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 acid salt 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 Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, CHÍNH * 4.38 x 10-4 C₂H5NH₂ C₂H5NH₂+ 5.6 x 10-4 Ethylamine Aniline Pyridine CHẠNH, C6H5NH3+ 3.8 x 10-10 CsHsN CH,NH* 1.7 x 10-⁹ 3. Compute the concentration of the weak base in Molarity. (round off answer to 3 decimal places)

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 acid salt 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 Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, CHÍNH * 4.38 x 10-4 C₂H5NH₂ C₂H5NH₂+ 5.6 x 10-4 Ethylamine Aniline Pyridine CHẠNH, C6H5NH3+ 3.8 x 10-10 CsHsN CH,NH* 1.7 x 10-⁹ 3. Compute the concentration of the weak base in Molarity. (round off answer to 3 decimal places)

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 a 5.55-102 M solution of H₂CHO calculate both the pH and the CH4O2 ion concentration. State symbols are not shown for water or the aqueous species in the reaction equations. HiệnHoDe+H2OHOHOH. Đó Ki-7,9×105 HC₂H₂O + H₂0H₂O + CH606² K₂21.6x10-12 pH = [CH₂O2)
Buffer Preparation: Acid-Base Reactions An aqueous solution contains 0.496 M hydrocyanic acid. Calculate the pH of the solution after the addition of 2.18x10 2 moles of sodium hydroxide to 125 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide) pH = Submit Answer Retry Entire Group 8 more group attempts remaining An aqueous solution contains 0.498 M ammonia. Calculate the pH of the solution after the addition of 3.30x102 moles of hydrobromic acid to 155 mL of this solution. (Assume that the volume does not change upon adding hydrobromic acid.) pH = Submit Answer Retry Entire Group 8 more group attempts remaining Use the References to a An aqueous solution contains 0.336 M ammonia. Calculate the pH of the solution after the addition of 2.95x102 moles of hydrochloric acid to 155 ml of this solution. (Assume that the volume does not change upon adding hydrochloric acid.) pH = Submit Answer Retry Entire Group 8 more group attempts remaining
A buffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate. What will the solution pH be if 0.126 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places) Type your answer...
Suppose you want to prepare a solution with a pH of 4.00 using acetic acid, CH3COOH, and sodium acetate, CH3CoOONa. What should the ratio of sodium acetate to acetic acid, CH3CO0-| : [CH3COOH], be in your buffer solution? Hint: The Ka for acetic acid is 1.8x105. 0.18:1 O 1.9:1 0.84:1 O 5.5:1 O 1:1
Fill in the blanks to show how you would solve for the pH of a 0.10 M aqueous solution of the weak acid HA. For the table and the equilibrium expression, do not ignore x. 0.10 POH Initial Concentration (M) Change 0.10 - X Equilibrium 2x² K₂ = 0.10 - 2x 4x² HA(aq) X (0.10 - x)² + 2x (0.10-2x)² H₂O(l) + +
Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > 5 A solution of phenol (HC H₂O) is prepared by dissolving 0.385 g of phenol in 2.00 L of H₂O. The solution has a pH = 6.29. Fill in the ICE table with the appropriate value for each involved species o determine the unknown concentrations of all reactants and products. H_O*(aq) + Initial (M) Change (M) Equilibrium (M) 1 HC,H,O(aq) + 5 H₂O(1) 2 C_H,O(aq)
5. Please solve the following chemistry problem.
Please answer all questions or leave for someone else to answer.
both parts please
A buffer solution is prepared by combining 0.795 moles of formic acid and 0.898 moles of sodium formate. What will the solution pH be if 0.120 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places)
pH calculation after the first equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5
pH calculation before the first equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 5.4 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka of oxalic acid = 5.60 x 10-2 and Ka of hydrogen oxalate anion = 5.42 x 10-5