Adding Net Ionic Equations


by yellowduck
Tags: adding, equations, ionic
yellowduck
yellowduck is offline
#1
Jul19-06, 08:34 PM
P: 16
This should be easy but I feel there is something I am mission

I need to write the net ionic equations and then add #1 & #2 and compare to #3.

Equation #1 - write net ionic equation for dissolution of solid NaOH in water
Equation: NaOH (s) + H2O --> Na+ (aq) + OH- (aq) + H2O (l)
Net: NaOH (s) --> Na+ (aq) + OH- (aq)
(it says in the book to seperate strong bases such as NaOH but if I do all ions cancel out???)

Equation #2 - write net ionic equation for aqueous soloutions of NaOH & HCl
Equation: NaOH (aq) + HCl (aq) ---> NaCl (aq) + H2O (l)
Net: OH- (aq) + H+ (aq) --> H2O (l)

Equation 3: Solid NaOH and aqueous HCl
Equation: NaOH (s) + HCl (aq) ---> NaCl (aq) + H2O
OH- (s) + H+ (aq) --> H2O (l)

Add #1 & #2
This is where I get lost. I think it should be net equation #2. The difference is in the solid/aqueous state.

thanks
Phys.Org News Partner Science news on Phys.org
Review: With Galaxy S5, Samsung proves less can be more
Making graphene in your kitchen
Study casts doubt on climate benefit of biofuels from corn residue
PPonte
#2
Jul19-06, 08:48 PM
P: n/a
1. Add #1 to #2.

[tex]NaOH \text{(s)} + OH^- \text{(aq)} + H^+ \text{(aq)} \longrightarrow Na^+ \text{(aq)} + OH^- \text{(aq)} + H_2O \text{(l)}[/tex]

2. Delete the common compounds on both members of the equation.

[tex]NaOH \text{(s)} + H^+ \text{(aq)} \longrightarrow Na^+ \text{(aq)} + H_2O \text{(l)}[/tex]
yellowduck
yellowduck is offline
#3
Jul19-06, 09:08 PM
P: 16
Is it possible that I have equation #3 wrong.
Should the net ionic equation look like your final answer above?

PPonte
#4
Jul19-06, 09:44 PM
P: n/a

Adding Net Ionic Equations


Quote Quote by yellowduck
Is it possible that I have equation #3 wrong.
Should the net ionic equation look like your final answer above?
You have #3 correct, I think.

sdekivit
sdekivit is offline
#5
Jul20-06, 02:44 AM
P: 92
Solid NaOH in HCl-solution. The HCl-solution contains [tex]H^{+}[/tex] and [tex]Cl^{-}[/tex] but the solid is just NAOH. So the reaction at 3 should be:

[tex]NaOH(s) + H^{+} \rightarrow Na^{+} + H_{2}O[/tex]
dissolver
dissolver is offline
#6
Aug6-06, 02:56 PM
P: 16
So if it states solid, then you must write out the entire formula even in the net ionic equation (because it is infered that the solid is not dissolved in the solution)?


Register to reply

Related Discussions
Chemistry - Net ionic equations, ionic solids..! Biology, Chemistry & Other Homework 2
ionic equations? Biology, Chemistry & Other Homework 2
Net Ionic Equations Biology, Chemistry & Other Homework 5
Ionic equations Chemistry 8
net ionic equations Chemistry 1