Back to quiz

6. A strong acid is

  • An acid that completely dissociates in solution
  • pH=-log[H+(aq)]

7. Aqueous acids react with bases (eg MgO) forming

  • Salt and water
  • Salt carbon dioxide and water

8. An alkali is

  • A base that dissolves in water forming OH-(aq) ions
  • Salt carbon dioxide and water

9. Depending on their formulae and bonding, different acids can

  • H2SO4: H2SO4(aq) ---> H+(aq) + HSO4-(aq) and HSO4-(aq) ---> H+(aq) + SO42-(aq)
  • Release different numbers of protons
  • A proton donor

10. HCl, HNO3, H2SO4, HBr, HI and HClO4 are all _______ acids

  • Strong
  • Weak

11. A pH change of 1 changes [H+(aq)] by

  • 10 times
  • pH=-log[H+(aq)]

12. The Ka expression for weak acids can be simplified:

  • Ka = [H+(aq)]^2 / [HA(aq)]
  • Low
  • HCl

13. An acid base pair is

  • A pair of two species that transform into each other by gain or loss of a proton
  • pH=-log[H+(aq)]

14. As the [H+(aq)] for a strong acid is equal to the concentration of the acid, (therefore [H+(aq)] = [HA(aq)]) the pH

  • Can be easily calculated using pH = -log[H+(aq)]
  • Low

15. H3PO4 is a

  • Tribasic acid
  • H2SO4: H2SO4(aq) ---> H+(aq) + HSO4-(aq) and HSO4-(aq) ---> H+(aq) + SO42-(aq)

16. Aqueous acids react with alkalis (KOH) forming

  • Salt and water
  • Salt carbon dioxide and water

17. A weak acid is

  • An acid that partially dissociates in solution
  • An acid that completely dissociates in solution

18. To work Ka out from pKa the formula is

  • Ka = 10^-pKa
  • pKa = -log10Ka
  • A small extent of dissociation therefore the acid is weak

19. A small Ka value indicates

  • The acid is strong
  • A small extent of dissociation therefore the acid is weak
  • An equilibrium

20. A bronsted Lowry acid

  • A proton donor
  • Salt and hydrogen