What is the pH of the solution that results from adding 26.2 mL of 0.14 M...

What is the pH of the solution that results from adding 26.2 mL of 0.14 M to 25.9 mL of 0.41 MNH3? (Ka for ammonium ion is 5.6*10^-10).

pH-------------------?

Expert Solution

What is the pH of the solution that results from adding 26.2 mL of 0.14 M HCl to 25.9 mL of 0.41 MNH3?
(Ka for ammonium ion is 5.6*10^-10).

pH-------------------?

moles of HCl ---> (0.14 mol/L) (0.0262 L) = 0.003668 mol
moles NH3 ---> (0.41 mol/L) (0.0259 L) = 0.010619 mol

The HCl and NH3 react in a 1:1 molar ratio and all the HCl is used up.

moles NH3 remaining ---> 0.010619 mol - 0.003668 mol = 0.006951 mol
moles NH4^+ produced ---> 0.003668 mol

the henderson-Hasselbalch equation:

pH = pKa + log (base/acid)

pH = -log(5.6*10^-10) + log (0.006951 / 0.003668)

pH = 9.252 + 0.277 = 9.53

The pH of the resulting solution is 9.53

queen_honey_blossom answered 2 years ago

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