What is the pH of a solution containing NH3 and NH4Cl?

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SUMMARY

The pH of a solution containing 0.05 ml of NH3 and 0.27 g of NH4Cl can be calculated using the Kb value of NH4OH, which is 1.8 x 10^-5. The NH3 dissolves in water, reacting with H+ ions to form NH4+. This scenario represents a classical buffer system, where NH3 acts as a weak base and NH4Cl provides the conjugate acid. The resulting pH can be determined using the Henderson-Hasselbalch equation.

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0.05ml of NH3 is dissloved in a solution containing water followed by 0.27g of NH4Cl. If the Kb for NH4OH is 1.8 * 10^-5 find the pH value of the solution.
I am finding it difficult to predict the reactions that are going to happen here. I know to calculate Kh or the constant of hydrolysis of NH4Cl from here but how does NH3 dissolve in water. I think it mixes with H+ in the solution to form NH4+.
But I don't know how to continue.
 
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This is classical buffer question.

Compare with this buffer question - not identical, but close.
 

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