If #0.276*mol# silver chloride was collected from a reaction between silver nitrate and magnesium chloride, how many equiv magnesium nitrate were used?

Question

Owen Ambrose · Accepted Answer

One equiv of silver ion, #Ag^+#, and half an equiv of #MgCl_2(aq)#.

And how do we know? Well, if we write the stoichiometric equation we have illustrated the stoichiometry: #2AgNO_3(aq) + MgCl_2(aq) rarr Mg(NO_3)_2(aq) + 2AgCl(s)darr# Alternatively, we could write the net ionic equation........... #Ag^(+) + Cl^(-) rarr AgCl(s)darr# Given the stoichiometry, #(0.276*mol)/2# #MgCl_2# were used..

Serenity Allen · Answer

undefined To find the number of equivalents of magnesium nitrate used, you need to use the stoichiometry of the reaction. Since magnesium chloride reacts with silver nitrate, you need to determine the mole ratio between magnesium chloride and magnesium nitrate. Then, you can use this ratio to calculate the number of moles of magnesium nitrate needed to produce the same amount of silver chloride as the reaction between silver nitrate and magnesium chloride. Finally, you convert the moles of magnesium nitrate to equivalents.

Without the balanced chemical equation for the reaction between silver nitrate and magnesium chloride, I cannot provide the exact stoichiometry. Once you provide the balanced equation, I can help you calculate the number of equivalents of magnesium nitrate used.