Advertisements
Advertisements
Question
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Advertisements
Solution
Given: [OH–] = `2.87 xx 10^-4` M
To find: pH of the solution
Formulae:
i. pOH = –log10[OH–]
ii. pH + pOH = 14
Calculation:
From formula (i),
pOH = –log10[OH–]
∴ pOH = –log10[2.87 × 10–4]
= –log102.87 – log1010–4
∴ –log102.87 + 4 = 4 – 0.4579
pOH = 3.5421
From formula (ii),
pH + pOH = 14
pH = 14 – pOH
= 14 – 3.5421
= 10.4579
pH of the solution is 10.4579
RELATED QUESTIONS
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 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
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 0.1M H2SO4 + 10 mL of 0.1M KOH
Which of the following solution will have a pH value equal to 1.0?
Answer the following in brief :
The pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation constant.
Define pH.
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:
The pH of 0.001 M HCl solution is ______.
The pH of 10−5 M KOH solution will be ____________.
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.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
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?
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 ______.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Define pOH.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Derive the relation pH + pOH = 14.
Define the following term:
pOH
