                           

Homework Answers

Answer #1

The aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa is called a Buffer. Buffer solutions are used as a means of keeping pH at a nearly constant value in a wide variety of chemical applications. When a small or moderate amount of strong acid or base is added to it, its pH changes very little and thus it is used to prevent changes in the pH of a solution.

A buffer is able to resist pH change because the two components (conjugate acid and conjugate base) are both present in appreciable amounts at equilibrium and are able to neutralize small amounts of other acids and bases when the are added to the solution. Many life forms thrive only in a relatively small pH range so they utilize a buffer solution to maintain a constant pH.

Hence, Buffer B is the better buffer.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base...
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the addedH+, forming more...
You have constructed a quinhydrone concentration cell with buffers of pH = 4.2 and pH =...
You have constructed a quinhydrone concentration cell with buffers of pH = 4.2 and pH = 2.5 according to the following notation: C(s, graphite) | pH 4.7 buffer, quinhydrone || pH 2.7 buffer, quinhydrone | C(s, graphite) Using the Nernst equation as derived in the Chemical Foundations section for the quinhydrone concentration cell, calculate the cell potential for this electrochemical cell.
For an experiment, you need two buffers, one with pH = 3.1 and one with pH...
For an experiment, you need two buffers, one with pH = 3.1 and one with pH = 9.7. You have the following reagents available. Which pair would you use for each buffer and what must the buffer ratio be in each case? 1) Hydrobromic acid (HBr) 2) Sodium bromide (NaBr) 3) Hydrofluoric acid (HF) 4) Sodium fluoride (NaF) 5) Pyridine (C5H5N) 6) Pyridinium chloride (C5H5NH+Cl-) 7) Triethylamine ((CH3CH2)3N) 8) Triethylammonium chloride ((CH3CH2)3NH+Cl-) 9) Sodium hydroxide (NaOH)
You have access to phosphoric acid (pKa1,2 = 2.1, 7.2), formic acid, acetic acid, and their...
You have access to phosphoric acid (pKa1,2 = 2.1, 7.2), formic acid, acetic acid, and their conjugate bases. You are asked to make 2 different buffers with pH 3.5 and 7.4. What acids and conjugate bases do you choose? If both buffers have 0.1 M total concentration ([acid] + [conjugate base]), calculate acid and conjugate base concentrations needed to make the buffers.
NH3/NH4 buffer: Mass NH4Cl used 1.3738g volume NaOH used 21.2 ml initial pH (0f the buffer)...
NH3/NH4 buffer: Mass NH4Cl used 1.3738g volume NaOH used 21.2 ml initial pH (0f the buffer) 9.6, pH after 1 drop HCl 9.03, pH after 10 drops HCl 8.91 Dilute NaOH solution Initial pH 10.35 pH :1 drop HCl 10.21, 10 drops HCl 2.85 Acetate buffer (0.500) Mass of CH3COONa * 3H2O 10.935 volume CH#COOH 44.3 ml initial pH 4.89 1.0 ml of NaOH pH 4.93 initial volume 2.2 final volume 16.2 final pH 5.91 Acetate buffer (0.100) Mass of...
a. Describe the preparation of 2 liters of 0.1 M Glutamate buffer, pH 10.0. You have...
a. Describe the preparation of 2 liters of 0.1 M Glutamate buffer, pH 10.0. You have available monosodium glutamate (MW=169), 0.5M NaOH and distilled water. b. Momentarily distracted by having a piece of old light fixture fall on your head, you add 10ml of the 0.5 HCL to the 2L of buffer. What would be the pH now?
2) Buffers are extremely important in biology as they allow you to prepare solutions with a...
2) Buffers are extremely important in biology as they allow you to prepare solutions with a specific pH that can match physiological conditions. To prepare a buffer, we frequently take a weak acid and react it with a strong base. 2a) In this reaction, we combine 1 ml of 0.1 M NaOH with 10 ml 1M CH3CO2H (acetic acid). Write the reaction that proceeds (it goes to completion) and determine the amount of each component. 2b) Using the Henderson-Hasslebach equation...
pH buffer preparation: You have a 1L volumetric flask, 10. M HCl, solid NaOH, nanopure water,...
pH buffer preparation: You have a 1L volumetric flask, 10. M HCl, solid NaOH, nanopure water, and a container of the weak base sodium bisulfide (NaSH, pKb = 7.0, – where in water this “salt” dissociates into Na+ and SH- ions).   a. (6 points) Describe your process for producing a pH buffer with 0.1M of both the weak acid and its conjugate base. Make sure to include the exact mass or volume of every single substance you utilize to create...
How would you prepare a 500mL of 100mM phosphate buffer at pH 7.2 if you have...
How would you prepare a 500mL of 100mM phosphate buffer at pH 7.2 if you have only solid Na3PO4 and 1M HCL and 1M NaOH (may not use all reagents). Find mass of Na2HPO4, Volume 1M HCL, and Volume 1M NaOH
Assume your blood has a pH of 7.4 and you have been producing urine with a...
Assume your blood has a pH of 7.4 and you have been producing urine with a pH of 7.4 for a while. You drive to very high altitude (ca. 4,000 m) and spend several hours there. Your alveolar ventilation rate increases (as expected), and eventually this causes your blood pH to rise above 7.4 (your blood plasma becomes more basic than normal). This change in blood pH will initiate compensatory homeostatic mechanisms in your kidneys ("renal compensation") that will alter...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT