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1. Calculate the number of moles of sulfuric
acid that is contained in 250 mL of 8.500 M
sulfuric acid solution
2.7.300 moles of sodium nitrite are needed for
a reaction. The solution is 5.450 M. How
many mL are needed?
3.What mass (in g) of NH3 must be dissolved
in 875 g of methanol to make a 0.430 molal
4.Calculate the molality of a solution that is
prepared by mixing 259.5 mL of CH3OH
5.(d = 0.792 g/mL) and 1387 mL of
CH3CH2CH2OH (d = 0.811 g/mL)
6.A solution is prepared by dissolving 318.6 g
sucrose (C12H22O11) in 4905 g of water.
Determine the molarity of the solution
7.Commercial grade HCl solutions are
typically 39.0% (by mass) HCl in water.
Determine the molarity of the HCl, if the
solution has a density of 1.20 g/mL.
Commercial grade HCl solutions are typically
39.0% (by mass) HCl in water. Determine the
mol of the HCl, if the solution has a density of
9. Determine the freezing point depression of a
solution that contains 50.7 g glycerin (C3H8O3,
molar mass = 92.09 g/mol) in 376 mL of water.
Some possibly useful constants for water are
Kf = 1.86°C/m and Kb = 0.512°C/m.
10. For the previous question determine the
boiling point elevation for the same solution
Calculate the boiling point of a solution of 570.0
g of ethylene glycol (C2H6O2) dissolved in 800.0
g of water. Kf = 1.86°C/m and Kb = 0.512°C/m.
Use 100°C as the boiling point of water.
12. For the previous question determine the
freezing point depression
13. What volume of a 0.6 M KBr solution is
needed to provide 30.5 g of KBr?
14. What volume of 3.00 M CH3COOH solution
is needed to provide 0.220 mol of CH3COOH?