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Acid and Base Worksheet 4 Answer document sample
NAME__________________________________ PERIOD _______ Page 1 of 18 UNIT 12 HW – ACID AND BASE CHEMISTRY ALL WORK MUST BE SHOWN FOR CREDIT NOTE: Ka & Kb TABLES AT END! Worksheet 12-1: Acid Base: Conjugate Pairs and Naming/Writing formulas (2 PGS) (REQUIRES INITIALS FOR STAMP! TEACHER INITIALS: Give the conjugate acid of the following bases: BASE CONJUGATE ACID BASE CONJUGATE ACID H2O ClO─ acetate H2PO4 ─ NH3 HSO4─ hydroxide A─ CO32- Methylamine (CH3NH2) Give the acid of the following conjugate bases: ACID CONJUGATE BASE ACID CONJUGATE BASE Water OH─ ammonia bromide ion SO42- O32- HCO3- CH3NH2 cyanide ion C2H3O2- Give the base of the following conjugate acids: BASE CONJUGATE ACID BASE CONJUGATE ACID HCN hydronium HCO3─ CH3NH3+ ammonium H2O HF HSO3─ HC2H3O2 HA NAME__________________________________ PERIOD _______ Page 2 of 18 Give the conjugate base of the following acids: ACID CONJUGATE BASE ACID CONJUGATE BASE HC2H3O2 H2SO4 HA oxalic acid hydrochloric acid H3PO4 NH4+ H2CO3 HCN hydrosulfuric acid Identify the acid (A), base (B), conjugate acid (CA), and conjugate base (CB) in the following: (a) NH3 (g) + H3O+ (aq) NH4+ (aq) + H2O (l) (b) CH3COOH (l) + NH2- CH3COO- (aq) + NH3 (g) (c) NH2 -(g) + H2O (l) NH3 (g) + OH-(aq) (d) HClO4 (aq) + H2O (l) H3O+ (aq) + ClO4- (aq) Name the following acids (they may not all exist, but use your rules to propose a name) Formula Anion Name Acid Name Formula Anion Name Acid Name H2Te H 2S H2SO2 HNO2 HBrO3 HIO H2CrO5 H3PO3 HCl HF H3PO2 H2CrO4 HIO2 H2SO3 HClO3 H2Se H2SO4 HI HBr HNO HNO4 HClO HBrO2 H2CrO2 NAME__________________________________ PERIOD _______ Page 3 of 18 Worksheet 12-1 Con’t Name Formula Name Formula Hyponitrous acid Perchromic acid Hydrobromic acid Nitrous acid Chloric acid Permanganic acid Chromous acid Hydrochloric acid Hydrotelluric acid Hyposulfurous acid Hypoiodous acid Iodic acid Bromic acid Bromous acid Phosphorous acid Perchloric acid Hypochromous acid Hydroselenic acid Hydrosulfuric acid Hypochlorous acid NAME__________________________________ PERIOD _______ Page 4 of 18 WKS 12-2 Calculations pH (1 page) Show all work and circle your answers! 1. (a) If the hydrogen ion concentration of a solution is 1.30 x 10-4 M, what is the pH of the solution? (pH = 3.89) (b) What is the pOH of this same solution? (pOH = 10.11) (c) What is the hydroxide concentration of the solution? [7.69 x 10-11] 2. (a) If the hydroxide ion concentration of a solution is 2.8 x 10-6 M, is it an acidic or a basic solution? (pH = 8.45, basic) (b) What is the pH of this solution? (pH = 8.45) (c) What is the hydrogen ion concentration of this solution? [3.61 x 10-9] (d) What is the pOH of this solution? (pOH = 5.65) 3. (a) If the pH of a solution is 4.67, what is the hydroxide ion concentration? [4.68 x 10-10] (b) What is the pOH of this solution? (pOH = 9.33) (c) What is the hydrogen ion concentration? [2.14 x 10-5 M] (d) Is this an acidic or basic solution? (acidic) 4. (a) If the pOH of a solution is 3.6, what is the pH? (pH = 10.40) (b) What is the hydrogen ion concentration of this solution? [3.98 x 10-11] (c) What is the hydroxide ion concentration of this solution? [2.51 x 10-4] (d) Does this solution have a higher hydrogen ion or hydroxide ion concentration? (hydroxide) 5. (a) If the pH of a solution is 12.5, what is the hydroxide ion concentration? (3.16 x 10-2) (b) What is the hydrogen ion concentration? (3.16 x 10-13 M) (c) What is the pOH of this solution? (pOH = 1.50) (d) What is the pH of this solution? (pH = 12.50) 6. Which would have a higher pH—a solution whose pOH is 5.42 or a solution whose hydrogen ion concentration is 9.44 x 10-8 M? (pOH = 5.42) 7. Which would have a more basic pH—a solution whose hydrogen ion concentration is 3.4 x 10-8 M or a solution whose hydroxide ion concentration is 2.6 x 10-5 M? (2.6 x 10-5 M) NAME__________________________________ PERIOD _______ Page 5 of 18 WKS 12-3 pH OF STRONG ACIDS AND BASES (two pages) SHOW ALL WORK AND CIRCLE FINAL ANSWER Part A: Given molarity 1. What is the pH of 0.80 M hydrobromic acid? (pH = 0.097) 2. If the pH of a strong acid solution is known to be 3.25, what is the molar concentration of the acid solution assuming the acid is diprotic? (2.8 x 10-4 M) 3. (a) If the pH of a barium hydroxide solution is known to be 12.50, what is the hydroxide ion concentration? (3.16 x 10-2 M) (b) What is the barium ion concentration? (1.58 x 10-2 M) (c) What is the molar concentration of the base solution? (1.58 x 10-2 M) 4. (a) What is the hydroxide ion concentration 0.166 M barium hydroxide solution? (0.33 M) (b) What is the hydrogen ion concentration of the solution? (3.03 x 10-14) (c) What is the pH of the solution? (pH = 13.52) (d) What is the Ba+2 ion concentration in this solution? (0.166 M) 5. If the pH of a cesium hydroxide solution is known to be 9.75, what is the molar concentration of the base solution?(5.62 x 10-5 M) 6. (a) If the pH of a hydroiodic acid solution is known to be 3.21, what is the hydroxide ion concentration? (1.62 x 10-11 M) (b) What is the molar concentration of the acid solution? (6.17 x 10-4) 7. (a) What is the molar concentration of the hydroxide ion for a 0.45 M calcium hydroxide solution? [0.90 M] (b) What is the pOH of this solution? (pOH = 0.05) (c) What is the pH of a 0.45 M calcium hydroxide solution? (pH = 13.95) (d) What is the hydrogen ion concentration of this solution? (1.12 x 10-14 M) (e) What is the molar concentration of the calcium ion? [0.45 M] NAME__________________________________ PERIOD _______ Page 6 of 18 WKS 12-3 pH OF STRONG ACIDS AND BASES continued Part B: More Challenging: Calculating Molarity from pH or pOH 8. A solution was prepared using 5.413 g of oxalic acid and a 0.50000 L volumetric flaks. Calculate the molarity of the solution. (0.1200 M) (b) What is the pH of the solution assuming both hydrogen ions dissociate (not a good assumption but let’s run with it!) (0.62) 9. A solution was prepared using 28.3 g of potassium hydroxide and then diluting to a final volume of 2.0000L. What is the molarity of the base solution? (0.252 M) (b) What is the pH of the solution? (13.40) 10. (a) A strong monoprotic acid was prepared by diluting 1.35 mL of a concentrated, 12.0 M solution to a final volume of 0.250 L. Calculate the final molarity of the solution. (0.0648 M) (b) What is the molar concentration of the hydrogen ion? (0.0648 M) (c) What is the pH of the solution? (1.19) (d) What color would phenolphthalein be in this solution? 11. Which would have a higher pH—a 0.035 M potassium hydroxide solution or a 0.018 M calcium hydroxide solution? Explain. (Ca(OH)2) 12. Which would have the more acidic pH-a 0.0025 M strontium hydroxide solution or a solution whose hydrogen ion concentration is 1.44 x 10-13? (.0025 M Sr(OH)2) 13. If the barium ion concentration of a barium hydroxide solution is known to be 0.25 M , what is the pH of the solution? (pH = 13.70) NAME__________________________________ PERIOD _______ Page 7 of 18 Worksheet 12-4 WEAK ACID AND BASE PROBLEM PRACTICE (three pages) A. Given molarity & K’s, find other stuff 1. Answer the following questions regarding a 0.35 M acetic acid solution. R Ka = I C % ionization = E _______________ (a) What is the percent ionization? (0.72%) _______________ (b) What is the pH of this solution? (pH = 2.60) _______________ (c) What is the hydroxide concentration in this solution? [4.0 x 10-12] 2. Answer the following questions regarding a 2.35 M ammonia solution. R Kb = I C % ionization = E _______________ (a) What is the pH? (pH = 11.81) _______________ (b) What is the hydroxide ion concentration in this solution? (6.50 x 10-3 M) _______________ (c) What percent is this solution ionizing? (0.28%) _______________ (d) Would you expect a more dilute ammonia solution to ionize a greater amount or a lesser percentage of its molecules compared to a more concentrated ammonia solution? (greater; more water available per molecule) _______________ (e) How many grams of ammonia must be added to water to make 1.0 liter of an ammonia solution with a pH of 11.81? (40 g) _______________ (f) Which would have a LOWER pH, a 2.35 M ammonia solution or a 0.235 M solution? Why? 3. Would you expect a 2.4 M or a 1.2 M solution of methylamine to ionize the greater percent? Justify your answer with calculations. (1.2 M) problem continued on next page! R Kb = I C % ionization = E NAME__________________________________ PERIOD _______ Page 8 of 18 WKS 12-4 Cont. R Kb = I C % ionization = E B. Given pH & K’s, find other stuff 4. Answer the following questions for a nitrous acid solution that is known to have a pH of 3.21. R Ka = I C % ionization = E _______________ (a) What is the hydrogen ion concentration of this solution? (6.17 x 10-4 M) _______________ (b) what is the molar concentration of the acid? (8.45 x 10-4 M) _______________ (c) Would you expect a 2.0 M or a 3.0 M nitrous acid solution to have a HIGHER pH? (2.0 M) _______________ (d) Would you expect a 2.0 M or a 3.0 M nitrous acid solution to ionize the greater percentage? Why? (see question 5 for a hint!) (2.0 M) 5. How many grams of aniline, C6H5NH2, must be dissolved in water to make 3.00 L of solution whose pH is 8.8? (26.9 g) R I Kb = C E NAME__________________________________ PERIOD _______ Page 9 of 18 WKS 12-4 Cont. C. Given molarity and % ionization, find K and other stuff. 6. Answer the following questions regarding a 4.0 M hydroflouric acid solution that is known to ionize 1.3 %. R Ka = I C % ionization = E _______________ (a) What is the hydrogen ion concentration? (5.0 x 10-2 M) _______________ (b) What is the pH of the solution? (pH = 1.28) _______________ (c) What is the hydroxide ion concentration of the solution? (1.92 x 10-13 M) _______________ (d) Would you expect a 1.5 M hydroflouric acid solution to have a higher or a lower pH than the 4.0 M solution? (higher) _______________ (e) Does a 4.0 M solution of hydroflouric acid or a 1.5 M solution of hydrofluoric acid ionize a greater amount? Why? (1.5 M) _______________ (f) Does a 4.0 M solution of hydroflouric acid or a 1.5 M solution of Hydrofluoric acid have a LOWER pH? Why? 7. Answer the following questions regarding a 0.15 M solution of a weak acid, HA, that is known to ionize 0.23%. R Ka = I C % ionization = E _______________ (a) Find the Ka of the weak acid. (7.9 x 10-7) _______________ (b) What is the pH of this acid solution? (pH = 3.46) _______________ (c) What is the hydroxide ion concentration of this solution? (2.9 x 10-11 M) _______________ (d) Is this acid a weaker or a stronger acid than acetic acid? How do you how? (weaker; Ka is smaller) NAME__________________________________ PERIOD _______ Page 10 of 18 WKS 12-5 pH OF ACIDS AND BASES – Mixed Strong and Weak (one page) Find the pH of each of the following acids or bases: 8 0.50 M hypochlorous acid (pH = 3.91) 1. 0.80 hydrobromic acid (pH = 0.10) 2. 0.40 M ammonia (pH = 11.43) 9. 0.35 M sodium hydroxide (pH = 13.54) 10. 0.72 M hydroflouric acid (pH = 1.80) 3. 0.35 M formic acid (pH = 2.10) 11. If the pH of a potassium hydroxide solution is 9.5, what is 4. 0.066 M strontium hydroxide (pH = 13.12) the hydroxide ion concentration? (3.16 x 10-5 M) (b) What is the molar concentration of the potassium hydroxide solution? (3.16 x 10-5 M) 5. 0.33 M lithium hydroxide (pH = 13.52) 12. If the pH of a hydrobromic acid solution is 1.3, what is the hydrogen ion concentration? [5.0 x 10-2] (b) What is the molar concentration of the acid? [5.0 x 10-2] (c) What is the hydroxide ion concentration of the acid solution? [2.0 x 10-13] 6. 0.025 M hydroiodic acid (pH = 1.60) 13. If the pH of a nitrous acid solution is 4.5, what is the hydroxide ion concentration of the solution? [3.2 x 10-10 M] 7. 1.50 M ethylamine (C2H5NH2) solution (pH = 12.49) (b) What is the molar concentration of the nitrous acid solution? [2.2 x 10-6 M] NAME__________________________________ PERIOD _______ Page 11 of 18 Worksheet 12-6 pH OF SALTS, ACIDS, AND BASES WORKSHEET (one page) Indicate whether each of the following salt solutions would be acidic, basic, neutral, or near neutral. YOU MUST SHOW THE HYDROLYSIS REACTION FOR EACH SALT FOR CREDIT! Salt Hydrolysis reaction Acid Base Strength acidity strength 1. ammonium nitrate 2. potassium nitrate 3. strontium acetate 4. iron (III) phosphate 5. beryllium perchlorate 6. copper (II) chloride 7. cesium sulfite 8. chromium (III) chloride _______________ 9. (a)What is the pH of a 0.025 M hydrochloric acid solution? (pH = 1.60) _______________ (b) What is the hydroxide ion concentration in this solution? (4 x 10-13 M) _______________ 10. If the pH of an acetic acid solution is found to be 3.95, what is the molar concentration of the acetic acid? (6.99 x 10-4 M) _______________ (b) What is the percent ionization of the above acid? (16.0%) _______________ 11. If 10.0 grams of sodium hydroxide are dissolved in enough water to make 2.00 liters of solution, what is the pH of the solution? (pH = 13.1) _______________ 12. If the pH of a strontium hydroxide solution is found to be 11.54, what is the molar concentration of the solution? (1.734 x 10-3 M) NAME__________________________________ PERIOD _______ Page 12 of 18 Worksheet 12-7 More Practice, Please (two pages) 1. (a) Find the pH of a 0.0030 M solution of hydrochloric 5. If the pH of an ammonia solution is known to be 11.85, acid. (pH = 2.52) what is the molar concentration of the weak (b) What is the [H+] of the above solution? (0.0030 M) base? (2.78 M) (c) What is the [0H-] of the above solution? (3.33 x 10-12 M) (b) What is the percent ionization of this ammonia solution? (d) What is the pOH of the above solution? (pOH = 11.48) (0.25 %) 2. (a) If the pH of a nitric acid solution is 2.1, what is the molar concentration of the acid? (0.0079 M) (b) What is the [OH-] of the above solution? (1.27 x 10-12 M) 6. If the pH of a calcium hydroxide solution is known to be 8.5, what is the molar concentration of the solution? (1.58 x 10-6M) (b) What is the percent ionization of the above compound? (100 %) (c) What is the [OH-] of this solution? (3.16 x 10-6) 3. (a) If the pH of a HF solution is 2.3, what is its molar concentration? (0.071 M) (b) What is the [H+] of this acid? (0.00501M) (c) What is the percent ionization of this acid? (7.0 %) 7. If a 0.15 M solution of a weak acid is known to be 0.114% ionized, what is the Ka for this acid? (Ka = 1.43 x 10-7) (b) What is the [H+] for this acid? (0.00017 M) 4. (a) Find the pH of a 0.32 M solution of strontium (c) What is the pH for this acid? (pH = 3.77) hydroxide. (pH = 13.81) (b) What is the [OH-] of the above? (0.64 M) (c) What is the [H+] of the above? (1.56 x 10-14) NAME__________________________________ PERIOD _______ Page 13 of 18 WKS 12-7 Cont. 11. (a) If the pH of a solution is 12.3, how many grams of 8. Find the pH of a 1.50 M solution of hydroflouric acid. (pH calcium hydroxide have been dissolved to make 500. ml of = 1.48) solution? (0.369 g) (b) What is the hydroxide ion concentration? (2.00 x 10-2 M) (c) What is the calcium ion concentration? (9.98 x 10-3 M) (d) What is the molar concentration of the solution? (9.98 x 10-3 M) 9. (a) Find the molar concentration of a potassium hydroxide solution if its pH is 11.3. (2.0 x 10-3 M) (b) What is the [OH-] of the above solution? (2.0 x 10-3 M) 12. What is the percent ionization of 0.33 M lactic acid solution? (2.1 %) (b) What is the hydrogen ion concentration? (6.8 x 10-3 M) (c) What is the hydroxide ion concentration? (1.5 x 10-12 M) (d) What is the pH of this solution? (pH = 2.17) 10. If the pH of a hypoiodous acid solution is 5.5, what is the molar concentration of the acid? (0.50 M) (b) What is the percent ionization of this acid? (6.3 x 10-4 %) (c) What is the hydroxide ion concentration? (3.16 x 10-9 M) (d) What is the hydrogen ion concentration? (3.16x 10-6 M) 13. How many grams of strontium hydroxide must be dissolved to make 3500 ml of a solution whose pH is 12.7? (10.7 g) (b) What is the hydroxide ion concentration of this solution? (5.01 x 10-2 M) (c) What is the strontium ion concentration of this solution? (2.51 x 10-2 M) (d) What is the molar concentration of the solution?(2.51 x 10-2) NAME__________________________________ PERIOD _______ Page 14 of 18 WKS 12-8: Titration Problems & Vocab review ( 3 pages) 1. What is the molarity of a solution of HCl if 25.0 mL is titrated to an endpoint by 10.0 mL of a 0.200-M solution of NaOH? (0.08 M HCl) 2. What is the molarity of a solution of Ba(OH)2 if 50.0 mL are titrated to an endpoint by 15.0 mL of a solution of HCl that is 0.00300 M? (4.5 x 10-4 M Ba(OH)2) 3. What is the molarity of a nitric acid solution if 21.0 mL are needed to completely neutralize 25.0 mL of 0.300 M NaOH? (0.357 M HNO3) 4. What is the molarity of a solution of KOH if 45.0 mL are completely neutralized by 15.0 mL of 0.500-M sulfuric acid solution in a reaction in which K2SO4 is one of the products? (0.333 M) 5. What is the concentration of a Sr(OH)2 solution if 20.0 mL of it is neutralized by 25.0 mL of a standard 0.0500 M HCl? (0.0313 M) 6. If 25.0 mL of a 0.10 M NaOH solution are required to neutralize 15.0 mL of HCl, what is the molarity of the acid? (0.17 M) 7. What is the molarity of a KOH solution if 35.0 mL of it are neutralized by 15.0 mL of 0.765 M sulfuric acid? (0.656 M) 8. If 25.0 mL of vinegar solution (acetic acid) is neutralized 15.0 mL of 0.500 M NaOH, what is the molarity of the vinegar? (0.300 M) 9. How many mL of 0.0200 M LiOH will neutralize 15.0 mL of 0.400 sulfuric acid? (600 mL) 10. What volume of 0.196 M LiOH is required to neutralize 27.3 mL of 0.413 M HBr? (57.5 mL) 11. What is the concentration of a solution of NaOH if 21.2 mL of a 0.0800 M solution of HBr is needed to neutralize 25.0 mL of the base? (0.0678 M base) 12. If 86.2 mL of 0.765 M NaOH neutralize 30.0 mL of HCl, what is the concentration of the acid? (2.20 M HCl) 13. If 40.8 mL of 0.106 M sulfuric acid neutralize 61.8 mL of KOH, what is the concentration of the base? (0.140 M) NAME__________________________________ PERIOD _______ Page 15 of 18 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 NAME__________________________________ PERIOD _______ Page 16 of 18 ACROSS 3. each whole number on the pH scale indicates the acid or base is _____ stronger or weaker than the 1. Substances such as water or HCO3─ are called next number (2 words) ____________________ because they can act as an 4. Indicators change ____ to show different pH acid or a base. values 6. pH 11 is ______ _________ times stronger than 5. Acid could have the pH value: pH 8 (2 words) 7. precipitation with a pH of less than 5.6 (2 words) 9. Strong bases can do this to the skin 8. Strong acids ionize __________ ____________ 10. H3O+ = ______ ion _________ (three words) 11. Mathematical tool for weak acids or bases 12. Bases feel __________________ 13. conducts electricity 15. Characteristic of a substance that reacts strongly 14. Type of solution that forms during the with a metal hydrolysis of potassium fluoride 17. Substance that can accept an electron pair (two 16. Reaction between an acid and a base words) 18. Substance that can donate an electron pair is 18. Bronsted’s buddy called a ____________base 19. Type of mathematics used for strong acids and 21. Type of acid or base that must be present in a bases buffer solution 20. used to measure strength of an acid or base (two 22. taste of an acid words) 23. Common name for well known weak acid used 21. one of the products of neutralization in food preparation 25. one product of a neutralization reaction 24. A polyatomic with a suffix “-ite” would form an 27 An acid with the suffix “-ic” is derived from a acid with the suffix “-_____” polyatomic with the suffix “-____” 26. Pure water would have this pH 29. pH of a solution that turns faint pink in the 28. These pairs differ only by a proton presence of phenolphthalein 31 A base could have this pH value 30. When the forward rate is equal to the reverse 32. point in a titration when an acid or base is fully rate in a solution of weak acid or base, the system neutralized (two words) has reached ______________________ 35. Resulting pH for the hydrolysis of ammonium 31. The hydroxide ion has this kind of charge perchlorate 33. organic material that changes color with an acid 37. Phosphoric acid is called _____________ or base because it can donate more than one proton. 34. indicator made from a lichen, comes in red or 42. highest number on pH scale blue 43. process used to find the concentration of an acid 36. Mathematical relationship between base or base by neutralizing it with a known amount of molarity and pH acid or base 37. Negative log base 10 of [OH─] 45. point in a titration when an indicator changes 38. ion formed when an acid ionizes color 39. taste of a base 47. A mixture that can resist changes in pH 40. pH for a solution of potassium chloride 49. Acids with larger values of Ka are 41. Mathematical relationship between pH and [H+] ______________ acids 42 What you must do to pass Pre-AP Chemistry 51. Gas that forms when active metals react with (focus) acids. 44. The binary acid, hydrobomic acidy had an ion with the suffix “______-“ in its name. DOWN 46. As the molarity of an acid increases, the pH of the solution goes _______________ 1. Dead guy whose theory defines a base as a 48. Phosphoric acid is a ______protic acid. substance that dissociates to form a hydroxide ion 50. the hydroxide ion is represented by this 2. Measure of the strength of an acid or base (two chemical formula words) NAME__________________________________ PERIOD _______ Page 17 of 18 Acid-Dissociation Constants at 25°C ACID Formula Ka1 Ka2 Ka3 Acetic CH3COOH 1.8 x 10 -5 Acetylsalicylic C 9H 8O 4 3.0 x 10 -4 Arsenic H3AsO4 5.6 x 10 -3 1.7 x 10 -7 4.0 x 10 -12 Arsenious H3AsO3 6 x 10 -10 Ascorbic HC6H7O6 8.0 x 10 -5 Benzoic C6H5COOH 6.5 x 10 -5 Boric H3BO3 5.8 x 10 -10 Carbonic H2CO3 4.3 x 10 -7 5.6 x 10 -11 Chloroacetic CH2ClCOOH 1.4 x 10 -3 Citric C 6H 8O 7 7.1 x 10 -4 1.7 x 10 -5 4.1 x 10 -7 Cyanic HCNO 1.8 x 10-4 Formic HCOOH 1.8 x 10 -4 Hydrazoic HN3 1.9 x 10 -5 Hydrocyanic HCN 4.9 x 10 -10 Hydrofluoric HF 3.5 x 10 -4 Hydrogen Peroxide H 2O 2 2.4 x 10 -12 Hydrosulfuric H 2S 1.0 x 10 -7 ~10 -19 Hypobromous HBrO 2.0 x 10 -9 Hypochlorous HClO 3.5 x 10 -8 Hypoiodous HIO 2.3 x 10 -11 Lactic HC3H5O3 1.4 x 10-4 Nitrous HNO2 4.5 x 10-4 Propionic HC3H5O2 1.3 x 10-5 NAME__________________________________ PERIOD _______ Page 18 of 18 Base-Dissociation Constants at 25°C Base Formula Kb Ammonia NH3 1.8 x 10-5 Aniline C6H5NH2 4.3 x 10-10 Codeine C18H21NO3 1.6 x 10-6 Dimethylamine (CH3)2NH 5.4 x 10-4 Ethylamine C2H5NH2 6.4 x 10-4 Hydrazine N 2H 4 8.9 x 10-7 Hydroxylamine NH2OH 9.1 x 10-9 Methylamine CH3NH2 4.3 x 10-4 Morphine C17H19NO3 1.6 x 10-6 Piperidine C5H11N 1.3 x 10-3 Propylamine C3H7NH2 5.1 x 10-4 Pyridine C5H5N 1.8 x 10-9 Strychnine C21H22N2O2 1.8 x 10-6 Trimethylamine (CH3)3N 6.5 x 10-5