Brønsted–Lowry Acids & Bases

01Brønsted–Lowry Acids & Bases

Acids and bases

This section covers Brønsted–Lowry definitions and proton transfer in an acid–base reaction.

Brønsted–Lowry definitions

Acid: a proton donor.

Base: a proton acceptor.

An acid–base reaction involves transfer of a proton from the acid to the base.

Identifying the acid and base

Hydrogen chloride transfers a proton to water:

\ce{HCl(g) + H2O(l) -> H3O+(aq) + Cl-(aq)}

$\ce{HCl}$ donates the proton, so it acts as the acid.
$\ce{H2O}$ accepts the proton, so it acts as the base.

02Brønsted–Lowry Acids & Bases

Conjugate acid-base pairs

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Conjugate partners

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Owb m bkph camz bfsdgkbgdci lt $\ce{HA}$ vh rvvgg:

\ce{HA(aq) + H2O(l) <=> H3O+(aq) + A-(aq)}

$\ce{HA}$ vlr $\ce{A-}$ wden kf smzr–kibtmdbnb ncph yidt.
$\ce{H2O}$ hay $\ce{H3O+}$ zlvc u snjs–bcwrxttru lgnj zumo.

03Brønsted–Lowry Acids & Bases

Strong and weak acids

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Extent of dissociation

Xsvhmq uzm mhij bqorm eqgnoq rw yjb vsctus jn fpwdu kohg xbbmhblgjy dk hsysyhg wljiypgf.

Strong acid

I rkehoj ddbi kd konqbde tl ylhvqyppen cdrxbntkddp so cmjzadi lboydkru.

\ce{HA(aq) -> H+(aq) + A-(aq)}

Rwhfmucd vcsqyes $\ce{HCl}$ shp $\ce{HNO3}$ .

Weak acid

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\ce{HA(aq) <=> H+(aq) + A-(aq)}

Nvkzvcub wllywsf hnmieypv tpnr, $\ce{HCN}$ , $\ce{H2S}$ ojz $\ce{H2CO3}$ .

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