What is the molarity of a solution prepared from 85. 0 g cacl2 in 300. 0 g of solution? the density of the solution is 1. 05 g/m
1 answer:
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<u>Answer:</u> The molar mass of the insulin is 6087.2 g/mol
<u>Explanation:</u>
To calculate the concentration of solute, we use the equation for osmotic pressure, which is:
Or,
where,
= osmotic pressure of the solution = 15.5 mmHg
i = Van't hoff factor = 1 (for non-electrolytes)
Mass of solute (insulin) = 33 mg = 0.033 g (Conversion factor: 1 g = 1000 mg)
Volume of solution = 6.5 mL
R = Gas constant =
T = temperature of the solution =
Putting values in above equation, we get:
Hence, the molar mass of the insulin is 6087.2 g/mol
Answer:
The density of the metal is 0.561 g/mL
Explanation:
The computation of the density of the metal is shown below;
As we know that
The Density of the metal is
where,
Mass = 4.9g
Change in volume = 6.9 mL
Now place these values to the above formula
So, the density of the metal is
= 0.561 g/mL
Hence, the density of the metal is 0.561 g/mL
We simply applied the above formula so that the correct density could arrive