Question

Question #85f29

Answer 1

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

Explanation:

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"`

Answer 2

`"0.601 moles"`

Explanation:

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)|)))`