Advertisements
Advertisements
प्रश्न
Derive the equation pH + pOH = 14.
Advertisements
उत्तर
The ionic product of water is given as:
Kw = [H3O+][OH–]
Now, Kw = 1 × 10–14 at 298 K
Thus, [H3O+][OH–] = 1.0 × 10–14
Taking logarithm of both the sides, we write
log10[H3O+] + log10[OH–] = –14
–log10[H3O+] + {– log10[OH–]} = 14
Now, pH = –log10[H3O+] and pOH = –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.
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
Calculate the pH of the resultant mixtures: 10 mL of 0.2M Ca(OH)2 + 25 mL of 0.1M HCl.
Which of the following solution will have a pH value equal to 1.0?
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Calculate the pOH of 10-8 M of HCl.
Which complex among the following gives a white precipitate on treatment with an aqueous solution of barium chloride?
The pH of 0.001 M NaOH(aq) solution will be:
Among the following, the CORRECT increasing order of acidity:
The least basic hydroxide from the following is:
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
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?
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
A sample of air turns lime water milky and also turns acidified potassium dichromate green in aqueous solution has low pH. This is due to the presence of pollutants.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
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.
Define pOH.
The mole fraction of the solute molal aqueous solution is:
Define pH.
Define pOH.
Define pH.
Define the following term:
pH
