Questions: Predict whether the compounds are soluble or insoluble in water. - Insoluble - KNO3 - AgI - NiCO3

Transcript text: Predict whether the compounds are soluble or insoluble in water. $\square$ Insoluble $\square$ $\mathrm{KNO}_{3}$ AgI $\mathrm{NiCO}_{3}$

Solution

Solution Steps

Step 1: Determine Solubility Rules

To predict the solubility of compounds in water, we use general solubility rules:

Nitrates (NO$_3^-$): All nitrates are soluble.
Iodides (I$^-$): Most iodides are soluble, except those of silver (Ag$^+$), lead (Pb$^2+$), and mercury (Hg$_2^{2+}$).
Carbonates (CO$_3^{2-}$): Most carbonates are insoluble, except those of alkali metals (e.g., Na$^+$, K$^+$) and ammonium (NH$_4^+$).

Step 2: Apply Solubility Rules to Each Compound

KNO$_3$: Contains the nitrate ion (NO$_3^-$), which is always soluble.
AgI: Contains the iodide ion (I$^-$) and silver (Ag$^+$), which is an exception and thus insoluble.
NiCO$_3$: Contains the carbonate ion (CO$_3^{2-}$), which is generally insoluble unless paired with alkali metals or ammonium. Nickel (Ni$^2+$) is not an exception.