I have the following problems- write net ionic equations for reactions if no reaction write NR....
silver nitrate and ammonium carbonate
sodium phosphate and potassium nitrate
silver nitrate and barium chloride
copper (II) chloride and sodium hydroxide
cobalt (III) chloride and sodium hydroxide
help... how do i know if there is a reaction or not?
For reactions of this type, look for any ONE of three things.
1. a precipitate is formed. You will need a table of solubilities.
2. a gas is formed. You need to know which elements/compounds are gases.
3. a weak electrolyte (slightly ionized compound) is formed. You need to know weak acids and weak bases; generally, those are the ones with Ka or Kb. H2O is a slightly ionized material also.
For example,
AgNO3 + (NH4)2CO3 ==>
Look at the ions. We will have Ag^+, NO3^-, NH4^+ and CO3^=.
Looking down your table of solubilities, I know immediately that Ag2CO3 is insoluble in aqueous solution and NH4NO3 is soluble; therefore, I know a reaction will take place, that Ag2CO3 will be a solid ppt and that NH4NO3 will be present as ions.
The net reaction is as follows:
2Ag^+(aq) + CO3^=)aq) ==> Ag2CO3(s)
I have a site for solutility rules if you need it.
To determine whether there is a reaction or not, you need to consider the solubility rules of compounds. Solubility rules provide guidelines on which compounds are soluble or insoluble in water.
Here are the solubility rules for the common compounds mentioned in your problems:
1. Silver nitrate (AgNO3): Silver compounds are usually soluble, except for silver chloride (AgCl), silver bromide (AgBr), and silver iodide (AgI) which are insoluble in water.
2. Ammonium carbonate (NH4)2CO3: Ammonium compounds are usually soluble, including ammonium carbonate.
3. Sodium phosphate (Na3PO4): Sodium compounds are usually soluble, including sodium phosphate.
4. Potassium nitrate (KNO3): Potassium compounds are usually soluble, including potassium nitrate.
5. Barium chloride (BaCl2): Barium compounds are soluble, except for barium sulfate (BaSO4) and barium carbonate (BaCO3), which are insoluble in water.
6. Copper (II) chloride (CuCl2): Copper compounds are usually soluble, including copper (II) chloride.
7. Sodium hydroxide (NaOH): Sodium hydroxide is soluble in water.
8. Cobalt (III) chloride (CoCl3): Cobalt compounds are usually soluble, including cobalt (III) chloride.
Using these solubility rules, let's determine the reactions:
1. Silver nitrate and ammonium carbonate:
- Silver nitrate (AgNO3) is soluble.
- Ammonium carbonate ((NH4)2CO3) is soluble.
- Both compounds are soluble, so a reaction occurs.
- The net ionic equation is: Ag+(aq) + CO3 2-(aq) → Ag2CO3(s) + (NH4)+ (aq)
2. Sodium phosphate and potassium nitrate:
- Sodium phosphate (Na3PO4) is soluble.
- Potassium nitrate (KNO3) is soluble.
- Both compounds are soluble, so a reaction occurs.
- The net ionic equation is: 3Na+(aq) + PO4 3-(aq) + 3K+(aq) + NO3-(aq) → Na3PO4(aq) + 3K+(aq) + NO3-(aq)
3. Silver nitrate and barium chloride:
- Silver nitrate (AgNO3) is soluble.
- Barium chloride (BaCl2) is soluble.
- Both compounds are soluble, so a reaction occurs.
- The net ionic equation is: Ag+(aq) + Cl-(aq) → AgCl(s)
4. Copper (II) chloride and sodium hydroxide:
- Copper (II) chloride (CuCl2) is soluble.
- Sodium hydroxide (NaOH) is soluble.
- Both compounds are soluble, so a reaction occurs.
- The net ionic equation is: Cu2+(aq) + 2OH-(aq) → Cu(OH)2(s)
5. Cobalt (III) chloride and sodium hydroxide:
- Cobalt (III) chloride (CoCl3) is soluble.
- Sodium hydroxide (NaOH) is soluble.
- Both compounds are soluble, so a reaction occurs.
- The net ionic equation is: Co3+(aq) + 3OH-(aq) → Co(OH)3(s)
In summary, by applying the solubility rules, you can determine if a reaction occurs between two compounds. If both compounds are soluble, a reaction occurs, and you can write the net ionic equation. If either of the compounds is insoluble, no reaction occurs, and you can write "NR" as the answer.