a) The active ingredient in Aspirin™ is acetylsalicylic acid, HC9H7O4 (Ka = 2.75 x 10–5). To treat your headache after writing exams, you take two tablets dissolved in 250 mL of water. If each tablet contains 0.32 g acetylsalicylic acid, find the pH of the solution.
Proper pH significant digit is required for full marks.
b)Hydrazine, N2H4, is a base in aqueous solution. A 0.20 mol/L solution of hydrazine in water has pH = 10.77. What is Kbfor hydrazine?
Express your answer in the a.b x 10-c format. abc
c)The two acid ionization constants for oxalic acid, HOOCCOOH, are Ka1 = 5.6 x 10–2 and
Ka2 = 1.5 x 10–4. What is the base dissociation constant, Kb, for OOCCOO2–(aq)? Express your answer in the a.b x 10-cd format. abcd
d)Sodium azide, NaN3(s) has many uses. It is the chemical used to make automobile air bags inflate with N2(g), and it is sometimes added to water to kill bacteria. What is the pH of a 0.010 mol/L aqueous solution of NaN3(aq)? Only the azide ion, N3–(aq), affects the pH of water. For hydrazoic acid, HN3(aq), Ka = 1.9 x 10–5.
a) The active ingredient in Aspirin™ is acetylsalicylic acid, HC9H7O4 (Ka = 2.75 x 10–5). To...
The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), a monoprotic acid with Ka=3.3×10−4 at 25 ∘C What is the pHpH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 590 mg of acetylsalicylic acid each, in 260 mL of water?
Calculate the pH of a 0.0164 M aqueous solution of acetylsalicylic acid (aspirin) (HC9H7O4, Ka = 3.0×10-4). pH = Submit Answer
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
A 45.0 mL sample of 0.135 M acetylsalicylic acid (HC9H7O4, commonly known as aspirin) is titrated with 0.165 M NaOH. Determine each of the following and then use your answers to make a sketch of the titration curve. Ka of HC9H7O4 = 3.3 x 10-4 a. The volume of base required to reach the equivalence point. b. The initial pH. c. The pH when 25.0 mL of base has been added. d. The pH at the half-way point. e. The...
Acetic acid CH3COOH 1.8 × 10-5 Acetylsalicylic acid (aspirin) HC9H7O4 3.0 × 10-4 Equal volumes of 0.506 M aqueous solutions of acetic acid (CH3COOH(aq)) and sodium acetylsalicylate (NaC,H-04) are mixed. (1) Write the net ionic equation for the overall reaction that takes place as the system comes to equilibrium. Write acetic acid, benzoic acid or formic acid and their conjugates in the form RCOOH/RCOO. For example, benzoic acid should be written "CH3COOH" NOT "CzH;CO,H". It is not necessary to include...
QUESTION 23 The Ka of hydrazoic acid (HN3) is 1.9 x 10-5 at 25.0 °C. What is the pH of a 0.15 M aqueous solution of HN3? OOO 0.82 1.95 5.23 2.77 -3.46
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from water to form the hydroxide ion, OH −, and hydrazoic acid, HN3, according to the following equation. N3−(aq) + H2O(l) equilibrium reaction arrow OH −(aq) + HN3(aq) The base-dissociation constant (Kb) for this base is 4.04 ✕ 10−10. If a 0.082 M solution of azide ions is prepared, what is the final pH of the solution? (Assume that the temperature is 25°C.)
The Ka of hydrazoic acid (HN3) is 1.9 x 10-5 at 25°C. What is the pH of a 0.35 M solution of HN3? 2.59 5.23 2.41 O 1.14
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...
16) The molar concentration of hydronium ion in pure water at 25°C is 1.0 x 10 b) 0.00 c) 1.0 x 1014 d) 1.0 e) 7.00 17) A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts...