Sea water is 3.5 % by mass of common salt and has a density 1.04 g cm-3 at 293 K. Assuming the salt to be sodium chloride, then osmotic pressure of sea water will be (assume complete ionisation of the salt)

Question

Sea water is 3.5 % by mass of common salt and has a density 1.04 g cm-3 at 293 K. Assuming the salt to be sodium chloride, then osmotic pressure of sea water will be (assume complete ionisation of the salt) (A) 25.45 atm (B) 11.56 atm (C) 29.98 atm (D) 30.20 atm

Tardigrade Admin · Accepted Answer

Let mass of solution be 100 g. Volume of solution = (Mass/Density) = (100/1.04) = 96.154 mL = 0.096 L wB = 3.5 g MB = 58.5 g mol-1 (molar mass of NaCl) For complete ionisation of NaCl, vanât Hoff factor will be '2'. i = 2 we know, π = iCRT = i (n/V)RT = 2 × (3.5 × 0.0821 × 293/58.7 × 0.096) = 29.98 atm

Q. Sea water is $3.5%$ by mass of common salt and has a density $1.04 g c m^{- 3}$ at $293 K$ . Assuming the salt to be sodium chloride, then osmotic pressure of sea water will be (assume complete ionisation of the salt)

$25.45 a t m$

$11.56 a t m$

$29.98 a t m$

$30.20 a t m$

Q. Sea water is 3.5% by mass of common salt and has a density 1.04gcm−3 at 293K. Assuming the salt to be sodium chloride, then osmotic pressure of sea water will be (assume complete ionisation of the salt)

25.45atm

11.56atm

29.98atm

30.20atm

Let mass of solution be 100g. Volume of solution =DensityMass​=1.04100​ =96.154mL=0.096L wB​=3.5g MB​=58.5gmol−1 (molar mass of NaCl) For complete ionisation of NaCl, van’t Hoff factor will be ′2′. i=2 we know, π=iCRT=iVn​RT =2×58.7×0.0963.5×0.0821×293​=29.98atm

Q. Sea water is $3.5%$ by mass of common salt and has a density $1.04 g c m^{- 3}$ at $293 K$ . Assuming the salt to be sodium chloride, then osmotic pressure of sea water will be (assume complete ionisation of the salt)

$25.45 a t m$

$11.56 a t m$

$29.98 a t m$

$30.20 a t m$