Advertisements
Advertisements
प्रश्न
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.
Advertisements
उत्तर
Given:
pH = 3.2
Concentration Dissociation = 0.02 M
Dissociation constant (Ka) = ?
Calculation:
Ka = `(Calpha^2)/(1 - alpha)`
`alpha = {[H^+]}/C`
pH = −log10[H+]
3.2 = −log10[H+]
−3.2 = log10[H+]
`10^-3.2 = [H^+]`
`6.3 xx 10^-4 = [H^+]`
`alpha = {[H^+]}/C`
= `(6.3 xx 10^-4)/0.02`
= 0.0315
Ka = `(Calpha^2)/(1 - alpha)`
`(0.02 xx (0.0315)^2)/(1 - 0.0315)`
= `(0.02 xx 0.000992)/0.9685`
= `(0.02 xx 9.92 xx 10^-4)/(1)`
= `0.1984 xx 10^-4`
APPEARS IN
संबंधित प्रश्न
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH?
Calculate the pH of the following solution:
2 g of TlOH dissolved in water to give 2 litre of solution.
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Calculate the pH and pOH of 0.0001 M HCl solution.
Select the INCORRECT relation.
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 ____________.
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?
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
The pH of 10−5 M KOH solution will be ____________.
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.
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Derive the relationship between pH and pOH.
Neutral solutions have the pH of ______.
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 pOH.
Define pH.
Define pH.
Define pOH.
Derive the relation pH + pOH = 14.
Define pH.
Derive the relation pH + pOH = 14.
Define pH.
