1. Unit 13 Marker Board Review Acids & Bases You need a marker board, marker, eraser, calculator, & periodic table.

2. Question #1 List 4 properties of acids. Answer: 1 – Sour taste 2 – React with metals to form hydrogen gas 3 – React with metal carbonates to form CO 2 gas 4 – Turn indicators red

3. Question #2 List 4 properties of bases. Answer: 1 – Taste bitter 2 – Unreactive with metals and carbonates 3 – Feel slippery 4 – Turn indicator blue

4. Question #3 According to Arrhenius, acids ionize to produce _______ ions & bases ionize to produce _______ ions. Answer: hydrogen hydroxide

5. Question #4 A Bronsted acid _____________ a _______________ and a base ______________ a ____________. ___________ is a substance that can either donate or accept a H+ ion. Answer: - donates, hydrogen ion - accepts, hydrogen ion - Amphoprotic/Amphoteric

6. Question #5 Label the Acid, Base, Conjugate Acid, & Conjugate Base for each reaction below: NH 3 + H 2 O  NH 4 + + OH - H 2 CO 3 + H 2 O  H 3 O + + HCO 3 - Answer: NH 3 + H 2 O  NH 4 + + OH - B A CA CB H 2 CO 3 + H 2 O  H 3 O + + HCO 3 - A B CA CB

7. Question #6 Strong acids ionize _______________ while weak acids ionize ________________. Which is the stronger acid? Oxalic Acid: Ka = 5.1 x 10 -5 Carbonic Acid: Ka = 4.8 x 10 -11 Answer: completely; only partially; Oxalic Acid (larger Ka value)

8. Question #7 When an acid reacts with a base to neutralize it, the products are a ___________ & ___________. Answer: Salt & Water

9. Question #8 List (write the formula for) the 6 strong acids. Answer: HCl HI HBr HClO 4 HNO 3 H 2 SO 4

10. Question #9 Acids have a pH ___________ than 7. Bases have a pH __________ than 7. Pure water has a pH of _____ because...? Answer: Less Greater 7 because it is neutral!

11. Question #10 HBr NaOH HNO 2 H 3 PO 3 NH 3 H 2 SO 4 Mg(OH) 2 H 2 CO 3 HC 2 H 3 O 2 Write the name for the following formulas. Is it an acid or base? Check your answers after you’ve written ALL of them! Hydrobromic Acid—acid Sodium Hydroxide—base Nitrous Acid—acid Phosphorous Acid - acid Ammonia—base Sulfuric Acid—acid Magnesium Hydroxide - base Carbonic Acid—acid Acetic Acid—acid

12. Question #11 Write & balance the equation for the neutralization of sulfuric acid with potassium hydroxide. Answer: H 2 SO 4 + 2 KOH  2 H 2 O + K 2 SO 4

13. Question #12 Write & balance the neutralization reaction of hydrobromic acid & calcium hydroxide. Answer: 2 HBr + Ca(OH) 2  2 H 2 O + CaBr 2

14. Question #13 The formula for the hydronium ion is ____________________ & for the hydroxide ion _______________. Answer: H 3 0 + & OH -

15. Question #14 An H + ion is really just a _______________ and cannot exist in solution. Answer: Proton

16. Question #15 Write the equation for the self-ionization of water. Answer: H 2 O + H 2 O  OH - + H 3 O +

17. Question #16 The formula for calculating [H 3 O + ] from pH is ______________________. I type this into my calculator as: _________ Answer: [H 3 O + ] = 10^(-pH) 2 nd log (negative pH)

18. Question #17 The formula for calculating [H 3 O + ] from [OH - ] is ______________________. I type this into my calculator as: _______ Answer: Kw = [OH - ][H 3 O + ] = 1.0 x 10 -14 [H 3 O + ] = 1.0 x 10 -14 [OH-] 1.0 E -14 / [OH-]

19. Question #18 List the formulas for pH, H + concentration, pOH, & OH - concentration. Answer: pH = -log [H + ] OR 14 - pOH [H+] = 10^(- pH) OR 1.0 x 10 -14 / [OH - ] pOH = -log [OH - ] OR 14 - pH [OH-] = 10^(- pOH) OR 1.0 x 10 -14 / [H 3 O + ]

20. Question #19 pH + pOH = ___________ Answer: 14

21. Question #20 What is the pH of an HCl solution with a concentration of 0.0015 M? Acidic or basic? Answer: pH = -log (0.0015) = 2.8 Acidic

22. Question #21 What is the pH of a solution with an pOH of 10.5? Acidic or basic? Answer: pH = 14 – pOH = 14 – 10.5 = 3.5 Acidic

23. Question #22 What is the [H + ] of a solution with a pH of 4.51? Answer: [H+] = 10^(-4.51) = 3.09 x 10 -5 M

24. Question #23 What is the pOH of a solution with a [H+] of 9.99 x 10 -9 M? Acidic or basic? Answer: pOH = -log [OH-] [OH-] = 1.0 x 10 -14 / 9.99 x 10 -9 = 1.0 x 10 -6 M pOH = -log(1.0 x 10 -6 ) = 6.0 pH = 14 – 6.0 = 8.0  Basic

25. Question #24 What is the pOH of a solution with an [OH-] of 7.81 x 10 -3 M? Acidic or basic? Answer: pOH = -log [OH-] = -log (7.81x10 -3 ) = 2.1 pH = 14 – 2.1 = 11.9  Basic

26. Question #25 Calculate the [OH - ] if the pOH is 5.21. Answer: [OH - ] = 10^(-5.21) = 6.17 x 10 -6 M.

27. Question #26 What is the purpose of a titration? What is the role of an indicator in a titration? What has been reached when acid and base completely neutralize one another? Answer: A titration enables you to determine the concentration of a solution by reacting a known volume of the solution with a solution of known concentration. An indicator changes color when the end point of the titration has been reached. The end point has been reached.

28. Question #27 You add a substance to pure water and the pH rises from 7 to 9. What has happened to the concentration of H 3 O + ? Is the substance added an acid or a base? Answer: The concentration of H 3 O + has decreased. The substance is a base.

29. Question #28 In the titration of a strong acid with a strong base, what pH range should the indicator have? Answer: 6-8

30. Question #29 Write the balanced equation for the reaction between nitric acid and magnesium hydroxide. Answer: 2 HNO 3 + Mg(OH) 2  Mg(NO 3 ) 2 + 2 H 2 O

31. Question #30 What is the molarity of HNO 3 if 15.0 mL is completely neutralized by 38.5 mL of 0.15 M Mg(OH) 2 ? Answer: 2 HNO 3 + Mg(OH) 2  Mg(NO 3 ) 2 + 2 H 2 O MaVaCb = MbVbCa Ma(15.0)( 1) = (0.15)(38.5)(2) Ma = 0.77 M