A biochemist carefully measures the molarity of magnesium ion in 47, mL of cell growth medium to be 97. ??. Unfortunately, a car
eless graduate student forgets to cover the container of growth medium and a substantial amount of the solvent evaporates. The volume of the cell growth medium falls to 6.0 mL. Calculate the new molarity of magnesium ion in the cell growth medium Be sure your answer has the correct number of significant digits. HM x 10
1 answer:
Complete Question
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Answer:
Answer: 760 uM
Explanation:
the addition of solvent to a solution in a such away that the volume of the solution increases and the concentration decreases is a process know as dilution
The concentration and the volume of the dilute and concentrated solution are given below as follows
Concentrated solution Dilute solution
Given that M1 = 97.0uM
V1 = 47.0 mL
V2 = 6.0 mL
M2 = ?
Therefore M1V1 = M2V2
M2 = M1V1/V2
M2 = (97*47)/6
M2 = 760 uM
Answer: 760 uM
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Norfenefrine (C₈H₁₁NO₂).
<h3>Further explanation</h3>We will solve a case related to one of the colligative properties, namely freezing point depression.
The freezing point of the solution is the temperature at which the solution begins to freeze. The difference between the freezing point of the solvent and the freezing point of the solution is called freezing point depression.
<u>Given:</u>
A mysterious white powder could be,
- powdered sugar (C₁₂H₂₂O₁₁) with a molar mass of 342.30 g/moles,
- cocaine (C₁₇H₂₁NO₄) with a molar mass of 303.35 g/moles,
- codeine (C₁₈H₂₁NO₃) with a molar mass of 299.36 g/moles,
- norfenefrine (C₈H₁₁NO₂) with a molar mass of 153.18 g/moles, or
- fructose (C₆H₁₂O₆) with a molar mass of 180.16 g/moles.
When 82 mg of the powder is dissolved in 1.50 mL of ethanol (density = 0.789 g/cm³, normal freezing point −114.6°C, Kf = 1.99°C/m), the freezing point is lowered to −115.5°C.
<u>Question: </u>What is the identity of the white powder?
<u>The Process:</u>
Let us identify the solute, the solvent, initial, and final temperatures.
- The solute = the powder
- The solvent = ethanol
- The freezing point of the solvent = −114.6°C
- The freezing point of the solution = −115.5°C
Prepare masses of solutes and solvents.
- Mass of solute = 82 mg = 0.082 g
- Mass of solvent = density x volume, i.e.,
We must prepare the solvent mass unit in kg because the unit of molality is the mole of the solute divided by the mass of the solvent in kg.
The molality formula is as follows:
Now we combine it with the formula of freezing point depression.
It is clear that we will determine the molar mass of the solute (denoted by Mr).
We enter all data into the formula.
We get
These results are very close to the molar mass of norfenefrine which is 153.18 g/mol. Thus the white powder is norfenefrine.
<h3>Learn more</h3>- The molality and mole fraction of water brainly.com/question/10861444
- About the mass and density of ethylene glycol as an antifreeze brainly.com/question/4053884
- About the solution as a homogeneous mixture brainly.com/question/637791
Keywords: a mysterious white powder, sugar, cocaine, codeine, norfenefrine, fructose, the solute, the solvent, dissolved, ethanol, normal freezing point, the freezing point depression, the identity
