In the reaction COOH + H₂O ⇒ H3O+ + CH³COO- base constant K₂ of acetic acid CH3COOH is approximately 10-5 at 25 °C. Wh e pk of the acetate ion, CH3COO™? (A) 10-⁹ (B) 9 (C) -5 (D) 5 (E) 10-5
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- In the reaction CH3 COOH+H₂O=H3O++CH3COO- the base constant K of the acetate ion CH3COO is approximately 10-⁹ at 25 °C. What is the pK, of acetic acid, CH3COOH? (A) 10-⁹ (B) 9 (C) -5 (D) 5 (E) 10-56. For the ionization of phenylacetic acid, C6H5CH₂CO₂H + H₂O = H3O+ + C6H5CH₂CO₂ K₂ = 49 × 10-5 (a) What is [C6H5CH₂CO₂] in 0.186 M C6H3CH₂CO₂H? (b) What is the pH of 0.121 M C6H3CH₂CO₂H?What is the correct equilibrium constant expression for the following reaction? NH3(aq) + H₂O(1) ⇒NH4*(aq) + OH¯(aq) O O (A) Ke (B) Kc (c) Ke (D) Kc (E) Kc - = = = [NH3] [H₂O] [NH4]+[OH]- [NH4+][OH-] [NH3] [NH4+] [OH [NH3] [H₂O] [NH3] [NH₂+] [OH-] 4 [NH₁+OH [NH3]
- In the reaction CH3 COOH+H₂O=H3O++CH3 COO- the base constant K₁ of the acetate ion CH3COO is approximately 10-⁹ at 25 °C. What is the pk of acetic acid, CH3COOH? a (A) 10-⁹ (B) 9 (C) -5 (D) 5 (E) 10-5PQ-14. Given the equilibrium constants for these reactions: (8) H+ (3)'H³Ɔ (3)'H Ke% D2.8×10-21 Ke =9.5×10 13 CH, (g)+ H,O(g) =CH,OH(g)+ H, (g) What is the value of K. for this reaction? 2CH,OH(g) + H,(g)=C,H,(g)+ 2H,0(g) (B) 2.9x10-9 (C) 3.4x10% (D) 1.2x1029 (A) 9.5x10-13COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
- The K, for acetic acid (CH,COOH) is 1.737 × 10-5. What is the pK, for this acid? pKa = Use the calculated pK, to determine the pH at which [CH,COOH] = [CH,COO¯]. %3D pH =(2) When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s)< 2NH4* + SO4²- NH4* + NH3(aq) + H* SO42- + H2O → HSO4 + OH- Ksp = 276 Ka = 5.70 ×10-10 Кь 3 9.80 х 10-13 (a) (b) (c) (Show your Calculation) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.What is the molar ratio of CH3COOH to CH3COONA that should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00? Ka (CH;COOH) = 1.8 x 10-5
- (a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.lodic acid, HIO3, has a pk of 0.77. What is the formula of its conjugate base? Correct. Kb= II H₂1O4 HIO3 OH 103™ H₂lO3+ What is the value of K, for the conjugate base? Incorrect. Did you calculate the pk, first? i||(c) Calculate the pH of 0.5 mol/L sodium hydrogen carbonate, NaHCO3. The Ka,1 of carbonic acid, H₂CO3, is 4.3 x 10-7. Нансез END