Advertisements
Advertisements
प्रश्न
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
पर्याय
1.585 × 10–3 mol dm–3
3.010 × 10–11 mol dm–3
3.010 × 10–3 mol dm–3
1.585 × 10–11 mol dm–3
Advertisements
उत्तर
The pH of a weak monoacidic base is 11.2, its OH– ion concentration is 1.585 × 10–3 mol dm–3.
Explanation:
pOH of the solution is given as:
pOH = 14 – pH
= 14 – 11.2
= 2.8
pOH = – log10[OH–]
log10[OH–] = – pOH
= – 2.8
= – 2 – 0.8 – 1 + 1
= – 3 + 0.2
= `overline(3)`.2
[OH–] = antilog `overline(3)`.2 = 1.585 × 10–3 mol/dm–3
APPEARS IN
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:
0.005 M NaOH
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.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
The pH of 0.001 M NaOH(aq) solution will be:
Which of the following when dissolved in water results in neutral solution?
Aqueous solution of ____________ will turn red litmus blue.
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?
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
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 ____________.
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.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
Derive the relationship between pH and pOH.
Neutral solutions have the pH of ______.
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.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Derive relationship between pH and pOH.
Define pH.
Define pOH.
Define pH.
Define pOH.
Define pOH.
