Advertisements
Advertisements
प्रश्न
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.
Advertisements
उत्तर
c = 0.1M
pH = 2.34
−log[H+] = pH
−log[H+] = 2.34
[H+] = 4.5 × 10−3
Also,
[H+] = cα
4.5 × 10−3 = 0.1 × α
`(4.5 xx 10^(-3))/0.1` = α
α = 4.5 × 10−3 = 0.045
Then,
Ka = cα2
= 0.1 × (45 × 10−3)2
= 202.5 × 10−6
= 2.02 × 10−4
APPEARS IN
संबंधित प्रश्न
Assuming complete dissociation, calculate the pH of the following solution:
0.005 M NaOH
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
Which of the following solution will have a pH value equal to 1.0?
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
Answer the following :
The pH of rainwater collected in a certain region of Maharashtra on a particular day was 5.1. Calculate the H+ ion concentration of the rainwater and its percent dissociation.
Which of the following is INCORRECT statement?
The pH of 0.001 M NaOH(aq) solution will be:
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 solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of \[\ce{NH^+_4}\] is 0.20 M. If the equilibrium constant, Kb tor NH3 equals 1.8 × 10-5, what is the pH of the solution?
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
The mole fraction of the solute molal aqueous solution is:
Define pOH.
Define pH.
Derive the relation pH + pOH = 14.
Derive the relation pH + pOH = 14.
Define pH.
Derive the relation pH + pOH = 14.
Which from the following compound in aqueous medium having minimum pH?
