Question

What is the mass of nickel(II) nitrate (182.71 g/mol) dissolved in 25.0 mL of 0.100 M Ni(NO3)2 solution? A) 157 g B) 0.250 g C) 4578 D) 0.4578 E) 4.00 g

Answer 1

Answer: 0.4578 g

Step-by-step explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

`Molarity=(n* 1000)/(V_s)`

where,

n= moles of solute

`Moles=\frac{\text{Given mass}}{\text{Molar mass}}=(xg)/(182.71g/mol)`

`V_s` = volume of solution in ml = 25.0 ml

`0.100M=(x* 1000)/(182.71* 25)`

`x=0.4578g`

Thus 0.4578 g of nickel(II) nitrate is to be dissolved in 25.0 mL of 0.100 M
`Ni(NO_3)_2` solution.