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.
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?
The solubility of Sr(OH)2 at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution.
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.
Derive the relation pH + pOH = 14.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
The CORRECT match between transition metal ion and its colour in aqueous solution.
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?
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.
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?
A lab assistant prepared a solution by adding a calculated quantity of HCl gas at 25°C to get a solution with [H3O+]= 4 × 10−5 M. Is the solution neutral (or) acidic (or) basic.
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
In which of the following solvents is silver chloride most soluble?
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 ______.
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
Derive the relationship between pH and pOH.
Define pOH.
Define pOH.
Define pH.
Define pH.
Define pH.
Define pOH.
Define the following term:
pH
