3.1.12.1 Bransted-Lowry acid-base equilibria in aqueous solution Flashcards
What are the properties of acids?
They form solutions in water below pH 7
They donate H+ ions to bases (proton donors)
What are the properties of bases?
They’re proton acceptors
They take H+ ions from acids
What is an alkali?
It is a soluble base
They form solutions with a pH above 7
They dissolve in water to produce OH- ions
What happens in a neutralisation reaction?
A base reacts with acid to form a salt and water
What is the Bronsted Lowry theory?
An acid is a substance which can donate a proton
A base is a substance which can accept a proton
What does the term conjugate mean?
The linking of an acid and a base by the transferring of a proton
What would happen if you replace water as the solvent in an acidic or alkaline solution?
It would not show any of the characteristic acidic properties
What is the difference between an acid of pH 1 or 5?
pH 1: fully dissociates, high concentration of H+ ions
pH 5: partly dissociate, low concentration of H+ ions
What does amphoteric mean?
Acid and base properties
What does monobasic or monoprotic mean?
There is one proton to donate
What does diprotic or triprotic mean?
Two or three protons to donate
How does an acid react with a metal?
Acid + metal = salt + hydrogen
How does an acid react with a metal oxide?
Acid + metal oxide = salt + water
How does an acid react with a metal hydroxide?
Acid + metal hydroxides = salt + water
How does an acid react with a metal carbonate?
Acid + metal carbonates = salt + carbon dioxide + water
