Reactivity 3.1 - Proton Transfer Reactions Flashcards
State the Arrhenius theory of acids and bases
acids have H+ in their chemical formula;
bases have OH- in their chemical formula
What is a Bronsted-Lowry acid
A proton (H+) donor
What is a Bronsted-Lowry base
A proton (H+) acceptor
State what conjugate bases and acids differ by
A proton
What are Amphiprotic substances
A species that can act as both a Bronsted-Lowry bas and acid such as water.
What are acid-base indicators
Acid-base indicators change color reversibly according to the concentration of H+ ions in the solution.
Describe the indication of litmus
Can distinguish between acids and alkalis but cannot indicate a particular pH.
How is the universal indicator made.
By mixing together several indicators .
State the colors in acids and bases of: Litmus, Methyl Orange, Phenolphthalein
What does the reaction between an acid and a base result in?
Salt and Water
What does the reaction between an acid and a metal result in?
Salt and Hydrogen
What does the reaction between an acid and a carbonate result in?
Salt and Water and Carbon Dioxide
Where does the equilibrium lie in this reaction with a strong acid?
Equilibrium lies to the right (towards the ions)
Where does the equilibrium lie in this reaction with a weak acid?
Equilibrium lies to the left (towards the undissociated form)
List three strong acids
List three strong bases
List two weak acids
List a weak base
List three experimental methods of distinguishing between strong and weak acids and bases.
- Electrical conductivity - Strong acids and bases will have a higher conductivity (higher concentration of mobile ions)
- Rate of reaction - Faster rate of reaction with strong acids (higher concentration of ions)
- pH - gives a number 0-14 for the acidity or alkalinity
what is H+ here
Number of moles of H+
State the ion product constant of water
State the relationship between pH and pOH scales
State the concept of strong acids and bases
Strong acids and bases completely dissociate in water.
State the concept of weak acids and bases
Weak acids and bases partially dissociate in water.
