Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
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Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
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Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Calculate the pH of a 0.30 M solution of aniline(C6H5NH2 , Kb = 3.8 x 10-10.)


We are being asked to calculate the pH for a 0.30 M solution of C6H5NH2. 

C6H5NH2 is a neutral amine, therefore we know that it is a weak base.

Since we’re dealing with a weak base and Kb is an equilibrium expression we will have to create an ICE chart to determine the equilibrium concentration of each species:

C6H5NH2weak baseproton acceptor
H2O → will act as the weak acidproton donor

Equilibrium reaction:        C6H5NH2(aq) + H2O(l)  C6H5NH3+(aq)(aq) + OH-(aq)

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