Question

the osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant ( r ). suppose the osmotic pressure of a certain solution is measured to be 17. atm at an absolute temperature of 395. k. write an equation that will let you calculate the molarity ( c ) of this solution. your equation should contain only symbols. be sure you define each symbol other than ( r ).

your equation:
( c = square )

definitions of your symbols:
( square = 17. ) atm
( square = 395. ) k

Explanation:

Step1: Recall osmotic pressure formula

The osmotic pressure ($\Pi$) formula is $\Pi = cRT$, where $\Pi$ is osmotic pressure, $c$ is molarity, $R$ is gas constant, $T$ is absolute temperature.

Step2: Solve for molarity $c$

Rearrange the formula to solve for $c$: $c=\frac{\Pi}{RT}$

Step3: Define symbols

• $\Pi$: osmotic pressure (17. atm)
• $T$: absolute temperature (395. K)
• $c$: molarity (to find)
• $R$: gas constant (not defined here as per problem)

Step4: Substitute values (for calculation part)

Given $\Pi = 17.$ atm, $T = 395.$ K, $R$ (gas constant, e.g., $R = 0.0821\ \frac{\text{L·atm}}{\text{mol·K}}$ for these units). Then $c=\frac{17.}{R\times395.}$

Answer:

Your equation: $c=\frac{\Pi}{RT}$
Definitions of your symbols:

• $\Pi$: osmotic pressure (17. atm)
• $T$: absolute temperature (395. K)
• $c$: molarity of the solution

(For numerical value, if $R = 0.0821\ \frac{\text{L·atm}}{\text{mol·K}}$, then $c=\frac{17.}{0.0821\times395.}\approx0.52\ \text{mol/L}$ (but the problem first asks for the equation and symbol definitions))