Advertisements
Advertisements
प्रश्न
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
उत्तर
c = 0.005
pH = 9.95
pOH = 4.05
pH = – log (4.105)
`4.05 = -log["OH"^-]`
`["OH"^-] = 8.91 xx 10^(-5)`
`"c" alpha = 8.91 xx 10^(-5)`
`alpha = (8.91 xx 10^(-5))/(5xx10^(-3)) = 1.782 xx 10^(-2)`
Thus `"K"_"b" = "c" alpha^2`
`= 0.005 xx (1.782)^2 xx 10^(-4)`
`= 0.005 xx 3.1755 xx 10^(-4)`
`= 0.0158 xx 10^(-4)`
`"K"_"b" = 1.58 xx 10^(-6)`
`"Pk"_"b" = - log "K"_"b"`
`= - log (1.58 xx 10^(-6))`
= 5.80
APPEARS IN
संबंधित प्रश्न
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 0.2M Ca(OH)2 + 25 mL of 0.1M HCl.
Choose the most correct answer:
The pH of 10-8 M of HCl is ______.
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.
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.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Calculate the pOH of 10-8 M of HCl.
Calculate the pH and pOH of 0.0001 M HCl solution.
Which of the following is INCORRECT statement?
Among the following, the CORRECT increasing order of acidity:
The number of ions given by Na3[Fe(CN)6] in aqueous 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?
Derive relationship between pH and pOH.
Define pOH.
Derive the relation pH + pOH = 14.
Define pOH.
Define pH.
Derive the relation pH + pOH = 14.
Define pOH.
