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
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH?
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Derive the relation pH + pOH = 14.
The pH of 0.001 M NaOH(aq) solution will be:
The pH of 0.001 M HCl 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?
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Calculate the pH of 0.04 M HNO3 solution.
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.
Define pH.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Derive a relationship between pH and pOH.
Define pOH.
Derive relationship between pH and pOH.
Define pOH.
Derive the relation pH + pOH = 14.
Define the following term:
pOH
