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