$$0.08206 \ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K}$$

$$0.015 \times 299.15 = 4.487$$ mol \cdot K / L

$$\frac{273.15 \ \text{mg}}{1000 \ \text{mg/g}} = 0.27315 \ \text{g}$$; $$M = \frac{0.27315}{81.389} = 0.00336$$ mol/L

Question 1

Which of the following best describes the process of osmosis in biological systems?

Accepted Answer

Movement of water from lower to higher concentration across a membrane.

Question 2

Which two factors directly influence the osmotic pressure of a solution according to the study materials?

Accepted Answer

Concentration and temperature

Question 3

Given the osmotic pressure formula $$\Pi = iMRT$$, what does the variable $$i$$ represent?

Accepted Answer

Van't Hoff factor, representing the number of particles the solute dissociates into

Question 4

A solution contains 18.30 mg of ZnO in 15.1 mL of solution at 26°C. What is the first step to calculate its molarity?

Accepted Answer

Convert the mass of ZnO to moles using its molar mass.

Question 5

If the osmotic pressure of blood is 5950.8 mmHg at 41°C, what is the equivalent pressure in atm? (1 atm = 760 mmHg)

Accepted Answer

$$\frac{5950.8}{760} = 7.83$$ atm

Question 6

Which of the following is the correct value for the gas constant $$R$$ used in the osmotic pressure formula?

Accepted Answer

$$0.08206 \ 	ext{L} \cdot 	ext{atm} / 	ext{mol} \cdot 	ext{K}$$

Question 7

A solution is prepared by dissolving 7.0 g of insulin per liter at 25°C. If the osmotic pressure is 3,059 mmHg, what is the osmotic pressure in atm?

Accepted Answer

$$\frac{3059}{760} = 4.03$$ atm

Question 8

Which of the following best explains why glucose (C$$_6H$_{12}O$_6) is $$used to match the osmotic pressure of blood in medical solutions?

Accepted Answer

Glucose is non-ionic and does not dissociate, so its Van't Hoff factor $$i is 1.$$

Question 9

If a solution has a concentration of 0.015 mol/L and the temperature is 299.15 K, what is the value of $$M 	imes T$$?

Accepted Answer

$$0.015 	imes 299.15 = 4.487$$ mol \cdot K / L

Question 10

A solution contains 273.15 mg of solute in 1.0 L. If the molar mass of the solute is 81.389 g/mol, what is the molarity of the solution?

Accepted Answer

$$\frac{273.15 \ 	ext{mg}}{1000 \ 	ext{mg/g}} = 0.27315 \ 	ext{g}$$; $$M = \frac{0.27315}{81.389} = 0.00336$$ mol/L

Question 11

Which of the following would increase the osmotic pressure of a solution?

Accepted Answer

Increasing the concentration of solute

Question 12

A hospital needs to prepare an isotonic solution for intravenous use. Which property must match that of blood to avoid cell damage?

Accepted Answer

Osmotic pressure

Question 13

If the temperature in Kelvin is doubled, what happens to the osmotic pressure of a solution, assuming all other variables remain constant?

Accepted Answer

It doubles

Question 14

Which of the following is the correct conversion from Celsius to Kelvin?

Accepted Answer

$$K = ^\circ C + 273.15$$

Question 15

A solution has an osmotic pressure of 8,235,458,866.728 mmHg. What is the most likely error in this calculation?

Accepted Answer

The units were not properly converted or a calculation step was missed.

Question 16

Which of the following is NOT a factor in the osmotic pressure formula $$\Pi = iMRT$$?

Accepted Answer

Volume of the solution

Question 17

Why is it important to use temperature in Kelvin when calculating osmotic pressure?

Accepted Answer

Kelvin is an absolute scale, ensuring proportionality in gas laws and osmotic pressure calculations.

Question 18

A solution is prepared with a solute that dissociates into three ions. What is the Van't Hoff factor $$i$$ for this solute?

Accepted Answer

$$i = 3$$

Question 19

Which of the following real-world scenarios best illustrates the importance of osmotic pressure in medicine?

Accepted Answer

Administering intravenous fluids that match the osmotic pressure of blood to prevent cell lysis or shrinkage.

Osmotic Pressure in Solutions: Principles and Calculations

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