1) An old sample of concentrated sulfuric acid to be used in the laboratory is a

Question

1) An old sample of concentrated sulfuric acid to be used in the laboratory is approximately 97.5 percent H2SO4 by mass. Calculate the Molarity of the acid solution. The density of the solution is 1.83g/ml. (enter your answer in scientific notation).

2) The solubility of N2 in blood at 37 degree C and at a partial pressure of 0.80 atm is 5.6 X10 to the minus 4 mol/L. A deep sea diver breathes compressed air with the partial pressure of N2 equal to 5.5 atm. Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of N2 gas released (in liters at 37 degree C and 1.00 atm) when the diver returns to the surface of the water where the partial pressure of N2 is 0.50 atm.

These two questions were not done. first question answer has to be written in scientific notation.

Explanation / Answer

1)
Let volume of solution be 1 L
volume , V = 1 L
= 1*10^3 mL


density, d = 1.83 g/mL
use:
mass = density * volume
= 1.83 g/mL *1*10^3 mL
= 1830.0 g
This is mass of solution
mass of H2SO4 = 97.5 % of mass of solution
= 97.5*1830.0/100
= 1784.25 g

Molar mass of H2SO4,
MM = 2*MM(H) + 1*MM(S) + 4*MM(O)
= 2*1.008 + 1*32.07 + 4*16.0
= 98.086 g/mol


mass(H2SO4)= 1784.25 g

use:
number of mol of H2SO4,
n = mass of H2SO4/molar mass of H2SO4
=(1784.25 g)/(98.086 g/mol)
= 18.2 mol
volume , V = 1 L


use:
Molarity,
M = number of mol / volume in L
= 18.2/1
= 18.2 M
Answer: 1.82*10^1 M

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