Advertisements
Advertisements
प्रश्न
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pKa of bromoacetic acid.
Advertisements
उत्तर
Degree of ionization, α = 0.132
Concentration, c = 0.1 M
Thus, the concentration of H3O+ = c.α
= 0.1 × 0.132
= 0.0132
`"pH" = - log["H"^+]`
`=- log(0.0132)`
= 1.879 : 1.88
Now
`"K"_"a" = "C" alpha^2`
`= 0.1 xx (0.132)^2`
`"K"_"a" = .0017`
`"pK"_"a" = 2.75`
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 KOH
Calculate the pH of the following solution:
2 g of TlOH dissolved in water to give 2 litre of solution.
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
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.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Derive the relation pH + pOH = 14.
Calculate the pH and pOH of 0.0001 M HCl solution.
Define pOH.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
What is the pH of 0.01 M solution of ammonium hydroxide which is 10% dissociated?
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 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 0.04 M HNO3 solution.
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?
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Calculate the pH of a buffer solution containing 0.1 M CH3COOH and 0.05 M CH3COONa. Dissociation constant of CH3COOH is 1.8 × 10-5 at 25°C.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Derive a relationship between pH and pOH.
