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Chemistry Jeopardy Unit 7

Chemistry Jeopardy Unit 7. Acids Donate H + ions B. React with metals C. Turn blue litmus red D. All of the above. Which ion could act as a base H + NH 4 + H 3 O + NO 2 -. Acid/Base definition that requires species be in solutions Lewis Arrhenius Bronsted/Lowry

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Chemistry Jeopardy Unit 7

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  1. Chemistry Jeopardy Unit 7

  2. Acids • Donate H+ ions • B. React with metals • C. Turn blue litmus red • D. All of the above

  3. Which ion could act as a base • H+ • NH4+ • H3O+ • NO2-

  4. Acid/Base definition that requires species be in solutions • Lewis • Arrhenius • Bronsted/Lowry • Dalton

  5. Weak acids have equilibrium constants that are. • Large • Small • Zero • Nonexistent

  6. Which of the following is a property of a base • Tastes sour • Is a nonelectrolyte • Turns blue litmus red • pH greater than 7

  7. Nitric Acid (HNO3) • Strong • Weak

  8. Ammonia (NH3) • Strong • Weak

  9. Sulfuric Acid (H2SO4) • Strong • Weak

  10. Potassium Hydroxide (KOH) • Strong • Weak

  11. Carbonic Acid (H2CO3) • Strong • Weak

  12. Solutions conduct electricity because • There are ions in solution • They feel like it • There are molecules in solution • Water conducts electricity

  13. Strong acids are also • Strong electrolytes • Weak electrolytes • Nonelectrolytes • Groovy

  14. What is the conjugate base of carbonic acid (H2CO3) • H3CO3+ • HCO3- • CO3-2 • OH-

  15. Buffered solutions • Minimize a solutions change in pH • Restrict any change in pH • Keep shoes shiny • Have no effect on pH

  16. What two ingredients could make a buffer? • A. HNO3 & NaNO3 • NH3 & HCl • HClO4 & KClO3 • HClO & NaClO

  17. Acidic solutions have a pH • Equal to 7 • Above 7 • Below 7 • Anywhere between 0 and 10

  18. A solution of .10 M HCl has a pH of • 0.10 • 1.00 • 10.00 • 13.00

  19. A solution of .10 M KOH has a pH of • 0.10 • 1.00 • 10.00 • 13.00

  20. A 1.0M solution of a weak acid with a Ka of 1.0x10-4 has a pH of • 1.00 • 2.00 • 4.00 • 12.00

  21. When the [OH-] is 1x10-4M What is the pOH? • 4.00 • 10.00 • 12.00 • 14.00

  22. Point in a titration where a color change occurs • Equivalence Point • End Point • Stop Point • Sharp Point

  23. Chemical used to mark the endpoint in a titration • Acid • Base • Indicator • Catalyst

  24. The solution of unknown concentration in a titration • Titrant • Indicator • Base • Analyte

  25. Long tubes used to deliver precise volumes on solution in a titration • Burets • Graduated cylinders • Volumetric Flask • Erlenmeyer Flask

  26. 20.00 mL of 1.0M NaOH is titrated with 20.00 mL of HCl of unknown concentration. What is the HCl concentration? • 0.50M • 1.0M • 2.0M • 4.0M

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