Question

500. ml of a solution containing 1. 5 m nh3(aq) is mixed with 500. ml of a solution containing 0. 50m of hcl(aq). what is the ph of the final solution? (kb(nh3) = 1. 8 x 10-5)

Answer 1

The pH of the solution is determined by the hydrogen ion concentration. The pH of the solution with 1.5 M ammonia and 0.50 M hydrochloric acid is 8.77.

What is pH?

The potential of the hydrogen ion in the solution is called pH which determines the basicity and acidity of the solution.  

Given,

The molar concentration of 500 mL ammonia = 1.5 M

The molar concentration of 500 mL hydrochloric acid = 0.50 M

Kb (NH₃) = 1. 8 x 10⁻⁵

First, pOH is calculated as,

pOH = pKb + log [NH₃][HCl]

= - log 1. 8 x 10⁻⁵ + log [1.5][0.50]

= - log 1. 8 x 10⁻⁵ + log [3]

= 4.744 + 0.477

= 5.221

Now, pH is calculated from pOH as,

pH = 14 - pOH

= 14 - 5.221

= 8.77

Therefore, 8.77 is the pH.

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