Question 18The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant. Suppose the osmotic pressure of a certain solution is measured to be at an absolute temperature of. Write an equation that will let you calculate the molarity of this solution. Your equation should contain only symbols. Be sure you define each symbol other than.

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Chemistry

Micheal Burton

2 May, 12:59

Question 18The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant. Suppose the osmotic pressure of a certain solution is measured to be at an absolute temperature of. Write an equation that will let you calculate the molarity of this solution. Your equation should contain only symbols. Be sure you define each symbol other than.

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Answers (1)

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Camryn Shepard · Answer 1

The given question is incomplete, the complete question is:

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 of a certain solution is measured to be 6.6 atm at an absolute temperature of 308. K. Write an equation that will let you calculate the molarity of this solution. Your equation should contain only symbols. Be sure you define each symbol other than R.

Answer:

The correct answer is 0.26 M.

Explanation:

The extra pressure, that is, presented upon the solution to inhibit the process of osmosis is termed as the osmotic pressure. The formula to use for the question is π = CRT.

In the given formula, C is the concentration, π is the osmotic pressure, T is the temperature, and R is the gas constant.

The values or R, T and π given in the question is 0.0821 atmLmol^-1K^-1, 308K and 6.6 atm.

By putting the values in the given equation we get:

6.6 atm = C * 0.0821 atmLmol^-1K^-1 * 308K

6.6 atm/25.3 Lmol^-1atm = C

C = 0.26 M

Hence, the molarity of the solution is 0.26M.