Question

soluble. exceptions include li₂co₃ and li₃po₄.

1. nitrate (no₃⁻) salts are generally soluble.
2. silver (ag⁺) and lead (pb²⁺) salts are generally insoluble.
3. halide (cl⁻, br⁻, and i⁻) salts are generally soluble. exceptions include pb²⁺, ag⁺, hg₂²⁺.
4. carbonate (co₃²⁻), phosphate (po₄³⁻), and hydroxide (oh⁻) salts are generally insoluble.
5. sulfate (so₄²⁻) salts are generally soluble. exceptions include caso₄, srso₄, baso₄, pbso₄, and ag₂so₄.

use the solubility rules to identify which product, kno₃ or pbi₂, 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(no₃)₂ + ki → pbi₂ + ki

Explanation:

Step1: Analyze \(KNO_3\) using solubility rules

Nitrate (\(NO_3^-\)) salts are generally soluble (rule 2). \(KNO_3\) has \(K^+\) and \(NO_3^-\), so \(KNO_3\) is soluble (aqueous, (aq)).

Step2: Analyze \(PbI_2\) using solubility rules

Halide (\(I^-\)) salts: silver (\(Ag^+\)) and lead (\(Pb^{2+}\)) salts are generally insoluble (rule 3 and 4). \(PbI_2\) has \(Pb^{2+}\) and \(I^-\), so \(PbI_2\) is insoluble (solid, (s)).

Step3: Determine states of reactants

\(Pb(NO_3)_2\) and \(KI\) are soluble ionic compounds (nitrate salts and potassium salts are soluble), so they are aqueous (aq).

Answer:

\(Pb(NO_3)_2\) (aq) + \(KI\) (aq) \(
ightarrow\) \(PbI_2\) (s) + \(KNO_3\) (aq) (Note: The original equation had a typo, it should be \(KNO_3\) not \(KI\) as a product. Correcting that, the states are \(Pb(NO_3)_2\) (aq), \(KI\) (aq), \(PbI_2\) (s), \(KNO_3\) (aq))