Question #32650

1 Answer
Oct 28, 2017

Answer:

#"55.5 g"#

Explanation:

Start by calculating the number of moles of calcium chloride that must be dissolved in your solution in order for it to have a molarity of #"0.100 mol L"^(-1)#.

You know that this solution must contain #0.100# moles of calcium chloride for every #"1 L"# of the solution, so you can say that your sample must contain

#5.00 color(red)(cancel(color(black)("L solution"))) * "0.100 moles CaCl"_2/(1color(red)(cancel(color(black)("L solution")))) = "0.500 moles CaCl"_2#

Now, to convert the number of moles of calcium chloride to moles, you need to use the molar mass of the salt.

#0.500 color(red)(cancel(color(black)("moles CaCl"_2))) * "110.98 g"/(1color(red)(cancel(color(black)("mole CaCl"_2)))) = color(darkgreen)(ul(color(black)("55.5 g")))#

The answer is rounded to three sig figs.