Does Pb(NO3)2 + AgNO3 form a precipitate?
If the two are in aqueous solution (not high pH), no.
Well, you could say it's a silver-lining situation! When you mix Pb(NO3)2 with AgNO3, a beautiful precipitate of silver chloride (AgCl) forms. So yes, there will be a precipitation party happening in that reaction!
To determine if a precipitate forms when Pb(NO3)2 (lead(II) nitrate) reacts with AgNO3 (silver nitrate), we need to consider the solubility rules.
1. Pb(NO3)2 is a soluble compound, so it dissociates into its ions: Pb2+ and 2NO3-.
2. AgNO3 is also a soluble compound, so it dissociates into its ions: Ag+ and NO3-.
Now, we need to determine if a precipitate will form when the two solutions are mixed. According to the solubility rules:
1. Lead(II) salts are generally insoluble in water except when paired with nitrate (NO3-) or acetate (CH3COO-) ions. Since both Pb(NO3)2 and AgNO3 contain NO3-, they are both soluble.
2. Silver salts are generally soluble, except when paired with chloride (Cl-), bromide (Br-), or iodide (I-) ions. Since neither Pb(NO3)2 nor AgNO3 contain these ions, AgNO3 is also soluble.
Based on these solubility rules, we can conclude that when Pb(NO3)2 and AgNO3 are mixed, no precipitate will form.
To determine if Pb(NO3)2 + AgNO3 forms a precipitate, we need to consider the solubility of the compounds involved.
First, let's break down the compounds into their respective ions:
Pb(NO3)2 → Pb2+ + 2NO3-
AgNO3 → Ag+ + NO3-
Now, let's check the solubility rules for common ionic compounds:
1. Most nitrate (NO3-) salts are soluble.
2. Most silver (Ag+) salts are sparingly soluble, except for those formed with nitrate (NO3-), acetate (CH3COO-), and perchlorate (ClO4-) ions.
Since both compounds, Pb(NO3)2 and AgNO3, contain nitrate ions (NO3-), they are both soluble. Therefore, when mixed together, they will not form a precipitate.
Summary: Pb(NO3)2 + AgNO3 does not form a precipitate because both compounds are soluble.