Chemistry: Acids And Bases
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
Key Terms
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
Related Flashcard Decks
Study Tips
- Press F to enter focus mode for distraction-free studying
- Review cards regularly to improve retention
- Try to recall the answer before flipping the card
- Share this deck with friends to study together
| 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 |
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 |
|
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 Kw= 1x10-14 |