Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acidsalt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5.Values of K, for Some Common Weak BasesConjugateAcidNameFormulaK51.8 x 10-54.38 x 10-45.6 x 10-43.8 x 10-101.7 x 10-9AmmoniaNH3MethylamineEthylamineAnilinePyridineCH;NH2CH;NH2C,H;NH2C;H;NNH,*CH;NH3*CH;NH;*CH;NH;*C3H;NH* To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember thelesson on dilution: C1V1=C2V2)4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off answer to 2 decimal places)

Answer: Buffer solution is the type of solution that resists the change in its pH on adding small…

To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off answer to 2 decimal places)

To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off answer to 2 decimal places)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 7CR: 7. Describe a buffered solution. Give three examples of buffered solutions. For each of your...

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Sulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.
Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.
7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?