Respuesta :
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
from the reaction 1 mol 1 mol 2 mol
from the problem 0.5 mol 0.5 mol 1 mol
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 [tex]Sr(NO_3)_2[/tex]. 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:
[tex]Sr(NO_3)_2(aq.)\rightarrow Sr^{2+}(aq.)+2NO_3^-(aq.)[/tex]
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 = [tex](1\times 0.5)=0.5mol[/tex] of strontium ions and [tex](2\times 0.5)=1mol[/tex] 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.
