What does
$\ce{Pb(NO3)2 + KI}$
form?
Answer
This is just a metathesis (double replacement) reaction.
We know that nitrates are soluble, and alkali metals are soluble (at least in these general cases).
Let's ignore balancing for now, and do that last.
$\ce{Pb(NO3)2 + KI -> Pb^{+2} + NO3^- + K+ + I-}$
$\ce{Pb^{+2} + NO3- + K+ + I- -> PbI2 + KNO3}$
But the $\ce{KNO3}$ is also soluble, and would dissociate.
$\ce{Pb^{+2} + NO3- + K+ + I- -> PbI2 + K+ + NO3-}$
Evidently, we can cancel out the spectator ions $\ce{K+}$ and $\ce{NO3-}$ and are left with a net ionic equation (which is easily balanced).
$\ce{Pb^{+2} + 2I- -> PbI2}$
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