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Chemistry ionic equations

hi guys, i'm really stuck,

the question is this:

when aqueous magnesium chloride is added to aqueous silver nitrate a white precipitate is formed.

write out full stoichiometric and ionic equation.

i knew how to to do this before, but i'm overthinking and now i'm confused. step by step would be really helpful if possible.

Thanks.

Reply 1

charco

Study Forum Helper

amina khan

In double decomposition (ppt) reactions:

XA + YB --> YA + XB

you have only two choices for the insoluble reagent, XB or YA

Your decision is which one?

Once you have decided you show only the ions that make this ppt...

Reply 2

Kevlar

Magnesium Chloride + Silver Nitrate ---> Precipitate + Salt ( SilverChloride + Magnesium Nitrate)

Stoichemetric Eqn

Spoiler

Ionic Eqn

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Net Ionic Eqn

Spoiler

idk I can just do it sorry cant explain lol! :3

Reply 3

chemicalguy

Kevlar

Magnesium Chloride + Silver Nitrate ---> Precipitate + Salt ( SilverChloride + Magnesium Nitrate)

Stoichemetric Eqn

Spoiler

Ionic Eqn

Spoiler

Net Ionic Eqn

Spoiler

idk I can just do it sorry cant explain lol! :3

These are just not right!, Mg is 2+ for starters

Reply 4

chemicalguy

Stoichiometric

MgCl2(aq) + 2AgNO3 (aq) --> 2AgCl(s) + Mg(NO3)2 (aq)

Ionic
Ag+(aq) + Cl-(aq) --> AgCl(s)

Its all about solubility, all nitrates are soluble, AgCl is the white ppt test for chlorides

thanks so much!

Original post by chemicalguy

Stoichiometric

MgCl2(aq) + 2AgNO3 (aq) --> 2AgCl(s) + Mg(NO3)2 (aq)

Ionic
Ag+(aq) + Cl-(aq) --> AgCl(s)

Its all about solubility, all nitrates are soluble, AgCl is the white ppt test for chlorides

Could you please tell me why it is not 2Ag+(aq) + Cl2- (aq) -> 2AgCl (s), i.e why do you eliminate the 2 from the balanced equation when you write the ionic equation? Many thanks