What is the pH of the buffer solution that contains 2.2 g of NH4Cl in 250...

What is the pH of the buffer solution that contains 2.2 g of NH4Cl in 250 mL of 0.12 NH3? Is the final pH lower than the pH of the 0.12 M ammonia solution?

Expert Solution

Calculate the concentration of NH4Cl in 250 ml solution ={2.2g *1000}/{53.5 *250} = 0.165 M

According to Henderson equation pOH = -logKb +log[conju.acid] / [base]

where Kb of ammonia solution = 1.8*10^-5

pOH = - log (1.8*10^-5 ) + log [0.165] /[0.12]

= 4.7448 + 0.1409= 4.88

∴pH = 14 - pOH

= 14 - 4.88

= 9.12

The pH of the solution at initial concentration pOH =√Kb * C

= √1.8*10^-5 * 0.12

= 1.469*10^-2

∴ pH = 14 -0.01469 = 13.985

Hence the final pH is lower than the original pH of the ammonia solution

queen_honey_blossom answered 1 year ago

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