help please.

[hard]

i have this question right, can you please tell me if i'm right regarding the full equations.


reaction                                             Equations                         

Hydrocholric acid + calcium carbonate            Full:

Hydrochloric acid + copper oxide                    Full:    

Hydrochloric acid + magnesium                    Full:
           .                               
Hydrochloric acid + sodium hydrogen carbonate  Full:

Hydrochloric acid + ammonia                   Full: 

hydrochloric acid + silver nitrate            Full:


however my concern here is the ionic reactions. Can someone please show me how to do then? i know that it is the spectator ions that are left out however the actual equation we havn't done yet, so would any one care to explain? thanx.

[cara.mel]

Aside from a typo, they're right (although I am not sure about hydrochloric acid + ammonia, but charges balance and stuff so it *looks* right at least)

For ionic equations, they're pretty much the same thing.
Eg in equation 1
CaCO3(s) + 2H+(aq) -> Ca2+ (aq) + CO2 (g) + H2O (l)
As Cl is aq on both sides, its not included
Everything balances as normal, don't worry about how the full equation is balanced.
From one example you should be able to do the rest

[hard]

thanks caramale, that's all i needed.

[hard]

sorry but for the ionic, i've learnt thorugh the text book that usually or always the products are of aqueous solution. then a precipitation reaction occurs or something, and one turns solid or changes state, i.e. in the products. can you show me the first two in terms of their ionic equations? trhannxxx

[cara.mel]

Like this one?

NaCl(aq) + AgNO3(aq) -> AgCl(s) + NaNO3(aq) (I sure hope AgNO3 is aqueous, if it isn't just pretend it is, I don't do chem any more I've forgotten a lot )
Ionic equation:
Ag + (aq) + Cl-(aq) -> AgCl (s)

[hard]

yer that's what i mean thought, in the test book, i've done questions similar to that one you've just done but take this for example.

Hydrochloric acid + magnesium                     Full: Mg(s) + Cl(aq)----> MgCl2(aq) + H2(g)


i got a solid, aqueous and gas in the equation.
what do i leave and what do i take?

[bturville]

if its a metal, its solid. if its a soluble compound, its aqueous. it helps to remember a few of the basic solubility rules in case you are not sure what compounds are soluble or not.

sorry if that sounds really obvious, i didn't quite get what you meant by "what do i leave and what do i take"

[cara.mel]

Edit: This post is incorrect, all future readers should ignore it
(yay for lack of sleep)

yer that's what i mean thought, in the test book, i've done questions similar to that one you've just done but take this for example.

Hydrochloric acid + magnesium                     Full: Mg(s) + Cl(aq)----> MgCl2(aq) + H2(g)


i got a solid, aqueous and gas in the equation.
what do i leave and what do i take?

In that one, there are no spectator ions, everything reacts so ionic equation is the same as the full one
(being picky, 2HCl )

[Mao]

the Cl doesnt do anything

[hard]

ohh thanks yes i get it now!

[cara.mel]

yeah i is idiot

[hard]

must be a pretty smart idiot

[Collin Li]

I disagree. Hydrochloric acid is covalently bonded, so it is not a spectator ion.

[Mao]

i believe dissociation occurs first, it is, afterall, a very strong acid.

[Lycan]

I disagree. Hydrochloric acid is covalently bonded, so it is not a spectator ion.

I agree with the disagreement. Spectator ions only occur when something is ionically bonded which HCl is not.