Consider the following reactions: (Chemistry Help)

Hello,
i am a little confused about these and am not sure about which is which. Please explain per questions below. they are probably a little harder then i am making them but i just wanna make sure. thanks so much for your help!

Consider the following reactions:

A) H2SO4 (aq) + Ba(OH)2 (aq) ----> BaSO4 (s) + 2H20

B) 2HCl (aq) + Mg(s) ----> MgCl2 (aq) + H2 (g)

C) Na3PO4 (aq) + 3AgNO3 (aq) ----> 3NaNO3 (aq) + Ag3PO4(s)

D) 3Cu(NO3)2 (aq) + 2Al (s) ----> 3Cu (s) + 2 Al (NO3)3 (aq)

Which of these reactions are:

1) Redox reactions why?

2) Precipitation reactions and why?

3) Neutralization reactions and why?

thanks again!

1) Redox reactions why?

Redox reactions involve one reagent becoming oxidised while the other becoming reduced.

B) is a redox reaction. Mg is originally at 0 oxidation state, therefore its solid form. But upon reacting with HCl, it becomes MgCl2, Mg now has an oxidation state of +2. Mg is then oxidised.
However for H, it is reduced. Its original oxidation state of +1 in HCl is reduced to 0 in H2.

D) is the only other redox reaction. While Cu is reduced from Cu2+ ions to Cu metal, Al is oxidised from Al metal to Al3+ ions.
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2) Precipitation reactions and why?

A)
BaSO4 is insoluble in water as shown in your equation above. It comes as a solid, therefore it is the precipitate.

Same goes for C) and D).
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3) Neutralization reactions and why?

Neutralisation reactions produce only SALT and WATER. If H2 gas is produced, it is no longer a neutralisation reaction, that's why B) is out.

A) is the only neutralisation reaction.