Advertisements
Advertisements
प्रश्न
The pH of 10−5 M KOH solution will be ____________.
पर्याय
9
5
19
none of these
Advertisements
उत्तर
The pH of 10−5 M KOH solution will be 9.
Explanation:
\[\ce{\underset{10^{-5} m}{KOH} -> \underset{10^{-5} m}{K^+} + \underset{10^{-5} m}{OH^-}}\]
[OH–] = 10−5 M
pH = 14 – pOH
pH = 14 – (– log [OH–])
= 14 + log [OH–]
= 14 + log 10−5
= 14 – 5
= 9
APPEARS IN
संबंधित प्रश्न
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pKa.
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Define pOH.
Define the following term:
pH
