I need help with solving this sentence.
Acetic acid is added to beaker containing a potassium hydroxide solution.
My teacher has told me that if the acid is not strong you should not ionize it.
Help is greatly appreciated.
Net Ionic Equations
Moderators: Xen, expert, ChenBeier
yes, you should not ionize CH3COOH.
Here is the net ionic equation:
Here is the net ionic equation:
Code: Select all
CH3COOH + OH{-} = CH3COO{-} + H2O
The reactions you are doing are called.... double displacement.
First, When you write a reaction
AgNO3(aq) + NaCl(aq) =
even though we write the atoms together they are actually seperate.
****In aqueous solutions Ionic compounds dissociate...This is big.
So even though we write them together, they are actually seperate(if they are ionic)
Molecular equation
writing a chemical equation with the substance together, like molecules, no matter what.
AgNO3(aq) + NaCl(aq) =
Ionic equation
This is a more realistic way yet not as nice to look at. If a reaction contains an ionic substance then the equation will actually show the substaces seperated as dissolved species.
Ag+ + NO3- + Na+ + Cl- =
Net ionic equations
Before explaining net ionic equations there is one more thing you need to understand. The order that the items are written make no difference. So, in order for an actual reaction to take place we need to actually have a Cation (+) and an Anion(-) come to gether and form a new solid.
In the example I chose It would be the Ag+ ion and the Cl- ion. I know this from solubility charts and or general trends of solubility.
Soooo inorder to have a reaction take place we need a new substance forming, usually a new solid but could be something like Water. (neutralization reaction)
The net ionic equation will only show those items that actually change. It will eliminate what are called "spectator ions" Spectator ions do nothing. They are floating around independatly before the rxn and are doing the same after.
AgNO3(aq) + NaCl(aq) = AgCl(s) + NaNO3(aq) note: new solid formed so reaction is OK.
Ag+ + NO3- + Na+ + Cl- = AgCl(s) + Na+ + Cl- note the new solid isn't floating around any more it is solid
Ag+ + Cl- = AgCl(s) Only changed items. No spectators
***Other ideas, or things your teacher will want you to be able to do
1. Write the correct products and write those formulas correctly.
2. Make sure that you can recognize an ionic compound when you see one. (usually metal/non-, or polyatomic)
3. Probably balancing.
4. Check for solubility of products to make sure a reaction is taking place.
_______________________________________________
SaaS ITSM change my ip
First, When you write a reaction
AgNO3(aq) + NaCl(aq) =
even though we write the atoms together they are actually seperate.
****In aqueous solutions Ionic compounds dissociate...This is big.
So even though we write them together, they are actually seperate(if they are ionic)
Molecular equation
writing a chemical equation with the substance together, like molecules, no matter what.
AgNO3(aq) + NaCl(aq) =
Ionic equation
This is a more realistic way yet not as nice to look at. If a reaction contains an ionic substance then the equation will actually show the substaces seperated as dissolved species.
Ag+ + NO3- + Na+ + Cl- =
Net ionic equations
Before explaining net ionic equations there is one more thing you need to understand. The order that the items are written make no difference. So, in order for an actual reaction to take place we need to actually have a Cation (+) and an Anion(-) come to gether and form a new solid.
In the example I chose It would be the Ag+ ion and the Cl- ion. I know this from solubility charts and or general trends of solubility.
Soooo inorder to have a reaction take place we need a new substance forming, usually a new solid but could be something like Water. (neutralization reaction)
The net ionic equation will only show those items that actually change. It will eliminate what are called "spectator ions" Spectator ions do nothing. They are floating around independatly before the rxn and are doing the same after.
AgNO3(aq) + NaCl(aq) = AgCl(s) + NaNO3(aq) note: new solid formed so reaction is OK.
Ag+ + NO3- + Na+ + Cl- = AgCl(s) + Na+ + Cl- note the new solid isn't floating around any more it is solid
Ag+ + Cl- = AgCl(s) Only changed items. No spectators
***Other ideas, or things your teacher will want you to be able to do
1. Write the correct products and write those formulas correctly.
2. Make sure that you can recognize an ionic compound when you see one. (usually metal/non-, or polyatomic)
3. Probably balancing.
4. Check for solubility of products to make sure a reaction is taking place.
_______________________________________________
SaaS ITSM change my ip