Problem 80P
Determine the pOH of each solution and classify it as acidic, basic, or neutral.
(a) [OH−] = 4.5 × 10−2 M
(b) [OH−] = 3.1 × 10−12 M
(c) [OH−] = 5.4 × 10−5 M
(d) [OH−] = 1.2 × 10−2 M
Step-by-Step Solution:
Solution 80P:
Here, we are going to calculate the pOH of each solution and identify whether the reaction is acidic, basic and neutral.
We know, the ion product constant Kw for water is
Kw =[H3O+][OH-] = 1x10-14
pH + pOH =14
And pOH = - log[OH- ] and pH = - log[H+ ]
(a) [OH−] = 4.5 × 10−2 M
Step 1: We know,
pOH = - log[OH- ]
= -log(4.5 × 10−2 )
= 2 -log4.5
= 2 -0.653
=1.35
The pOH of the solution is 1.35
Step 2 of 3
Chapter 14, Problem 80P is Solved
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Step 3 of 3
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