mass of aspirin = 327 mg = 0.327 g
molar mass of aspirin = 180 g / mol
moles of aspirin = 0.327 / 180
= 1.82 x 10^-3
volume = 237 mL = 0.237 L
molarity = 1.82 x 10^-3 / 0.237 = 7.67 x 10^-3
= 0.00767 M
HA ----------------------> H+ + A-
0.00767 0 0
-x + x +x
0.00767-x x x
Ka = x^2 / 0.00767 -x = 3.3 x 10^-4
x^2 + 3.3 x 10^-4 x - 2.53 x 10^-6
x = [H+] = 1.43 x 10^-3 M
pH = -log[ H+ ]
pH = 2.84
327 mg acety c acid (HC H-04). Calculate the pH of a A typical aspirin tablet...
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...
please explain, no clue whats going on. ' LLT UT Aspirin (C,H,04; M = 180.2 g/mol; pk, = 3.5) and Ibuprofen (C13H1809; M = 206.3 g/mol; pK, = 4.9) are over-the-counter acidic drugs used for relieving pain and reducing fever. Consider a 300 mg tablet of Aspirin and a 600 mg tablet of Ibuprofen. Relative pH Homework – Unanswered Which of these tablets will generate a more acidic solution when dissolved in 250 ml of water
The pH of an aqueous solution of 0.450 M acetylsalicylic acid (aspirin), HC,H,O4, is
b) In this experiment an aspirin tablet mark with deionized water. Using a pipette into a 100-mL volumetric flask and diluted to t make a 'diluted aspirin solution'. an aspirin tablet was placed in a 250-ml volumetric flask o dissolved in 10 mL of 1.0M NaOH solution, the flask was then 1.0M NaOH solution, the flask was then filled to the nized water. Using a pipette, 5.0 mL of this solution was added mL volumetric flask and diluted to the...
3a) The solubility of Aspirin (acetylsalicylic acid) at 25C is 3.0 mg/mL of water. Calculate the molar concentration (M) of acetylsalicylic acid in solution at this temperature. What density assumption can help you in solving this problem? b) The acid dissociation constant, Ka for acetylsalicylic acid is 3.0 x 10 -4. calculate the pH of this solution.
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Calculate the pH of a solution that is prepared by dissolving 0.500 mol of hydrocyanic acid (HCN, KA = 6.17x10-19) and 0.187 mol of acetylsalicylic acid (HC,H,04, K4 = 3.40x104) in water and diluting to 3.40 L. Also, calculate the equilibrium concentrations of HCN, CN, HC,H,O4, and C,H,O4. Do not make an approximation unless the initial acid concentration is greater than 1000 × K. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCN]=...
What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 420 mg of acetylsalicylic acid each, in 310 mL of water? Express your answer to two decimal places. The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), a monoprotic acid with a Ka of 3.3×10−4 at 25 ∘C.
A chemist dissolves 132. mg of pure perchloric acid in enough water to make up 380. mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits. XS ? A chemist dissolves 136. me of pure barium hydroxide in enough water to make up 160 ml of solution Calculate the pH of the solution. The temperature of the solution is 25 °C) Be sure your answer has the correct number of...
The active ingredient in aspirin is acetylsalicylic acid (HC9H704), a monoprotic acid with a Ka of 3.3 x 10-4 at 25°C. Part A You may want to reference (Pages 680 - 690) Section 16.6 while completing this problem. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 410 mg of acetylsalicylic acid each, in 270 mL of water? Express your answer to two decimal places. V AED o 2 ? pH = pH= Submit