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Brønsted /Lowry Neutralization

Brønsted /Lowry Neutralization. What is an acid?. Brønsted /Lowry acid: a proton donor proton donor ?... a proton is also an H + ion in water , H 2 O + donated H +  H 3 O + H 3 O + = “ hydronium ion”. What is a base?. Brønsted /Lowry base: a proton acceptor

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Brønsted /Lowry Neutralization

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  1. Brønsted/Lowry Neutralization

  2. What is an acid? • Brønsted/Lowry acid: a proton donor proton donor?... a proton is also an H+ ion • in water, H2O + donatedH+ H3O+ • H3O+= “hydronium ion”

  3. What is a base? • Brønsted/Lowry base: a proton acceptor proton acceptor?... any substance that will take an H+ ion • in water, H2O+ base  OH- + Hbase

  4. Brønsted/Lowry “Neutralizations” • Acid1+ Base1 Acid2 + Base2 • For weak acids and weak bases • Note the double arrow!

  5. Acid1+ Base1 Acid2 + Base2 • Acid1 H++ Base2 • Acid1 donates H+ and becomes Base2, its “conjugate base” • H+ + Base1Acid2 • Base1 accepts the H+ from Acid1 and becomes Acid2, its “conjugate acid”

  6. Brønsted/Lowry examples • Examples… HF + H2O  F- + H3O+ • HF donates an H+…so it is an “acid” • H2O takes the H+ from the HF… so it is the “base”

  7. Cont… HF + H2O  F-+ H3O+ • Look at the “reverse” reaction • which donates an H+?...it is an “acid” H3O+ • which takes the H+ from the H3O+?...it is the “base” F-

  8. Cont… HF + H2O F-+ H3O+ • HF –a weak acid –becomes F-, a base • H2O, acting as a base, becomes H3O+,an “acid” • The acid becomes its “conjugate base” • The base becomes its “conjugate acid”

  9. Another example NH3 + H2O  NH4+ + OH- • H2O donatesan H+... So it is an “acid” • NH3 takes the H+ from the H2O… so it is the “base”

  10. Cont… NH3+ H2O NH4++ OH- • H2O–a weak acid –becomes OH-, a base • NH3, acting as a base, becomes NH4+,an “acid” • The acid becomes its “conjugate base” • The base becomes its “conjugate acid”

  11. Brønsted/Lowry neutralization Their conjugate acid and base A weak acid + A weak base Remember… • Weak acids lose an H+ and become their conjugate bases • Weak bases gain an H+ and become their conjugate acids

  12. Did you notice? • …that H2O was listed as an acid, and as a base, but a pure H2O solution has pH = 7? • H2O can act as an acid (lose an H+) or a base (accept an H+) depending on what it is combined with • AMPHOTERIC: act as an acid when with a base; act as a base when with an acid

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