Question

A 4,000 mL solution of AgNO3 contains 17.00 g of solute in water. Calculate the molarity (molar concentration) of the solution.

3 x 10 -5M
3 x 10 -2M
4 x 10 -1M
1 x 10 -4M

Answer 1

2.5 x 10⁻² ≅ 3.0 x 10⁻² M.

Step-by-step explanation:

Molarity is defined as the no. of moles of a solute per 1.0 L of the solution.

M = (no. of moles of solute)/(V of the solution (L)).

∴ M = (mass/molar mass)of AgNO₃/(V of the solution (L)).

∴ M of AgNO₃ = (17.0 g / 169.87 g/mol)/(4.0 L) = 2.5 x 10⁻² ≅ 3.0 x 10⁻² M.

Answer 2

Answer:
`3* 10^(-2)mol/L`

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

`V_s` = volume of solution in ml

moles of solute =

Now put all the given values in the formula of molarity, we get

`Molarity=(0.1moles* 1000)/(4000ml)=0.03mole/L=3* 10^(-2)M`

Thus molarity of the solution will be
`3* 10^(-2)M`