Question #85f29

2 Answers
Apr 6, 2016

The answer is really easy. It just takes to use molarity definition to calculate it.


Molarity or molar concentration, #M# is defined by:

#M= {"number of solute moles"}/{"number of litres of disolution"}#

We just must find the number of moles of solute, so:

#"number of moles of solute" =#
#= 0.325 " M" cdot 1.85 " L" = 0,60125 " mol"#

Apr 6, 2016

#"0.601 moles"#


A solution's molarity tells you how many moles of solute you get in one liter of solution.

In essence, molarity is a measure of concentration that deals with moles of solute and liters of solution. This means that a solution's molarity can be used as a conversion factor that can help you convert moles to liters of solution and vice versa.

In your case, the solution is said to have a molarity of

#c = "0.325 M" = "0.325 mol L"^(-1)#

This tells you that every liter of this solution will contain #"0.325# moles of solute.

Use this as a conversion factor to see how many moles you'd get in #"1.85 L"# of solution

#1.85 color(red)(cancel(color(black)("L solution"))) * overbrace("0.325 moles"/(1color(red)(cancel(color(black)("L solution")))))^(color(purple)("a molarity of 0.325 M")) = "0.60125 moles"#

Rounded to three sig figs, the answer will be

#"no. of moles of solute" = color(green)(|bar(ul(color(white)(a/a)0.601color(white)(a/a)|)))#