A
solution contains 0.600 g of Ca2 in enough water to make a 1875 mL
solution....
A
solution contains 0.600 g of Ca2 in enough water to make a 1875 mL
solution. What is the milliequivalents of Ca2 per liter (mEq/L) for
this solution?
A solution contains 0.750 g of Mg2 in enough water to make a
1875 mL solution. What is the milliequivalents of Mg2 per liter
(mEq/L) for this solution?
A solution contains 0.725 g of Mg2 in enough water to make a
1875 mL solution. What is the milliequivalents of Mg2 per liter
(mEq/L) for this solution?
If 4.90 g of Na2CO3 is dissolved in enough
water to make 250. mL of solution, what is the molar concentration
of the sodium carbonate?
Molar concentration of Na2CO3 =
______M
What are the molar concentrations of the Na+ and
CO32- ions?
Molar concentration of Na+ = ______M
Molar concentration of CO32- =
_______M
A solution is prepared by dissolving 171g of CdCl2 in
enough water to make 250.0 mL of solution. If the density of the
solution is 1.556 g/mL, calculate: Molarity of the solution, mole
fraction of CdCl2, and molality of the solution.
A 0.4400-g sample of impure Ca(OH)2 is dissolved in enough water
to make 60.30 mL of solution. 20.00 mL of the resulting solution is
then titrated with 0.1461-M HCl. What is the percent purity of the
calcium hydroxide if the titration requires 18.33 mL of the acid to
reach the endpoint?
An ethylene glycol solution contains 16.2 g of ethylene glycol
(C2H6O2) in 87.4 mL of water.
Part A
Calculate the freezing point of the solution. (Assume a density
of 1.00 g/mL for water.)
Part B
Calculate the boiling point of the solution.
An ethylene glycol solution contains 27.6 g of ethylene glycol
(C2H6O2) in 90.4 mL of water. (Assume a density of 1.00 g/mL for
water.) Kb of water=0.51C/m and Kf of water=-1.86C/m
Part A: Determine the freezing point of the solution. Express
your answer in degrees Celsius.
Part B: Determine the boiling point of the solution. Express
your answer in degrees Celsius.