Saturated Solution Concentrations and Osmotic Pressure Calculations

[kateman]

There are 3 questions below with my working and answers, could someone please check that I am right, even if you can only give approval or correction on just one question and nothing else - anything would be appreciated. Please forgive my not following the template, as I didn't think it would work with checking correct answers. Thanks for any responces!

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Q1: A theoretical salt (X<sub>2Y3) (with Ksp= 6.26 x 10 ^-15 ) is in a saturated solution. What is its millimolar concentration (mM) of X?

A1: Ksp= [X]² [Y]³ = 6.26 x 10 ^-15

therefore concentration of Y = 3/2 concentration of X (or is it 2/3, iam not sure?)

therefore rewrite Y as [3/2 X]³

therefore Ksp= [X]²x 27/8 X³
= 27/8 [X]⁵

therefore, with rearranging, [M] = 1.131514468x10^-3 mol/L
= 1.131514468 mM/L

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Q2: A reaction at temperature of 287K gives a change in enthaply of -7KJ and a free energy change of -10kJ, what is the change in entropy for this reaction (in J/K)?

A2: \DeltaG = \DeltaH - T\DeltaS

with rearranging: \DeltaS = \DeltaH - \DeltaG / T
=(-7 - -10)/287 = 0.010452961 J/K

That doesn't seem right to me.

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Q3: If a 0.5 L solution at a temperature of 294.75 K contains 13.7g of an unknown solute (with a molecular mass of 60.094g), what is its osmotic pressure in atmospheres?

A3: since moles (n) = concentration (c)/ volume (v) = mass (m)/ molecular weight (M)

then C = m/Mv = 13.7 / (60.094x0.5) = 0.455952341 mol/L

Now use the values of C, T and the gas constant (8.314 J/mol K) into the osmotic pressure formula P=CRT

P= 0.455952341x8.314x294.75 = 1117.334694 Pa (am I right to say that its in pascals, or is it in killapascals [Kpa]?)

atmospheres = 101.325 Kpa = 101325 Pa

osmotic pressure (in atmospheres) = 1117.334694/101325 = 0.011027236 atms

This is something iam really not sure about, the answer seems almost wrong to me but iam not sure where I would have gone wrong in my working, can someone please help? It would be very much appreciated!

Thank you!</sub>

 

[Borek]

You use too many significant digits every time.

First looks OK.

Second and third - approach seems correct (even if in the second your formula misses parantheses), but second opinion won't hurt.

 

[kateman]

Thank you Borek, and I agree, I'd still appreciate at least another person's opinion on my working.