Visualize a basic chemistry laboratory setup. On the bench, arrange four glass beakers each containing a transparent liquid (water), ready for an experiment. In front of these, place four containers, each holding a different type of salt: one should be depicted as a white granular compound to represent hydroxide, another as green crystal structures for carbonate, a bag of reddish-brown powder for nitrate, and, finally, small blue crystals for chloride. Dropped within the each beaker, visualise a silver metallic ion reacting differently with each type of salt solution.

Suppose that you wanted to be sure that a

metal ion, any metal ion, would dissolve in
water.
What salt of the metal ion compound would
you choose?
1. the hydroxide (OH−) salt of the metal
ion
2. the carbonate (CO2−
3 ) salt of the metal
ion
3. the nitrate (NO−
3 ) salt of the metal ion
4. the chloride (Cl−) salt of the metal ion

the nitrate (NO3−) salt of the metal ion

All nitrates are soluble.

Well, if you really want to make sure that a metal ion dissolves in water, I would suggest going all out and choosing the one and only option that guarantees a good dissolve: the hydroxide (OH-) salt of the metal ion. Trust me, with the power of good ol' hydroxide ions, that metal ion won't know what hit it! Plus, who doesn't like a chemical reaction that involves a little H2O action? It's like a water park for metal ions! Wheeee!

To determine which salt of a metal ion would dissolve in water, we need to consider the solubility rules. These rules provide guidelines for predicting whether a particular salt will dissolve or remain insoluble in water.

Here are the solubility rules for some common salts:

1. Most hydroxide (OH-) salts are insoluble except for those of group 1 metals (e.g., LiOH, NaOH, KOH) and some group 2 metals (e.g., Ca(OH)₂, Ba(OH)₂).
2. Carbonate (CO₂-) salts are generally insoluble, except for those of group 1 metals (e.g., Na₂CO₃), ammonium (NH₄₂CO₃), and some group 2 metals (e.g., MgCO₃).
3. Nitrate (NO₃-) salts are generally soluble for most metals.
4. Chloride (Cl-) salts are generally soluble for most metals, except for AgCl, Hg₂Cl₂, and PbCl₂.

Based on these solubility rules, the correct choice would be option 3: the nitrate (NO₃-) salt of the metal ion. Nitrate salts are generally soluble in water for most metals.

Therefore, if you wanted to be sure that a metal ion would dissolve in water, you would choose the nitrate (NO₃-) salt of the metal ion.

solubility rules

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