Advertisements
Advertisements
Question
Derive the relationship between pH and pOH.
Advertisements
Solution
The ionic product of water is
KW = \[\ce{[H3O+][OH–]}\]
Now, KW = 1 × 10−14 at 298 K and thus
\[\ce{[H3O+][OH–]}\] = 1 × 10−14
Taking logarithm of both sides,
\[\ce{log10[H3O+] + log10[OH–]}\] = −14
Multiply the entire equation by '−1'
\[\ce{(-log10[H3O+]) + (-log10[OH–])}\] = 14
Now pH = \[\ce{- log10[H3O+]}\] and pOH = \[\ce{- log10[OH–]}\]
∴ pH + pOH = 14
RELATED QUESTIONS
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Which of the following solution will have a pH value equal to 1.0?
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Answer the following :
The pH of rainwater collected in a certain region of Maharashtra on a particular day was 5.1. Calculate the H+ ion concentration of the rainwater and its percent dissociation.
Calculate the pOH of 10-8 M of HCl.
Which of the following is INCORRECT statement?
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Select the INCORRECT relation.
Aqueous solution of ____________ will turn red litmus blue.
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 ____________.
Equal volumes of three acid solutions of pH 1, 2 and 3 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
Calculate the pH of a buffer solution containing 0.1 M CH3COOH and 0.05 M CH3COONa. Dissociation constant of CH3COOH is 1.8 × 10-5 at 25°C.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Define pOH.
Derive relationship between pH and pOH.
Define pOH.
Define pOH.
Derive a relationship between pH and pOH.
Derive relationship between pH and pOH.
Derive relationship between pH and pOH.
Define pH.
Define pH.
Define pOH.
Define the following term:
pOH
