Advertisements
Advertisements
प्रश्न
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
उत्तर
The concentration of OH ion in a water sample is found to be 2.5 × 10−6 M
pOH = – log10 [OH–]
pOH = – log10 [2.5 × 10−6]
= – log10 [2.5] – log10 [10−6]
= – 0.3979 – (– 6)
= – 0.3979 + 6
pOH = 5.6
We know that,
pH + pOH = 14
pH + 5.6 = 14
pH = 14 – 5.6
pH = 8.4
pH = 8.4, shows the nature of the solution is basic.
APPEARS IN
संबंधित प्रश्न
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
Answer the following in brief :
The pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation constant.
Select the INCORRECT relation.
An aqueous solution of which of the following will have a pH greater than 7?
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5NH) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10−9) is ____________.
Calculate the pH of 0.04 M HNO3 solution.
Define pH.
Derive relationship between pH and pOH.
Derive the relation pH + pOH = 14.
Define pOH.
