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Brønsted-Lowry theory of acids and bases

H + is transferred. Note:We often say “Proton”. Brønsted-Lowry theory of acids and bases. H + Cl - + NH 3 Cl - + NH 4 +. An acid is a H + donor HCl A base is a H + acceptor NH 3. HCl + H 2 O H 3 O + (aq) + Cl - (aq). Oxonium Ion. acids and bases in solution.

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Brønsted-Lowry theory of acids and bases

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  1. H+ is transferred Note:We often say “Proton” Brønsted-Lowry theory of acids and bases H+ Cl- + NH3Cl- + NH4+ An acid is a H+ donor HCl A base is a H+ acceptor NH3

  2. HCl + H2O H3O+(aq) + Cl- (aq) Oxonium Ion acids and bases in solution HCl H+(aq) + Cl- (aq)

  3. NaOH Na+(aq) + OH- (aq) CO3 2- (aq) +H2O(l) HCO33-aq) + OH-(aq) Alkalis vs bases A base is a H+ acceptor An alkali is a base that dissolves in water to form hydroxide ions. All alkalis are bases; not all bases are alkalis!

  4. HA(aq) H+(aq) + A- (aq) Conjugate acid Conjugate base Acid-base pairs An acid exists in solution in equilibrium: Overall we call this a conjugate acid-base pair

  5. H2O(aq) H+(aq) + OH- (aq) H3O+(aq) H+(aq) + H2O(aq) Acid-base pairs Water can act as an acid OR a base: Proton donor Proton acceptor We say water is amphoteric

  6. HCl(aq) H+(aq) + Cl- (aq) C2H5OH (aq) H+(aq) + C2H5O -(aq) Strength of acids and bases A strong acid donates protons easily. A weak acid donates protons less easily, however the conjugate base accepts protons more easily than a strong acid

  7. HIn(aq) H+(aq) + In-(aq) base When you add an acid Acid-base Indicators Acid base indicators are coloured organic substances that are weak acids. For example: Litmus acid

  8. HIn(aq) H+(aq) + In-(aq) base When you add a base: HIn(aq) + OH- H2O(l) + In-(aq) Acid-base Indicators Acid base indicators are coloured organic substances that are weak acids. For example: Litmus acid

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