The molar mass of acetic acid in benzene and in water is to be determined. The state of acetic acid in both solutions is to be explained and the structure of acetic acid in benzene is to be drawn. Concept introduction: Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are, Decrease in the vapor pressure Increase in the boiling point Decline in the freezing point Osmotic pressure Change in freezing point is calculated by using the equation, Δ T f p = K f p m s o l u t e where, K f p is the molal freezing point depression constant. The number of moles of any substance can be determined using the equation Number of mole = Given mass of the substance Molar mass
The molar mass of acetic acid in benzene and in water is to be determined. The state of acetic acid in both solutions is to be explained and the structure of acetic acid in benzene is to be drawn. Concept introduction: Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are, Decrease in the vapor pressure Increase in the boiling point Decline in the freezing point Osmotic pressure Change in freezing point is calculated by using the equation, Δ T f p = K f p m s o l u t e where, K f p is the molal freezing point depression constant. The number of moles of any substance can be determined using the equation Number of mole = Given mass of the substance Molar mass
Solution Summary: The author explains the molar mass of acetic acid in benzene and in water.
Interpretation: The molar mass of acetic acid in benzene and in water is to be determined. The state of acetic acid in both solutions is to be explained and the structure of acetic acid in benzene is to be drawn.
Concept introduction:
Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are,
Decrease in the vapor pressure
Increase in the boiling point
Decline in the freezing point
Osmotic pressure
Change in freezing point is calculated by using the equation,
ΔTfp=Kfpmsolute
where,
Kfp is the molal freezing point depression constant.
The number of moles of any substance can be determined using the equation
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.
In regards to freezing point depression:
The original experiment calls for 3 grams lauric acid and .4 g benzoic acid to be melted and then observed to crystalize to demonstrate freezing point depression.
A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning.
I think that since the amount of lauric acid (3g) doesnt change that the solution may be too oversaturated with benzoic acid. I'm not sure if this would still demonstrate freezing point depression since it is a colligative property based on amount of solute....
Illustrate dissolution of the ionic solid NaCl in water?