Question

How many milliliters of 2.36 M copper nitrate would be needed to react with 250 mL of 0.519 M silver nitrate solution according to the following unbalanced equation?

Cu + AgNO3 → Ag + Cu(NO3)2

Answer 1

0.028dm³

Step-by-step explanation:

Given parameters:

Molarity of Cu(NO₃)₂ = 2.36M

Volume of AgNO₃ = 250mL

Molarity of AgNO₃ = 0.519M

Unknown:

Volume of Cu(NO₃)₂ = ?

Solution:

To solve this problem, we are going to use the mole concept working from the known to the unknown specie in the balanced expression.

The known specie is the silver nitrate solution.

We should obtain our number of moles of the unknown product here and establish its volume.

Balanced equation:

Cu + 2AgNO₃ → 2Ag + Cu(NO₃)₂

Molarity =
`(number of moles)/(Volume)`

Number of moles = molarity x volume

Number of moles of AgNO₃ = ?

Convert mL to L

1000mL = 1L = 1dm³

250mL, = 0.25dm³

Number of moles of AgNO₃ = 0.519 x 0.25 = 0.13mole

From the balanced reaction equation:

2 mole of AgNO₃ = 1 mole of Cu(NO₃)₂

0.13mole of AgNO₃ =
`(0.13)/(2)` = 0.07mole of Cu(NO₃)₂

Volume of Cu(NO₃)₂ =
`(number of moles)/(molarity)` =
`(0.07)/(2.36)` = 0.028dm³