A buffer solution contains 1.00 M NH3 (Kb = 1.8  10-5 ) and 2.00 M...

A buffer solution contains 1.00 M NH3 (Kb = 1.8  10-5 ) and 2.00 M NH4Cl. (a) Write the net ionic equations to show how this buffer solution neutralizes the added H + and OH- . (b) Calculate the pH of this buffer solution.

Solutions

Expert Solution

Given the mixture of basic buffer.

It is (NH3+ NH4Cl).Mixture of weak base and a salt containing its conjugate acid.

a) When an acid is added for example HCl,then it reacts with the base and the equation is as follows:

NH3 (aq) + HCl(aq) ----------------> NH4Cl(aq)

net ionic equation is: H3O+ (aq) + NH3 (aq) ---------------> H2O(l) + NH4+ (aq)

when a base is added, for example NaOH ,it reacts with the salt and the equtaion is as shown below:

NH4Cl (aq) + NaOH (aq) ------------> NaCl(aq) + H2O(l) + NH3 (aq)

net ionic equation is: NH4+ (aq) + OH- (aq) -------------> NH3 (aq) + H2O(l)

b) pH of a buffer solution can be obtained by using Handerson Hesselbalch equation.

pH = 14 - pOH

= 14 - [pKb + log[salt]/[base]]

= 14 - [-log (1.8x10^-5) + log (2/1)]

= 8.95

queen_honey_blossom answered 1 year ago

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