A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium[H2C6H6O6] = 5.5 X 10-5 M, [HC6H5061] = 3.5 X 10-4 M, and Ką = 8.00 x 10-5 ?everything is based upon the acid dissolving in water:H2C6H6O6+ H20<-> HC6H601 + H3O*1Kasolve for [H30+1] then put in the numbersKa [[H3O+' :%3D[[H3O*'] =%3DpH = - loga. H30*1b. OH-1c. H2C6H6O6d. HC6H6061е. HSO31f. SO3?g. H2SO3h. HC2H3O2i. C2H3O21j. H2Sk. HS-1I. S2m. HXn. X-1О. 1р. 2q. 3r. 0.5000s. 5.5 X 10-5t. 3.5 X 10-4u. 8.00 x 10-5v. 1.75 x 10-6w. 1.11 x 10-8х. 5.5 х 10-2у. О.7000z. 1.60 x 10-5aа. 1.143 х 10-5bb. 0.4900сс. 1.104 х 10-5dd. 0.7100ее. 1.26 х 10-5 ff. 4.901gg. 7.93hh. 4.942ii. 4.957

Given,H2C6H6O6 = 5.5 × 10-5 MHC6H6O6-1 = 3.5 × 10-4 MKa = 8.00 × 10-5Required,…

A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H2C6H6O6] = 5.5 X 10-5 M, [HC6H6061] = 3.5 X 10-4 M, and Ka = 8.00 × 10-5 ? everything is based upon the acid dissolving in water: H2C6H6O6 + H2O <-> HCGH6061 + H3O*1 Ka = [ solve for [H30+1] then put in the numbers Ka [ [H3O*'] = [H3O*1] = pH = - log a. H30+1 b. ОН-1 c. H2C6H6O6 d. HCGH,061 е. HSO31 f. SO32 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. S2 m. HX n. X-1 р. 2 О. 1 q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10-5 aa. 1.143 x 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ee. 1.26 x 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957

A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H2C6H6O6] = 5.5 X 10-5 M, [HC6H6061] = 3.5 X 10-4 M, and Ka = 8.00 × 10-5 ? everything is based upon the acid dissolving in water: H2C6H6O6 + H2O <-> HCGH6061 + H3O1 Ka = [ solve for [H30+1] then put in the numbers Ka [ [H3O'] = [H3O*1] = pH = - log a. H30+1 b. ОН-1 c. H2C6H6O6 d. HCGH,061 е. HSO31 f. SO32 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. S2 m. HX n. X-1 р. 2 О. 1 q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10-5 aa. 1.143 x 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ee. 1.26 x 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 10Q

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Similar questions

For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. (a) Equal volumes of 0.10 M acetic acid, CH3CO2H, and 0.10 M KOH are mixed. (b) 25 mL of 0.015 M NH3 is mixed with 12 mL of 0.015 M HCl. (c) 150 mL of 0.20 M HNO3, is mixed with 75 mL of 0.40 M NaOH. (d) 25 mL of 0.45 M H2SO4 is mixed with 25 mL of 0.90 M NaOH.
The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of 5.82. a Calculate the value for the equilibrium constant for the reaction CH3NH3++H2OCH3NH2+H3O+ b What is the Kb value for methylamine? c What is the pH of a solution in which 0.450 mol of solid methylammonium chloride is added to 1.00 L of a 0.250 M solution of methylamine? Assume no volume change.
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Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
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What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
Sodium benzoate is a salt of benzoic acid, C6H5COOH. A 0.15 M solution of this salt has a pOH of 5.31 at room temperature. a Calculate the value for the equilibrium constant for the reaction C6H5COO+H2OC6H5COOH+OH b What is the Ka value for benzoic acid? c Benzoic acid has a low solubility in water. What is its molar solubility if a saturated solution has a pH of 2.83 at room temperature?
What are the pH and ion concentrations in a solution of 0.10 M sodium formate, NaCHO2? Kb for the formate ion, HCO2 is 5.6 1011. pH [Na+] [CHO2] [OH] (a) 5.63 0.10 0.10 2.4 10-6 (b) 837 0.10 0.10 2.4 10 6 (c) 822 0.050 0.050 17 10- (d) 5.63 0.10 0.10 42 10
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
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