NaOH is a strong base. What will be the pH of 5.0×10−2MNaOH solution?
(log2=0.3)
14.00
13.70
12.70
13.00
A
12.70
B
14.00
C
13.00
D
13.70
Open in App
Solution
Verified by Toppr
Given that, 5.0×10−2MNaOH≡[OH−]=5×10−2M
[H+][OH−]=1×10−14
[H+]×5×10−2=1×10−14
[H+]=1×10−145×10−2=2×10−13
pH=−log[H+]=−log(2×10−13)
=12.69≈12.70.
Option D is correct.
Was this answer helpful?
4
Similar Questions
Q1
NaOH is a strong base. What will be the pH of 5.0×10−2MNaOH solution?
(log2=0.3)
View Solution
Q2
The pH of a M10 solution of a weak base, if its Kb value at 25oCis2.5×10−4, will be: [log2=0.3]
View Solution
Q3
What will be the resultant pH when 150 mL of an aqueous solution of HCl(pH=2.0) is mixed with 350 mL of an aqueous solution of NaOH(pH=12.0)?
Take log(2)=0.3
View Solution
Q4
10 mL of a strong acid solution of pH = 2.000 is mixed with 990 mL of another strong acid solution of pH = 4.000. What will be the pH of the resulting solution?
log1.99=0.3
View Solution
Q5
pH of a solution of a strong acid is 5.0. What will be the pH of the solution obtained by diluting the given solution 100 times?