Question

Write the equation for the dissolution of sr(no3)2 in water. how many moles of strontium ions and nitrate ions are produced by dissolving 0.5 mol of strontium nitrate?

Answer 1

                                    Sr(NO3)2 ---> Sr²⁺ +       2 NO3⁻
from the reaction         1 mol            1 mol           2 mol
from the problem         0.5 mol         0.5 mol        1 mol

Answer 2

Answer: Moles of strontium and nitrate ions formed by dissolving 0.5 moles of strontium nitrate in water are 0.5 moles and 1 mole respectively.

Explanation:

We are given a chemical compound known as strontium nitrate having chemical formula $Sr(NO_3)_2$. This is an ionic compound and when it is dissolved in water, it will dissociate into its respective ions.

We are given:

Moles of strontium nitrate = 0.5 moles

The chemical equation for the ionization of strontium nitrate follows:

$Sr(NO_3)_2(aq.)\rightarrow Sr^{2+}(aq.)+2NO_3^-(aq.)$

By Stoichiometry of reaction:

1 mole of strontium nitrate produces 1 mole of strontium ions and 2 moles of nitrate ions.

So, 0.5 moles of strontium nitrate will produce = $(1\times 0.5)=0.5mol$ of strontium ions and $(2\times 0.5)=1mol$ of nitrate ions.

Hence, moles of strontium and nitrate ions formed by dissolving 0.5 moles of strontium nitrate in water are 0.5 moles and 1 mole respectively.