Interpretation:
From the given percent dissociation, the concentration of the weak acid is to be determined.
Concept introduction:
pH is the measure of the acidity of a solution and it depends on the concentration of hydronium ions and the temperature of the solution.
The formula to calculate the pH of the solution from the concentration of hydronium ions is:
The ionization of the weak acid takes place as:
Percent ionization is the percentage of acid that gets dissociated upon addition to water. It depends on the hydronium ion concentration.
Here,
Want to see the full answer?
Check out a sample textbook solutionChapter 16 Solutions
Chemistry
- Apple ciders have pH's of approximately 2.9 – 3.3. Are they acidic, basic, or neutral? Answerarrow_forwardA) Which of the following reactions show how HSeO3- acts as a Bronsted-Lowry acid? (Select all that apply.) a) HSeO3-(aq) + CN-(aq) → SeO32-(aq) + HCN(aq) b) HSeO3-(aq) + Li+(aq) → LiHSeO3(s) c) HSeO3-(aq) + H3O+(aq) → H2SeO3(aq) + H2O d) HSeO3-(aq) + H2SO4(aq) → H2SeO3(aq) + HSO4-(aq) e) HSeO3-(aq) + OH-(aq) → SeO32-(aq) + H2O B) Which of the following reactions show how HSeO3- acts as a Bronsted-Lowry base? (Select all that apply.) a) HSeO3-(aq) + CN-(aq) → SeO32-(aq) + HCN(aq) b) HSeO3-(aq) + Li+(aq) → LiHSeO3(s) c) HSeO3-(aq) + H3O+(aq) → H2SeO3(aq) + H2O d) HSeO3-(aq) + H2SO4(aq) → H2SeO3(aq) + HSO4-(aq) e) HSeO3-(aq) + OH-(aq) → SeO32-(aq) + H2Oarrow_forwardWhat is the pH of a 0.25 M solution of H3PO4? Ka = 7.2 x 10-³ (A) 0.25 (B) 7.2 x 10-3 (C) 0.0018 (D) 0.042 (E) 1.37arrow_forward
- Which of the following statements are true about weak acids? (select all that are correct) a) They have a pKa within the pH range that might be encountered in foods. b) At a pH at or near the pKa they are partially dissociated. c) At a pH more than 2 units below the pKa they are almost completely dissociated. d) They include commonly encountered food acids such as acetic, lactic, citric and galacturonic. e) They include mineral acids such as hydrochloric, sulfuric and nitric. There are more than 1 answerarrow_forwardCalculate the percent lonization of hydrogen peroxide (H₂O₂) in solutions of each of the following concentrations (K,-2.4-12.) (a) 0.267 M (b) 0.382 M (C) 0.622 Harrow_forwardEXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.arrow_forward
- Problem Solving Chemistry at Work Save Fern Hill Lake! Fern Hill Lake has a low pH, presumably the result of acid rain. The lake is about 3 kilometers long, 2.5 kilometers across, and has an average depth of 8 meters. Its pH is 4.1. Someone in your community proposes that calcium hydroxide be added to the lake to increase the pH to 6.5, a more favourable level. *About how many grams of calcium hydroxide should be added to the lake to accomplish this task? *What approximations must you make in your calculations? Hoe reasonable do you think your approximations are? *Is adding calcium hydroxide a long-term solution to the problem of acid rain?arrow_forwardKa of acetic acid is 1.77 x105? Problem: A buffer is prepared containing 1.00 molar acetic acid and 0.800 molar sodium acetate. What is its pH if the Problem: A buffer is prepared containing 1.00 molar acetic acid and 0.800 molar sodium acetate. What is its pH if the Ka of acetic acid is 1.77 x105? LESSON WRAP-UP(5 minutes) You will now mark (encircle) the session you have finished today in the tracker below. This is simply a visual to help yoL track how much work you have accomplished and how much work there is left to do. You are done with the session! Let's track your progress. PERIOD 1 PERIOD 2 PERIOD 3 1 2 3 4 7. 8. 9. 10 11 12 13 14 15 16 17 18 19 20 21 22arrow_forwardtion will be acidic. Simila Practice Exercise Predict whether the following solutions will be acidic, basic, or nearly neutral: (a) LiClO,, (b) Na,PO4, (c) Bi(NO3)3, (d) NH,CN. Finally we note that some anions can act either as an acid or as a base. For example, the bicarbonate ion (HCO;) can ionize or undergo hydrolvsis nn follarrow_forward
- A 0.50 M solution of an acid HA has pH = 2.24. What is thevalue of Ka for the acid? (a) 1.7 x 10-12 (b) 3.3 x 10-5(c) 6.6 x 10-5 (d) 5.8 x 10-3 (e) 1.2 x 10-2arrow_forwardA lone pair of electrons can be used to act as a/an: (Select ALL that apply) a) Hydrogen Bond Donor b) Hydrogen Bond Acceptor c) Acid d) Base 3arrow_forward10. What is the value of [OH-] in a 0.015 MCHCOOH solution? Ka= 1.8 x 10-5 (a) 1.9 x 10-11 M(b) 2.0 x 10-6 M(c) 1.0 x 10-9 M (d) 5.0 x 10-8 M(e) 5.0 x 10-7 Marrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co