The question is incomplete, here is the complete question:
A bottle of rubbing alcohol having aqueous solution of alcohol contains 70% (v/v) alcohol. If Carl buys a 946 ml bottle of rubbing alcohol, how much of the aqueous solution is water?
<u>Answer:</u> The amount of water present in the given bottle of rubbing alcohol is 283.8 mL
<u>Explanation:</u>
We are given:
Volume of bottle of rubbing alcohol = 946 mL
70% (v/v) alcohol solution
This means that 70 mL of rubbing alcohol is present in 100 mL of solution
Amount of water present in solution = [100 - 70] = 30 mL
Applying unitary method:
In 100 mL of solution, the amount of water present is 30 mL
So, in 946 mL of solution, the amount of water present will be = 
Hence, the amount of water present in the given bottle of rubbing alcohol is 283.8 mL
What is the question? Explain what answer you need(
16 g/ml
<h3>Further explanation</h3>
Given
mass = 32.40 g
volume = 2.0mL
Required
Density
Solution
Density is a quantity derived from the mass and volume
Density is the ratio of mass per unit volume
Density formula:
ρ = density
m = mass
v = volume
Input the value :
ρ = 32.40 g / 2.0 ml
ρ = 16.2 g/ml
Rules for division: The least number of significant figures in the problem determines the number of significant figures in the answer.
32.40 = 4 sig.fig
2.0 = 2 sig fig
The answer must be 2 sig fig
So the answer = 16 g/ml
Answer:
151 g/mol
Explanation:
When a nonvolatile substance is added to a solvent, the freezing point of the solvent is changed, which is called cryoscopy. When temperature change can be calculated by:
ΔT = Kf*W
Where Kf is the molal freezing point constant of the solvent and W is the molality of the solution.
For cyclohexane, Kf = 20.2 °C/molal, and the freezing point is 6.4 °C, so:
6.4 - 1.05 = 20.2 * W
20.2W = 5.35
W = 0.26485 molal
The molality is:
W = m1/m2*M1
Where m1 is the mass of the solute (in g), m2 is the mass of the solvent (in kg), and M1 is the molar mass of the solute. So:
0.26485 = 2.00/0.05M1
0.0132425M1 = 2.00
M1 = 151 g/mol
Answer:
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Explanation:
