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Chemistry: Acids And Bases

Chemistry37 CardsCreated 2 months ago

This flashcard set outlines the Brønsted–Lowry theory, which defines acids and bases in terms of proton transfer. It explains that acids donate H⁺ ions and are classified as strong or weak based on how completely they dissociate in solution.

What does bronsted Lowry theory describe acids and bases in terms of

Protons

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Key Terms

Term
Definition

What does bronsted Lowry theory describe acids and bases in terms of

Protons

What does an acid-base reaction involve

Proton transfer

Acid

A substance that donates H+ ions

What are acids classified as strong or weak depending on

The extent of dissociation

Strong acid

Completely dissociates in solution

Weak acid

Partially dissociates in solution

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TermDefinition

What does bronsted Lowry theory describe acids and bases in terms of

Protons

What does an acid-base reaction involve

Proton transfer

Acid

A substance that donates H+ ions

What are acids classified as strong or weak depending on

The extent of dissociation

Strong acid

Completely dissociates in solution

Weak acid

Partially dissociates in solution

Base

A substance that accepts H+ ions

Alkali

A base that releases hydroxide ions in aqueous solution

What type of reaction is that of acids with metals

Redox

What is the role of H+ ions in the reaction of acids with metals

Oxidising agent

What are acid base equilibria

Reversible reactions involving the transfer of protons

pH

-log[H+]

What does a low pH mean

Larger concentration of H+ ions

What does a high pH mean

A small concentration of H+ ions

[H+]

10 ttp -pH

How many moles of H+ ions does one mole of a monoprotic acid donate

One mole

What do you assume in pH calculations for strong acids


Complete ionisation

What does it mean that for pH calculations of strong acids, you assume complete ionisation

[H+]=original conc of acid

Is sulfuric monoprotic

Diprotic

[H+]=2[HA]

What are a weak acids undissociated molecules in equilibrium with

It’s ions

Acid dissociation constant

Ka

Ka

Conc product/conc reactants

Units of Ka

Moldm-3

What is the value of Ka a quantitative measure of

The strength of a weak acid

What is the relationship between degree of dissociation and Ka value and why

Greater degree of dissociation, higher conc of H+ and larger Ka value

What is pKa sometimes used for

To compare the relative strengths of acids

pKa

-logKa

Relationship between Ka value and strength of acid

Higher Ka value = stronger acid

Relationship between pKa value and acid strength

Lower pKa value = stronger acid

Expression for ionisation of water

h20 > H+ + OH-

To what extent does pure water ionise to

A very small extent

What is Kw derived from

The equilibrium constant for the dissociation of water into H+ ions and OH-

Definition of Kw

[H+][OH]

What is Kw at 298K

1x10-14 mol2dm-6


Why is the dissociation of water an endothermic process

Energy is required to break bonds

Why does Kw increase when temperature increases

The equilibrium moves to the right

Assumptions to make to calculate the pH of a strong base

  • assume complete ionisation

| - assume Kw= 1x10-14