A) Considering the dissociation reaction for sulfuric acid in water, what is the pH of a 1.00 x 10^-2 M solution of H2SO4? B) HSO4- will hydolize in water to produce additional H30+; its Ka = 1.2 x 10^-2. Recalculate the pH of the 1.00 x 10^-2 H2SO4 solution, this time also considering the additional H30+ produced from the reaction.
A) Considering the dissociation reaction for sulfuric acid in water, what is the pH of a...
9. Sulfuric acid (H2S04), a diprotic acid, is a strong acid in its first deprotonation (deprotonation- loss of H'). The first deprotonation is considered complete (complete ionization). It is, however considered a weak acid for its second deprotonation with a Ka value of 1.2 X 102, For a 0.0456 M H2S04(aq) solution determine: (16 pts total) a. The chemical reaction equations for the successive loss of protons. (4 pts b. The concentration of HSO4-1 and H (H30') after the first...
1- Calculating [H+] for Pure Water: In a certain acidic solution at 25 ∘C, [H+] is 100 times greater than [OH −]. What is the value for [OH −] for the solution? In a certain acidic solution at 25 , [] is 100 times greater than [ ]. What is the value for [ ] for the solution? 1.0×10−8 M 1.0×10−7 M 1.0×10−6 M 1.0×10−2 M 1.0×10−9 M 2. ± Acid-Base Relationships in Water: Water ionizes by the equation H2O(l)⇌H+(aq)+OH−(aq)The...
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Answer: 7. Sulfuric acid is produced through the reaction of sulfur trioxide with water. SO3(g) + H200 = H2SO4(aq) a. At standard state, the forward reaction is (10 pts) Spontaneous at all temperatures. ii. Not spontaneous at any temperature. iii. Spontaneous at temperatures greater than iv. Spontaneous at temperatures less than (calculate the value) (calculate the value). Book Pro b. 0.801 g sulfur trioxide is added to 1.00 L of water at 298 K. Calculate the equilibrium concentration...
Calculate the concentrations of H2SO4, HSO4−, SO42− and H3O+ ions in a 0.12 M sulfuric acid solution at 25°C (Ka2for sulfuric acid is 1.3 × 10−2.) a). H2SO4 b). HSO4- c). SO42- d). H3O+
a) Write the dissociation reaction and corresponding K, expression for CH3NHs in water 8. b) Write the reaction with water and corresponding Ko expression for aniline (CGHsNH2) 9 A typical sample of vinegar has pH of 3.0. Assuming the vinegar in only an aqueous solution of acetic acid (Ka 1.8 x 105), calculate the concentration of acetic acid in vinegar? 10. Calculate the pH of a solution that contains 1.0 M HF (K-7.2x10) and 1.0 M CHsOH (K-1.6x1010). Calculate the...
The acid dissociation constant Ka of trichloroacetic acid CCl3COOH, is 2.2x10^-1 calculate the ph of 1.00 M aqueous solution of trichloroacetic acid.
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...
Question 1 : HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.075 M. Question 2 : We place 0.143 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.28 . Calculate the ionization contant, Ka, of HA. Question 3 : We place 0.661 mol of a weak acid, HA,...
7. Sulfuric acid is produced through the reaction of sulfur trioxide with water. S03(g) + H20(1) = H2SO4(aq) a. At standard state, the forward reaction is (10 pts) i. ii. Spontaneous at all temperatures. Not spontaneous at any temperature. Spontaneous at temperatures greater than Spontaneous at temperatures less than iii. (calculate the value). (calculate the value) iv. b. 0.801 g sulfur trioxide is added to 1.00 L of water at 298 K. Calculate the equilibrium concentration of each substance in...
Exp5 - Determining the Dissociation of a Weak Acid using pH Measurement 16. (3 pts) A solution was made by adding 30.00 mL of 0.215 M NaOH solution to 25.00 mL of 0.445M HA solution. This mixture was diluted to 250.00 mL. The pH of this solution was 5.83. Calculate the dissociation constant, Ka. HA (aq) + H2O(l) = H30 (aq) + A (aq)