21.1. Acid-Base Definitions www.ck12.org 21.1 Acid-Base Definitions Worksheet Name _____________________ Class ______________________ Date ________________ Answer each of the questions below to show your achievement of the lesson objectives Lesson Objective: Describe the properties of acids and bases. 1. All of the following are acids except 1. 2. 3. 4. citrus fruits carbonated soda drain cleaner vinegar 2. All of the following are properties of acids except 1. 2. 3. 4. sour taste aqueous solutions are electrolytes turn litmus blue react with some metals to produce H2 3. All of the following are properties of bases except 1. 2. 3. 4. 4. 5. 6. 7. turn litmus red bitter taste do not react with metals aqueous solutions are electrolytes True/False: Oranges contain ascorbic acid True/False: Sodium hydrogen carbonate is an antacid. True/False: All acids are strong electrolytes. Fill in the table below TABLE 21.1: Property color with phenolphthalein color with litmus taste reactivity with metals Acids Bases 8. Fill in the table below by naming the acid or base contained in the material 206 www.ck12.org Chapter 21. Acids and Bases Worksheets TABLE 21.2: Material drain cleaner carbonated soda vinegar antacid cleaners orange Acid or Base Present in Material Lesson Objective: Define an acid and a base according to the Arrhenius theory. 9. An Arrhenius acid is a compound with 1. 2. 3. 4. reactive hydrogen atoms ionizable hydrogen atoms covalently bound hydrogen atoms hydrogen atoms attached to carbon 10. An Arrhenius base is a compound with 1. 2. 3. 4. ionizable OH group covalently bound OH group reactive OH group OH group attached to carbon 11. True/False: CH3 CH2 OH is an Arrhenius base. 12. True/False: All Arrhenius bases are completely ionizable. 13. Define the following terms: 1. monoprotic acid 2. polyprotic acid 14. Fill in the blank spaces in the table below: TABLE 21.3: Compound CH3 COOH Mg(OH)2 Name hypochlorous acid phosphoric acid calcium hydroxide KOH sulfuric acid Lesson Objective: Define an acid and a base according to the Brønsted-Lowry theory. Be able to identify the conjugate acid-base pairs in a Brønsted-Lowry acid-base reaction. 15. A hydrogen ion is often referred to as a 1. 2. 3. 4. positron H atom proton portion 207 21.1. Acid-Base Definitions www.ck12.org 16. All of the following are true about ammonia except 1. 2. 3. 4. contains hydroxide group reacts with acid turns litmus blue turns phenolphthalein pink 17. A Brønsted-Lowry acid-base reaction involves 1. 2. 3. 4. 18. 19. 20. 21. formation of hydroxide ion transfer of proton utilization of water formation of free hydrogen ion True/False: A hydrogen atom is also called a proton. True/False: Water can act as a Brønsted-Lowry acid. True/False: The hydroxide ion is a Brønsted-Lowry acid. Define the following terms: 1. 2. 3. 4. 5. Brønsted-Lowry acid Brønsted-Lowry base amphoteric conjugate acid conjugate base 22. Identify the acid and base and the conjugate acid and base in each of the following reactions: 1. HClO4 (aq) + H2 O(l) H3 O+ (aq) +ClO− 4 (aq) − (aq) + H SO (aq) 2. HF(aq) + HSO− (aq) F 2 3 3 3. HNO2 (aq) + HS− (aq) NO− 2 (aq) + H2 S(aq) Lesson Objective: Define an acid and a base according to the Lewis theory. 23. A Lewis acid 1. 2. 3. 4. donates a pair of electrons to form a covalent bond releases a proton accepts a proton accepts a pair of electrons to form a covalent bond 24. A Lewis base 1. 2. 3. 4. donates a pair of electrons to form a covalent bond releases a proton accepts a proton accepts a pair of electrons to form a covalent bond 25. True/False: Ammonia can serve as a Lewis base. 26. True/False: A Lewis base forms an ionized compound 27. Identify the acid and the base in each Lewis acid-base reaction. 1. 2. 3. 4. (CH3 )2 O + BF3 → (CH3 )2 O : BF3 H2 O + SO3 → H2 SO4 BeCl2 + 2Cl − → BeCl42− BH3 + (CH3 )2 S → H3 B : S(CH3 )2 28. A Lewis acid is a substance that accepts a pair of electrons to form a covalent bond. A Lewis base is a substance that donates a pair of electrons to form a covalent bond. In a Lewis acid-base reaction, a new covalent bond is formed, but both of the electrons in that bond were originally present on the base. 29. Is the bond formed truly covalent? 208 www.ck12.org Chapter 21. Acids and Bases Worksheets 30. Why did scientists develop three different classifications for acids and bases? 209 21.1. Acid-Base Definitions www.ck12.org TABLE 21.4: Property color with phenolphthalein color with litmus taste reactivity with metals Acids colorless red sour good Bases pink blue bitter non-reactive TABLE 21.5: Material drain cleaner carbonated soda vinegar antacid cleaners orange Acid or Base Present in Material sodium hydroxide phosphoric acid acetic acid magnesium hydroxide, sodium hydrogen carbonate ammonia citric acid, ascorbic acid TABLE 21.6: Compound CH3 COOH Mg(OH)2 HClO H3 PO4 Ca(OH)2 KOH H2 SO4 Name acetic acid magnesium hydroxide hypochlorous acid phosphoric acid calcium hydroxide potassium hydroxide sulfuric acid TABLE 21.7: Acid HClO4 HF HNO2 210 Base H2 O HSO3 − HNO2 Conjugate Acid H3 O+ H2 SO3 H2 S Conjugate Base ClO4 − F− NO2 −
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