Answer) 2.0 is the pH of acetylsalicylic acid.
Explanation:
Acetylsalicylic acid is a weak acid. Write the dissociation reaction of acetylsalicylic acid as follows:
The equilibrium constant is written as:
pKa of acetylsalicylic acid is 3.5
pKa = - log Ka
Ka = 10-pKa
Ka = 10-3.5
Calculate the pH as follows:
pH = - log[H3O+] = - log(0.0105) = 1.97 ~ 2.0
1. What is the pH of a 0.35 mol/l solution of acetylsalicylic acid (C9H8O4)? 2 points...
What is the pH of a 0.35 mol/L solution of acetylsalicylic acid (C9H8O4) 1. What is the pH of a 0.35 mol/L solution of acetylsalicylic acid (C9H804)?
Maps 1. What is the pH of a 0.35 mol/L solution of acetylsalicylic acid (C9H804)? 2 points Your answer 2. What is the pH of a 1.50 mol/L solution of ammonium chloride (NH4Cl)? 2 points Your answer 4 points 3. What is the pH of the buffer resulting of the mixing of 34.4 g of sodium dihydrogen phosphate (NaH2PO4) and 48.5 g of sodium hydrogen phosphate (Na2HPO4) in 2.5 L of distilled water? Your answer 4. What is the pH...
1. What is the pH of a 0.35 mol/L solution of acetylsalicylic acid (C9H804)?
What is the pH of a 0.35 mol/L solution of facetylsalicylic acid 2
Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH. What was the Ka value calculated by the student if the pH of the solution was 2.62?
A typical aspirin tablet contains 324 mg of acetylsalicylic acid (C9H8O4), a monoprotic acid having a Ka = 3.0 x 10-4. If you dissolve two aspirin tablets in 300. mL of water, what is the pH of the solution acetylsalicylic acid? A typical aspirin tablet contains 324 mg of acetylsalicylic acid (C9H8O4), a monoprotic acid having a Ka = 3.0 x 10-4. If you dissolve two aspirin tablets in 300. mL of water, what is the percent dissociation of the...
What is the pH of a 5.00 times 10^-3 M solution of acetylsalicylic acid, pK_a = 3.52. (Enter your answer to 2 decimal places) pH =
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2 points after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your answer O BE
What is the pH of a 1 L solution containing 0.5 mol of propionic acid and 0.4 mol of sodium propionate? Ka for propionic acid = 1.3 x 10-5. Select one: O a. 4.8 O b. -1.3 C. 1.3 O d. -5.0 e. 5.0 O O O
Consider a weak acid "HA". What is the pH of a 0.853 mol L-1 solution of HA? The KA of HA is 6.32 x 10-6