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
Assuming complete dissociation, calculate the pH of the following solution:
0.005 M NaOH
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
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 in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Which complex among the following gives a white precipitate on treatment with an aqueous solution of barium chloride?
Aqueous solution of ____________ will turn red litmus blue.
The least basic hydroxide from the following is:
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.
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
Assertion (A): Increasing order of acidity of hydrogen halides is \[\ce{HF < HCl < HBr < HI}\]
Reason (R): While comparing acids formed by the elements belonging to the same group of periodic table, \[\ce{H - A}\] bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
Define pOH.
Derive a relationship between pH and pOH.
Define pH.
Derive the relation pH + pOH = 14.
