Question

Given that the molar mass of NaCl is 58.44 g/mol, what is the molarity of a solution that contains 87.75 g of NaCl in 500. mL of solution?

Use mc006-1.jpg.
0.333 M
0.751 M
1.50 M
3.00 M

Answer 1

Answer: D on Edge :)

Step-by-step explanation:

Answer 2

hi friend,


`the \: answer \: is \: 3 \: molar`
the solution is as follows


`moles \: of \: NaCl \: in \: the \: solution`

=

`give \: mass \: of \: sodium \: chloride \\ - - - - - - - - - - - - - - - - \\ molecular \: mass \: of \: sodium \: chloride \:`

=

`\: \: 87.75 \\ - - - - \\ \: \: 58.44`

`= \: 1.501 \: moles`


`\: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: moles \: of \: solute \\ Molarity \: = \: \: \: \: \: - - - - - - - \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: volume \: of \: solution(litrs)`

`applying \: the \: formulae \:`
converting ml to litres

1.501/(500/1000)

1.501 X 2

3 M



Hope it helps