Ionic Equilibria (Exercise)

Ionic Equilibria (I) [H + ] = [HA] pH = - log [HA] [OH - ] = [B] pOH = - log [B] Strong Acid Strong Base Weak Acid Weak Base [H + ] < [HA] [H + ] = K a [HA] pH = - log [H + ] pOH = - log [OH - ] [OH - ] < [B] [OH - ] = K b [B]

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],Question 5 [H + ] = K a [HA] [OH – ] = degree of ionisation × [B] [H + ] = % ionisation × [HA] [OH – ] = K b [B]

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],[object Object],Question 6

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],Question 6

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],Question 6 [OH – ] = K b [salt]

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],Question 6

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],Question 12 Fe(OH) 2 Mg(OH) 2

Electrochemistry ,[object Object],[object Object],[object Object],Question 12 Fe(OH) 2 Mg(OH) 2

Electrochemistry ,[object Object],[object Object],[object Object],[object Object],[object Object],Question 12 Fe(OH) 2 Mg(OH) 2

Ionic Equilibria (Exercise)

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Ionic Equilibria (Exercise)