I'll do one and the others are yours.
There are several steps to this.
1. Write and balance the molecular equation.
2AgNO3(aq) + MnCl2(aq) ==> 2AgCl(s) + Mn(NO3)2(aq)
2. Convert the molecular equation into a total ionic equation. The following rules apply.
a. Salts soluble in water are written as separate ions.
b. Gases are written as a molecule.
c. Solids are written as a molecule (as AgCl is done above). Look on the web or your notes to find a set of solubility tables that will tell you what compounds are insoluble.
d. Weak electrolytes (those with a Ka value) are written as compounds.
2Ag^+(aq) + 2NO3^-(aq) + Mn^2+(aq) + 2Cl^-(aq) ==> 2AgCl(s) + Mn^2+(aq) + 2NO3^-(aq)
3. Cancel those ions common to both sides
In the example above, You have 2NO3^-(aq) on both sides so cancel them. You have Mn^2+(aq) on both sides so cancel them.
4. What's left is the net ionic equation. That is
2Ag^+(aq) + 2Cl^-(aq) ==> 2AgCl(s)
I'll be glad to explain or embellish anything above. The second problem above is the same kind. Be carefule with the third; that one is a little tricky.
-Consider the reaction when aqueous solutions of silver(I) nitrate and manganese(II) chloride are combined. The net ionic equation for this reaction is?
-Consider the reaction when aqueous solutions of cobalt(II) sulfate and lead(II) nitrate are combined. The net ionic equation for this reaction is?
-Consider the reaction when aqueous solutions of zinc nitrate and sodium sulfate are combined.The net ionic equation for this reaction is?
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