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Question
17.4% (w/v) K2SO4 solution at 27°C is isotonic with 5.85% (w/v) NaCl solution at 27°C. If NaCl is 100% ionized, what is the % ionization of K2SO4 in aq. solution?
17.4% (w/v) K2SO4 solution at 27°C is isotonic with 5.85% (w/v) NaCl solution at 27°C. If NaCl is 100% ionized, what is the % ionization of K2SO4 in aq. solution?
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Solution
Isotonic solutions have same osmotic pressure.
Osmotic pressure (p) =icRT
Since solutions are isotonic,
(ic)NaCl = (ic)K2SO4
For NaCl, i=2,
since it dissociates 100%.
c for NaCl = 5.85
c for K2SO4 = 17.84
Substiuting the values we get i= 0.655
i.e K2SO4 is 65.5% ionised
Osmotic pressure (p) =icRT
Since solutions are isotonic,
(ic)NaCl = (ic)K2SO4
For NaCl, i=2,
since it dissociates 100%.
c for NaCl = 5.85
c for K2SO4 = 17.84
Substiuting the values we get i= 0.655
i.e K2SO4 is 65.5% ionised
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