Calculate the pH of the solution that results from the addition of 0.040 moles of HNO3 to a buffer made by?

Question

Calculate the pH of the solution that results from the addition of 0.040 moles of HNO3 to a buffer made by combining
0.500 L of 0.080 M NH4Cl ( use Ka = 5.60 x 10 -10 )
and 0.500 L of 0.160 M

Answer 1

I don't think you quite finished typing your question.

When you add HNO3 to the buffer solution, the number of moles of the acid (NH4+) will increase by the amount of HNO3 added, and the moles of the base (NH3, I'm guessing) will decrease by the same amount.

So, start by calculating the initial moles of NH4+ and NH3 present in your initial buffer solution from their individual molarities and volumes. Then, decrease the moles of NH3 by 0.040 and increase the moles of NH4+ by the same amount.

Finally, use the expression for Ka to calculate the [H+] in the solution under those conditions, and then convert [H+] to pH.

Hope this helps...

Answer 2

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Answer 3

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Answer 4

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