A nonelectrolyte compound is found to have a molar mass of...

A nonelectrolyte compound is found to have a molar mass of 598 g/mol. If 33.7 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C, what is the osmotic pressure (in torr) of the resulting solution? (Note: Report your answer to three significant digits and only input the number in the answer box.)

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Transcript

00:03 Here in this problem, given 33 .7 milligram of a non -electolite is dissolved in enough water to make 175 milliliters solution at 25 degrees celsius.

00:16 We have to find the osmotic pressure in turn.

00:20 Now, we have the mass of the non -electolite.

00:24 So, let's write that 33 .7 milligram.

00:29 And let's convert it into gram.

00:32 So 33 .7 times 10 to the power negative 3 gram.

00:38 Since 1 milligram is 10 to the power negative 3 gram.

00:44 So we have the mass of the solute in gram.

00:48 Now let's find out moles of salute.

00:52 Moles of salute is here is the mass 33 .7 times 10 to the bar negative 3 .3 .7 times 10 to the gram divided by its molar mass which is given here 598 gram per mole so write 598 gram per mole and we get 0 .0635 times 10 to the power negative 3 modes now the now we have 175 milliliter solution.

01:40 So, volume of solution is 175 milliliter.

01:50 Let's convert it into liter by multiplying with 10 to the per negative 3.

01:56 Since 1 milliliter is 10 to the power negative 3 later.

02:01 Now we have moles of solute, we have volume of solution in litre.

02:06 So we can find out the molar concentration.

02:10 So, molarity is most absolute divided by volume of solution in liter.

02:19 Let's like this one, 175...