K2+1CO32–(aq) + Sr2+(NO3–)2(aq) → SrCO3(s) + 2K+NO3–(aq). What is the net ionic equation for the reaction?
a) 2K+(aq) + 2NO3–(aq)
b) 2K+1(aq) + CO32–(aq) + Sr2+(aq) + 2(NO3–)(aq) → SrCO3(s) + 2K+(aq) + 2NO3–(aq)
c) This is a combustion reaction so there is no net ionic equation
d) CO32–(aq) + Sr2+(aq) → SrCO3(s)
b is the total ionic equation. Cancel the items on the left that appear on the right to obtain d which is the net ionic equation.
@DrBob222 thank you
To determine the net ionic equation for the given reaction, we need to first write the balanced molecular equation and then separate the soluble compounds into their respective ions.
The balanced molecular equation is:
K2CO3(aq) + Sr(NO3)2(aq) → SrCO3(s) + 2KNO3(aq)
Now, let's write the complete ionic equation by breaking down the soluble compounds into their ions:
2K+(aq) + CO32–(aq) + Sr2+(aq) + 2NO3–(aq) → SrCO3(s) + 2K+(aq) + 2NO3–(aq)
In the complete ionic equation, we can see that the two potassium (K+) and two nitrate (NO3-) ions appear on both sides of the equation. These ions do not take part in any chemical change and are referred to as spectator ions.
Therefore, the spectator ions can be canceled out to obtain the net ionic equation:
CO32–(aq) + Sr2+(aq) → SrCO3(s)
Hence, the correct answer is (d) CO32–(aq) + Sr2+(aq) → SrCO3(s).