Calculate the molality of each of the following aqueous
solutions: (a) 2.01 M NaCl (density of...
Calculate the molality of each of the following aqueous
solutions: (a) 2.01 M NaCl (density of solution = 1.08 g/mL) m (b)
51.8 percent by mass KBr solution
Calculate the molality for each of the following solutions.
Then, calculate the freezing-point depression
?TF =
KFcm
produced by each of the salts. (Assume the density of water is
1.00 g/mL and
KF = 1.86
Calculate the molality of each of the following solutions.
1) 583g of H2SO4 in 1.50 kg of water.
2) 0.86g of NaCl in 1.00x10^2g of water.
3) 46.85g of codeine, C18H21NO3, in 125.5g of ethanol,
C2H5OH.
4) 25g of I2 in 125g of ethanol, C2H5OH.
A 0.380 m aqueous solution of NaCl is prepared at 20.0∘C. Assume
that the density of the solution at 20.0∘C is 1.082 g/mL.
Calculate the molarity of the salt solution.
Calculate molality for the following solutions. (Assume solution
density is 0.998 g/mL) a) 0.540g Mg(NO3)2 in 250 mL of solution, b)
35 mL of 9.00 M H2SO4 diluted to 0.500 L
What is the concentration of each of the following solutions?
(a) The molality of a solution prepared by dissolving 25.0 g of
H2SO4 in 1.30 L of water (b) The mole fraction of each component of
a solution prepared by dissolving 2.25 g of nicotine, C10H14N2, in
80.0 g of CH2Cl2
Calculate the number of moles of solute present in each of the
following aqueous solutions. 600 mL of 0.250 M SrBr2 122.0 g of a
solution that is 6.65% glucose (C6H12O6) by mass.
You have 825.0 mL of 0.550 M aqueous NaCl. For each of the
following statements, determine whether the statement is true of
false.
If the statement is true, type "true" in the blank next to the
statement.
If the statement is false, type "false" in the blank next to the
statement.
________ There are 825 mL of solution
________ If you add water to the solution, the molarity will
increase.
________ There is 0.550 moles of NaCl in 825 mL...