Question

we use the solubility rules to determine the precipitate. the precipitate is the insoluble compound. here are the solubility rules: 1. alkali metal ($li^{+}$, $na^{+}$, $k^{+}$, etc) and ammonium ($nh_{4}^{+}$) salts are generally soluble. exceptions include $li_{2}co_{3}$ and $li_{3}po_{4}$. 2. nitrate ($no_{3}^{-}$) salts are generally soluble. 3. silver ($ag^{+}$) and lead ($pb^{2 + }$) salts are generally insoluble. 4. halide ($cl^{-}$, $br^{-}$, and $i^{-}$) salts are generally soluble. exceptions include $pb^{2+}$, $ag^{+}$, $hg_{2}^{2+}$. 5. carbonate ($co_{3}^{2 - }$), phosphate ($po_{4}^{3 - }$), and hydroxide ($oh^{-}$) salts are generally insoluble. 6. sulfate ($so_{4}^{2 - }$) salts are generally soluble. exceptions include $caso_{4}$, $srso_{4}$, $baso_{4}$, $pbso_{4}$, and $ag_{2}so_{4}$. use the solubility rules to identify which product, $kno_{3}$ or $pbi_{2}$, is insoluble. identify the precipitate as the solid product in the reaction below by entering the correct states of matter into the equation. hint: select (s) for solid to show which product is insoluble according to the solubility rules. the other product is soluble. this means it is aqueous. $pb(no_{3})_{2}$? + $ki$? → $pbi_{2}$? + $kno_{3}$?

Explanation:

Step1: Recall nitrate solubility rule

Nitrate ($\text{NO}_3^-$) salts are generally soluble. So, $\text{KNO}_3$ is soluble as it is a nitrate - potassium salt.

Step2: Recall halide solubility rule

Halide ($\text{Cl}^-$, $\text{Br}^-$, $\text{I}^-$) salts are generally soluble, but salts with $\text{Pb}^{2 + }$ are exceptions. $\text{PbI}_2$ is a lead - iodide salt. Since lead ($\text{Pb}^{2+}$) is an exception for halide salts, $\text{PbI}_2$ is insoluble.

Step3: Write the balanced equation with states

The balanced chemical equation with states of matter is $\text{Pb}(\text{NO}_3)_2(aq)+2\text{KI}(aq)
ightarrow\text{PbI}_2(s) + 2\text{KNO}_3(aq)$

Answer:

The insoluble product is $\text{PbI}_2$. The balanced equation with states is $\text{Pb}(\text{NO}_3)_2(aq)+2\text{KI}(aq)
ightarrow\text{PbI}_2(s) + 2\text{KNO}_3(aq)$