Acids, bases and neutralisation Flashcards Preview

CHEM - 2.1.4 - 2.1.5 Acids and Redox > Acids, bases and neutralisation > Flashcards

Flashcards in Acids, bases and neutralisation Deck (7)
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1
Q

What are acids?

A
  • Acids are proton donors as they release hydrogen ions when mixed with water.
    e.g:
    H2SO4 + H2O = 2H(+) + SO4(2-)
  • Strong acids completely dissociates by releasing all Hydrogen atoms in aqueous solution:
    HCl -> H(+) + Cl(-)
  • Weak acids partially dissociates as only small proportion of hydrogen atoms are released as ions in aq. solutions:
    CH3COOH <=> H(+) + CH3COOH(-)
    <=> equilibrium sign indicates that forward reaction is incomplete.
2
Q

Bases and alkalis

A
  • Bases neutralise acid to form salts.
  • Alkali is a base that dissolves in water and releases Hydroxide ions (OH-) in solution:
    NaOH -> Na(+) + OH(-)
3
Q

Neutralisation

A
  • General formula of neutralisation reaction is:
    Acid + Base -> Salt + Water
    Ionic reaction:
    H(+) + OH(-) -> H2O
4
Q

Products of neutralisation

A
  • Acid + METAL -> salt + hydrogen
  • Acid + metal OXIDE* -> salt + water
  • Acid + metal CARBONATE** -> salt + water = carbon dioxide
  • reaction of metal hydroxide is the same as metal oxide ** reaction of metal hydrogen carbonate is the same as metal carbonate
5
Q

Charges of some ions

A

NH4(+)

NO3(-), HCO3(-), Ethanoate: CH3COO(-)

SO4(2-), CO3(2-)

PO4(3-)

6
Q

Partial and complete neutralisation reactions of carbonic acid w/ sodium hydroxide

A

NaOH + H2CO3 -> NaHCO3 + H2O

2NaOH + H2CO3 -> Na2CO3 + 2H2O

7
Q

Why is sodium hydrogencarbonate called an acid salt?

A

One hydrogen atom has been replaced by a metal ion. The other hydrogen atom can still behave as an acid.