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
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 KOH
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
The pH of milk, black coffee, tomato juice, lemon juice and egg white are 6.8, 5.0, 4.2, 2.2 and 7.8 respectively. Calculate corresponding hydrogen ion concentration in each.
If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its pH?
Calculate the pH of the resultant mixtures: 10 mL of 0.2M Ca(OH)2 + 25 mL of 0.1M HCl.
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Define pH.
Calculate the pOH of 10-8 M of HCl.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
An aqueous solution of which of the following will have a pH greater than 7?
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?
The pH of an aqueous solution is Zero. The solution is ____________.
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
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?
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Define pH.
