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Unit 13 Marker Board Review

Unit 13 Marker Board Review. Acids & Bases Made with love and care by. 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. Question #2.

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Unit 13 Marker Board Review

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  1. Unit 13 Marker Board Review Acids & Bases Made with love and care by

  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 CO2 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 must contain _______ ions & bases must contain _______ ions. Answer: hydrogen hydroxide

  5. Question #4 A Bronsted acid _____________ a _______________ and a base ______________ a ____________. Answer: - donates - hydrogen ion - accepts - hydrogen ion

  6. Question #5 Label the Acid, Base, Conj Acid, Conj Base • NH3 + H2O  NH4+ + OH- • H2CO3 + H2O  H3O+ + HCO3- Answer: NH3 + H2O  NH4+ + OH- B A CA CB H2CO3 + H2O  H3O+ + HCO3- A B CA CB

  7. Question #6 (Acc Only) Base anhydrides contain a _________________ and oxygen. Acid anhydrides contain a _________________ and oxygen. Answer: Metal Nonmetal

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

  9. Question #8 Pure water has a pH of _________ because … Answer: 7…Because it is neutral!

  10. Question #9 Acids have a pH ___________ than 7; bases _____________ than 7. Answer: Less Greater

  11. Question #10 Write the name for the following formulas. Is it an acid or base? Check your answers after you’ve written ALL of them! • HBr • NaOH • HNO2 • HCN • NH3 • H2SO4 • Mg(OH)2 • H2CO3 • HC2H3O2 Hydrobromic Acid—acid Sodium Hydroxide—base Nitrous Acid—acid Hydrocyanic 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: H2SO4 + 2 KOH  2 H2O + K2SO4

  13. Question #12 Write & balance the neutralization reaction of hydrobromic acid & calcium hydroxide. Answer: 2 HBr + Ca(OH)2 2 H2O + CaBr2

  14. Question #13 The formula for the hydronium ion is ____________________ & for the hydroxide ion _______________. Answer: H30+ & 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: H2O + H2O  OH- + H3O+

  17. Question #16 The formula for calculating [H3O+] from pH is ______________________. I type this into my calculator as: _________ Answer: [H3O+] = 10^(-pH) 2nd log (negative pH)

  18. Question #17 The formula for calculating [H3O+] from [OH-] is ______________________. I type this into my calculator as: _______ Answer: Kw = [OH-][H3O+] = 1.0 x 10-14 [H3O+] = 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 / [H3O+]

  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? • Answer: pH = -log (0.0015) = 2.8

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

  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? 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

  25. Question #24 • What is the pOH of a solution with an [OH-] of 7.81 x 10-3 M? Answer: pOH = -log [OH-] = -log (7.81x10-3) = 2.1

  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? 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.

  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 H3O+? Is the substance added an acid or a base? Answer: The concentration of H3O+ 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 #29provided by Sam B.S for your benefit • In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluoric acid solution. What is the molarity of the hydrofluoric acid solution? • MHF = 0.5015M

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