Bronsted-Lowry theory of acid and bases

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12 Terms

1
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What is a bronsted-lowry acid?

Acids are proton donors.

2
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What is a bronsted-lowry base?

Bases are proton acceptors.

3
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Acids dissociate according to what equilibrium?

HA(aq) ​⇌ H+ (aq) ​+ A− (aq)​

4
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What is a strong acid?

Strong acids completely dissociate (ionise) into their ions.

5
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What is a weak acid?

Weak acids partially dissociate (ionise) into their ions.

6
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What is a conjugate acid?

A species which has gained a proton.

  • Conjugate acids act as acids in the backwards reaction i.e. they donate a proton to return to the original base.

<p>A species which has gained a proton.</p><p></p><ul><li><p>Conjugate acids act as acids in the backwards reaction i.e. they donate a proton to return to the original base.</p></li></ul><p></p>
7
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What is a conjugate base?

A species which has lost a proton.

  • Conjugate bases act as bases in the backwards reaction i.e. they accept a proton to return to the original acid.

<p>A species which has lost a proton.</p><p></p><ul><li><p>Conjugate bases act as bases in the backwards reaction i.e. they accept a proton to return to the original acid.</p></li></ul><p></p>
8
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Identify the conjugate pairs in this reaction.

HCl and Cl- are a conjugate pair.

H2O and H3O+ are another conjugate pair.

<p>HCl and Cl<sup>-</sup> are a conjugate pair.</p><p>H<sub>2</sub>O and H<sub>3</sub>O<sup>+</sup> are another conjugate pair.</p>
9
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What is Ka?

The equilibrium constant for acids.

Ka= [H(aq)+​][A(aq)−​] / [HA(aq)​]

10
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What does the Ka value of a weak acid suggest?

The degree of dissociation- the higher the Ka, the stronger the acid.

11
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What is the ionic product of water?

Kw​=[H+][OH−]

Kw has a value of 1×10−14 mol2 dm−6 (at 298 K).

12
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What can be said about the concentration of H+ ions and OH- ions in pure water?

The concentrations are equal.