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For each [OH?], determine the pH and state whether the solution is acidic or basic.(a)
Chapter 14, Problem 100P(choose chapter or problem)
Problem 100P
For each [OH−], determine the pH and state whether the solution is acidic or basic.
(a) [OH−] = 1.8 × 10−5 M
(b) [OH−] = 8.9 × 10−12 M
(c) [OH−] = 3.1 × 10−2 M
(d) [OH−] = 1.96 × 10−9 M
Questions & Answers
QUESTION:
Problem 100P
For each [OH−], determine the pH and state whether the solution is acidic or basic.
(a) [OH−] = 1.8 × 10−5 M
(b) [OH−] = 8.9 × 10−12 M
(c) [OH−] = 3.1 × 10−2 M
(d) [OH−] = 1.96 × 10−9 M
ANSWER:
Solution: Here, we are going to determine the pH of the given solutions.
Step1:
pH is the negative logarithm to base 10 of hydrogen ion concentration whereas pOH is the negative logarithm to base 10 of hydroxyl ion concentration, i.e.,
pOH = - log[OH- ] and pH = - log[H+ ]
And pH + pOH =14
We can distinguish acidic, neutral and basic aqueous solutions by the relative values of their pH
Acidic: pH < 7
Neutral: pH = 7
Basic: pH > 7
Step2:
- Given, [OH- ] = 1.8 x 10-5 M
Therefore pOH = - log[OH- ]
= - log (1.8 x 10-5)
= - log 1.8 - log 10-5
= -0.255 + 5
= 4.745