Advertisements
Advertisements
प्रश्न
Derive the relationship between pH and pOH.
उत्तर
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
संबंधित प्रश्न
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
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.
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 following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pKa of bromoacetic acid.
Derive the relation pH + pOH = 14.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Define pOH.
Derive the equation pH + pOH = 14.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Which complex among the following gives a white precipitate on treatment with an aqueous solution of barium chloride?
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
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.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
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 the relationship between pH and pOH.
Derive relationship between pH and pOH.
Define pOH.
Define pH.
Derive the relation pH + pOH = 14.
