Question
Asked Jul 13, 2019

what mass of insulin must be dissolved in 100.0mL of water to produce a solution with an oosmotic pressure of 16.8 mmHg at 25 degrees centigrade? 

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Step 1

The osmotic pressure is one of the colligative properties of solutions which has influence on solute concentration present in it.

The formula used to calculate the osmotic pressure is shown as below,

II MRT
|here, II Osmotic pressure in atm
M Molarity
R Gasconstant in L.atm/K.mol
T Temperature in K
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II MRT |here, II Osmotic pressure in atm M Molarity R Gasconstant in L.atm/K.mol T Temperature in K

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Step 2

Using above formula first the Molarity of solution is determined as follows,

Given
II 16.8mm Hg
R 0.08206L atm/K mol
T 25°C
II MRT
П
M
RT
16.8mm Hg
Kmol
1
760mm Hg/atm 0.08206L atm^25+273.15K
9.035x104M
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Given II 16.8mm Hg R 0.08206L atm/K mol T 25°C II MRT П M RT 16.8mm Hg Kmol 1 760mm Hg/atm 0.08206L atm^25+273.15K 9.035x104M

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Step 3

The molarity is defined as moles of solute present in one liter of solution. Hence, the obtained molarity is...

Number of moles of solute
Molarity (M)Volume of solution in liter
Number of molesof solute Molarity (M)x Volume of solution in liter
=9.035x10 mol/L x100x10L
9.035x10 moles
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Number of moles of solute Molarity (M)Volume of solution in liter Number of molesof solute Molarity (M)x Volume of solution in liter =9.035x10 mol/L x100x10L 9.035x10 moles

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