1.12 Acids And Bases
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What is the definition of an acid?
Proton donor
What is the definition of a base?
Proton acceptor
What is the definition of conjugate base?
Accepts a H+ to reform original acid
How is a conjugate acid formed?
When base accepts a proton
Definition of a strong acid?
Proton fully dissociates
What are the two chemical tests to distinguish between strong and weak acids?
Universal Indicator- Strong acids= lower pH Titration- Weaker acids will require less alkali to neutralise
What is the definition of pH?
pH=-log[H+]
How to calculate concentration from pH?
10^-pH
What is the equation for the dissociation of water?
H2O>< H+ + OH-
What is the expression for Kw?
Kw= [H+][OH-] Or Kw= [H+]^2
What happens to Kw of pure water as temperature increases?
• Kw becomes disproportional • More H+ ions dissociate • Kw Increases
Why is water at whatever pH still neutral?
Because OH- and H+ ions are equal
What is the definition of a buffer?
A solution which resists a small change of acid or alkali to maintain pH
What is the definition of pKa?
-log(Ka)
What indicator is suitable for a strong acid weak base reaction?
Methyl orange
Which indicator is suitable for weak acid strong base reaction and why?
• Phenolphthalein • End point of phenolphthalein is within vertical point of graph so colour will change as equillibrium of H+ ions and OH- ions shift
Why does the ph of pure water change with temperature?
• Ionisation of water is endothermic • When temp increases equilibrium shifts to right increasing concentration of ions