Double Replacement Reaction Lab
Title: Double Replacement Reactions (Data and Calculations)
Objective: Classify the chemical reaction through observation, which each reagent produce when mixed with another reagent. After careful observation, be able to prove each observation using the net ionic equation.
Background: First, a double-replacement reaction is when two cations in different compound switch anions, AX + BZ → BY. If either compounds are insoluble a precipitate occurs, and if there is no precipitate formed there is no reaction. Also, not all ionic compounds are soluble in water, and there are a few solubility rules that need to be followed (see Chapter 8 in book). Second, there is also something known as a neutralization reaction, here the reaction is between …show more content…
This left us with the silver and chlorine which yield us silver chloride which is a solid. We did note on our observation that we had a change in color and a solid precipitate.
3. Na2CO3(aq)+ HCl(aq) → NaCl(aq) + HCO3(aq)
Na2CO3 + 2HCl → 2NaCl + H2O + CO2(aq)
2Na+ + CO32- + 2H+ + 2Cl- → 2Na+ + 2Cl- + H2O + CO2
CO32- + 2H+ → H2O(l) + CO2(g)
With this reaction the carbonate and the diatomic hydrogen combined together to make the bubbling effect that we had noted. This leaves us with the water molecule with the sodium chloride dissolved in it with the carbon dioxide gas bubbles.
4. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
Na+ + OH- + H+ + Cl- → Na+ + Cl- + H2O(l)
OH- + H+ → H2O
This reaction with a strong acid, as noted, released heat, which we call an exothermic reaction.
5. BaCl2(aq) + H2SO4 → BaSO4(s) + 2HCl
Ba+2 + 2Cl- + 2H+ + SO4-2 → BaSO4(s) + 2H+ + 2Cl-
Ba+2 + SO4-2 → BaSO4(s)
Here we have Hydrogen and chlorine as spectator ions. One of the solubility rules is that sulfates are soluble except in Barium. During observation we noted a color change in liquid though not a solid …show more content…
NH3 + H2O+ H2SO4 → (NH4)2 SO4 + 2H2O
2NH4OH + H2SO4 → (NH4)2 SO4 + 2H2O
2NH4+ + OH- + 2H+ + SO4-2 → 2NH4+ + SO4-2 + 2H2O
OH- + 2H+ → 2H2O(l)
Aqueous ammonia is ammonia in water. Aqueous ammonia reacts with sulfuric acid, which then forms the salt ammonium sulfate and water. This is a neutralization reaction.
7. CuSO4 + Zn(NO3)2 → Cu(NO3)2 + ZnSO4
Cu+2 + SO4-2 + Zn+2 + 2NO3- → Cu+2 + 2NO3- + Zn+2 + SO4-2
All are cancelled out as spectator ions, so as observed there was no reaction that took place.
8. Na2CO3 + CaCl2 → 2NaCl + CaCO3(s)
2Na+ + CO3-2 + Ca+2 + 2Cl- → 2Na+ + 2Cl- + CaCO3(s)
Ca+2 + CO3-2 → CaCO3(s)
As observed there was a color change and solid precipitate noted, of which the calcium and carbonate ions. The sodium and chlorine are cancelled, as spectator
Objective: Classify the chemical reaction through observation, which each reagent produce when mixed with another reagent. After careful observation, be able to prove each observation using the net ionic equation.
Background: First, a double-replacement reaction is when two cations in different compound switch anions, AX + BZ → BY. If either compounds are insoluble a precipitate occurs, and if there is no precipitate formed there is no reaction. Also, not all ionic compounds are soluble in water, and there are a few solubility rules that need to be followed (see Chapter 8 in book). Second, there is also something known as a neutralization reaction, here the reaction is between …show more content…
This left us with the silver and chlorine which yield us silver chloride which is a solid. We did note on our observation that we had a change in color and a solid precipitate.
3. Na2CO3(aq)+ HCl(aq) → NaCl(aq) + HCO3(aq)
Na2CO3 + 2HCl → 2NaCl + H2O + CO2(aq)
2Na+ + CO32- + 2H+ + 2Cl- → 2Na+ + 2Cl- + H2O + CO2
CO32- + 2H+ → H2O(l) + CO2(g)
With this reaction the carbonate and the diatomic hydrogen combined together to make the bubbling effect that we had noted. This leaves us with the water molecule with the sodium chloride dissolved in it with the carbon dioxide gas bubbles.
4. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
Na+ + OH- + H+ + Cl- → Na+ + Cl- + H2O(l)
OH- + H+ → H2O
This reaction with a strong acid, as noted, released heat, which we call an exothermic reaction.
5. BaCl2(aq) + H2SO4 → BaSO4(s) + 2HCl
Ba+2 + 2Cl- + 2H+ + SO4-2 → BaSO4(s) + 2H+ + 2Cl-
Ba+2 + SO4-2 → BaSO4(s)
Here we have Hydrogen and chlorine as spectator ions. One of the solubility rules is that sulfates are soluble except in Barium. During observation we noted a color change in liquid though not a solid …show more content…
NH3 + H2O+ H2SO4 → (NH4)2 SO4 + 2H2O
2NH4OH + H2SO4 → (NH4)2 SO4 + 2H2O
2NH4+ + OH- + 2H+ + SO4-2 → 2NH4+ + SO4-2 + 2H2O
OH- + 2H+ → 2H2O(l)
Aqueous ammonia is ammonia in water. Aqueous ammonia reacts with sulfuric acid, which then forms the salt ammonium sulfate and water. This is a neutralization reaction.
7. CuSO4 + Zn(NO3)2 → Cu(NO3)2 + ZnSO4
Cu+2 + SO4-2 + Zn+2 + 2NO3- → Cu+2 + 2NO3- + Zn+2 + SO4-2
All are cancelled out as spectator ions, so as observed there was no reaction that took place.
8. Na2CO3 + CaCl2 → 2NaCl + CaCO3(s)
2Na+ + CO3-2 + Ca+2 + 2Cl- → 2Na+ + 2Cl- + CaCO3(s)
Ca+2 + CO3-2 → CaCO3(s)
As observed there was a color change and solid precipitate noted, of which the calcium and carbonate ions. The sodium and chlorine are cancelled, as spectator