The net ionic equation is Ag+(aq) + I- --> AgI(s)
The sodium (Na+) and nitrate (NO3-) are spectators as always.
Potassium nitrate and a precipitate of Silver iodide are formed
A precipitate of Lead iodide and Potassium nitrate are formed
If you add iodide (iodine ions) to Acidfied Silver Nitrate, a pale yellow precipitate is formed. This precipitate is Silver Iodide (AgI).
A precipitate of yellow Lead iodide and Sodium nitrate are formed
A yellow Lead(II) iodide precipitate
Potassium nitrate and a precipitate of Silver iodide are formed
A precipitate of Lead iodide and Potassium nitrate are formed
If you add iodide (iodine ions) to Acidfied Silver Nitrate, a pale yellow precipitate is formed. This precipitate is Silver Iodide (AgI).
A precipitate of yellow Lead iodide and Sodium nitrate are formed
Produces Silver iodide precipitate and Sodium nitrate
A yellow Lead(II) iodide precipitate
Chloride and iodide ions can be distinguished by the colour of their precipitate which are formed by treatig it with silver nitrate solution.
When combined, these two compounds produce a precipitate of Silver iodide and Strontium nitrate.
A yellow precipitate of silver iodiode (AgI) is formed.
Pb(NO3)2(aq) + 2NaI(aq) → PbI2(s) + 2NaNO3(aq) Aqueous lead II nitrate reacts with aqueous sodium iodide to form solid lead II iodide precipitate and aqueous sodium nitrate.
In the reaction: Lead (Ⅱ) Nitrate + Potassium Iodide → Potassium Nitrate + Lead (Ⅱ) Iodide.. all nitrates are soluble and lead(ii)iodide is insoluble.
Aqueous lead nitrate plus aqueous sodium iodide produce solid lead iodide and aqueous sodium nitrate.