Predict the prdeucts of the following acid/base and precipitation reactions and balance the equations.
Remeber to indicate (s), (l) or (aq
Q1. HCI(aq) + Mg(OH)2(aq)---->
Q2. Pb(NO3)2(aq)+ Na2S (aq)--->
Q3. write the ionic equation for question 2.
1. acid + base = salt + water
2HCl + Mg(OH)2 ==> 2H2O + MgCl2
You add the phases.
2.
Pb(NO3)2 + Na2S ==> PbS(s) + 2NaNO3(aq)
You add the other phases.
3.
Pb^2+(aq) + S^2-(aq) ==> PbS(s)
To predict the products of acid/base reactions and precipitation reactions, we need to follow a series of steps. Let's go through each question and find the answers:
Q1. HCI(aq) + Mg(OH)2(aq) --->
Step 1: Identify the acid and base
In this case, the acid is hydrochloric acid (HCI) and the base is magnesium hydroxide (Mg(OH)2).
Step 2: Swap the partners
The hydrogen ion (H+) from the acid swaps with the hydroxide ion (OH-) from the base. This gives us the predicted products: H2O and MgCl2.
HCI(aq) + Mg(OH)2(aq) ---> H2O(l) + MgCl2(aq)
Step 3: Check the states
Based on their solubilities, H2O is a liquid (l) and MgCl2 is an aqueous solution (aq).
Q2. Pb(NO3)2(aq) + Na2S(aq) --->
Step 1: Identify the reactants
In this case, we have lead nitrate (Pb(NO3)2) and sodium sulfide (Na2S).
Step 2: Swap the partners
The lead ion (Pb2+) from the lead nitrate swaps with the sulfide ion (S2-) from sodium sulfide. This gives us the predicted products: PbS (lead sulfide) and NaNO3 (sodium nitrate).
Pb(NO3)2(aq) + Na2S(aq) ---> PbS(s) + NaNO3(aq)
Step 3: Check the states
Based on their solubilities, PbS is a solid (s) and NaNO3 is an aqueous solution (aq).
Q3. Ionic equation for question 2.
To write the ionic equation, we need to break down all the soluble compounds into their respective ions.
Pb(NO3)2 (aq) + Na2S (aq) ---> PbS (s) + 2NaNO3 (aq)
Now, write the net ionic equation by removing the spectator ions (the ions that appear on both sides of the equation unchanged).
Pb2+ (aq) + S2- (aq) ---> PbS (s)
So, the net ionic equation for question 2 is Pb2+ (aq) + S2- (aq) ---> PbS(s).