Which of the following statements is true? A) When a nonvolatile solute is added to a solvent, the solute vapor pressure decreases. B) When a nonvolatile solute is added to a solution, the solvent vapor pressure increases. C) When a nonvolatile solute is added to a solvent, the solute vapor pressure increases. D) When a nonvolatile solute is added to a solution, the solvent vapor pressure decreases.

Why can measuring osmotic pressure help you find the molar mass of a solute? Assume that the solute is not an electrolyte. Choose the best answer. Choose one: Osmotic pressure depends on the hydrogen bonding capacity of the solute. Osmotic pressure depends on the molarity of the solute. Osmotic pressure depends on the mass of the solute. Osmotic pressure depends on the chemical identity of the solute. The osmotic pressure inside human cells is about 8 atm. at 20.85 °C. My advisor once misread a protocol I gave him, and without thinking washed the cells with a solution of 1.88 M NaCl. He immediately swore. What happened to the cells? Choose one: O The cells absorbed water and exploded. The high concentration of salt made the water boil at room temperature. The high concentration of salt made the water freeze at room temperature. The cells lost their water to the solution and collapsed.

The dispersed phase of a certain colloidal dispersion consistes of spheres of diameter 1.0 x 102 nm. What are the volume and surface area of each sphere? V = _ and SA = _ How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters? _ spheres, total SA = _ m2 The dispersed phase of a certain colloidal dispersion consistes of spheres of diameter 1.0 x 102 nm.

Molality is defined as g solute/L of solvent mol solute/kg of solution mol solute/L of solution mol solute/kg of solvent

Which of the following is a proper procedure for creating a supersaturated solution of potassium nitrate if you have 100g of water and 80g of potassium nitrate available?      Add all of the solute to 100g of water and stir for an extremely long time.       Add all of the solute to 100g of water and heat it up past 48 degrees C.       Add all of the solute to 100g of water & heat it up past 48 degrees C. Make sure everything dissolves, and then carefully cool it down below 48 degrees C.       Add all of the solute to 100g of water & heat it up just over 35 degrees C. Once everything dissolves, cool it down to below 35 degrees C.       It is impossible to make a supersaturated solution of potassium nitrate with 80g of solute & 100g of water.

I add a non-volatile solute to a pure solvent to form a solution. Will the vapor pressure of this newly formed solution be lower than that of the pure solvent at the PURE SOLVENT's normal boiling point?

In 200 words or less, give a real-world example of a colligative property of a solvent.  How does mixing a solution with a solvent change the physical properties of that solvent. For example, salt is placed on ice on a snowy day to decrease the freezing point of the ice, preventing it from melting and becoming slick and causing accidents.  The colligative property here is freezing point depression.

At a certain temperature the vapor pressure of water is 25.0 torr. A glucose solution is prepared by mixing 5.00 g of glucose and 2.00 moles of water. What is the expected vapor pressure of the solution? Molar mass of water = 18.02 g/mol and molar mass of glucose = 180.2 g/mol a) 0.342 torr b) 3.05 torr c) 22.0 torr d) 24.7 torr

Why does heating increase the speed at which a solid dissolves??

A 10.00 mL sample of ethanol is added to 250.0 mL of water in order to observe the freezing point depression of the water. Consider the possible errors in this experiment, and determine whether each would cause the freezing point of the water to increase, decrease, or remain the same compared with the expected results. It is discovered that the 10.00 g ethanol sample is actually 95% ethanol and 5% water.   The ethanol sample is left out for several minutes before being added to the water, allowing a significant amount to evaporate.   Instead of starting the experiment with room temperature water, the experiment is started with cold water.   Some of the water is splashed out of the container before the ethanol is added.   Some of the ethanol and water solution is spilled out of the container during temperature measurement.