Question

Using water, how could you distinguish between the white solids kcl an pbcl2

Answer 1

KCl and PbCl2 both are salts having the same white color, however, potassium salts are soluble in water while lead salts are not.
This means that KCl is soluble in water while PbCl2 is not.

So, to distinguish between them, add the same amount of each salt in a beakers containing water (each salt in a separate beaker of course), ans shake the beaker or steer it.
The salt that dissolves in water would be KCl while the salt that doesn't dissolve in water would be PbCl2.

Answer 2

Both the white solids, KCl and ${\mathbf{PbC}}{{\mathbf{l}}_{\mathbf{2}}}$ can be distinguished by dissolving them in water.

Further Explanation:

Solubility rules:

1. The common compounds of group 1A are soluble.

2. All the common compounds of ammonium ion and all acetates, chlorides, nitrates, bromides, iodides, and perchlorates are soluble in nature. Only the chlorides, bromides, and iodides of ${\text{A}}{{\text{g}}^+}$, ${\text{P}}{{\text{b}}^{2+}}$, ${\text{C}}{{\text{u}}^+}$ and ${\text{Hg}}_2^{2+}$ are not soluble.

3. All common fluorides, except for ${\text{Pb}}{{\text{F}}_{\text{2}}}$ and group 2A fluorides, are soluble. Moreover, sulfates except ${\text{CaS}}{{\text{O}}_{\text{4}}}$, ${\text{SrS}}{{\text{O}}_{\text{4}}}$, ${\text{BaS}}{{\text{O}}_{\text{4}}}$, ${\text{A}}{{\text{g}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}$ and ${\text{PbS}}{{\text{O}}_{\text{4}}}$ are soluble.

4. All common metal hydroxides except ${\text{Ca}}{\left({{\text{OH}}}\right)_{\text{2}}}$, ${\text{Sr}}{\left({{\text{OH}}}\right)_{\text{2}}}$, ${\text{Ba}}{\left({{\text{OH}}}\right)_{\text{2}}}$ and hydroxides of group 1A and that of transition metals are insoluble in nature.

5. All carbonates and phosphates, except those formed by group 1A and ammonium ion, are insoluble.

6. All sulfides, except those formed by group 1A, 2A, and ammonium ion are insoluble.

7. Salts that contain ${\text{C}}{{\text{l}}^-}$, ${\text{B}}{{\text{r}}^-}$ or ${{\text{I}}^-}$ are usually soluble except for the halide salts of ${\text{A}}{{\text{g}}^+}$, ${\text{P}}{{\text{b}}^{2+}}$ and ${\left({{\text{H}}{{\text{g}}_2}}\right)^{{\text{2+}}}}$.

8. The chlorides, bromides, and iodides of all the metals are soluble in water, except for silver, lead, and mercury (II). Mercury (II) iodide is water-insoluble. Lead halides are soluble in hot water.

9. The perchlorates of group 1A and group 2A are soluble in nature.

10. All sulfates of metals are soluble, except for lead, mercury (I), barium, and calcium sulfates.

KCl and ${\text{PbC}}{{\text{l}}_{\text{2}}}$ both are the chloride salts that are white in color. According to the solubility rules, KCl is a soluble salt whereas ${\text{PbC}}{{\text{l}}_{\text{2}}}$ is an insoluble one and forms precipitate.

KCl and ${\text{PbC}}{{\text{l}}_{\text{2}}}$ can be distinguished by dissolving both the salts separately in water. The salt that forms precipitates in water is ${\mathbf{PbC}}{{\mathbf{l}}_{\mathbf{2}}}$ while the one that dissolves completely in water is KCl. This way, both solids can be distinguished.

Learn more:

1. Identify the precipitate in the reaction: brainly.com/question/8896163

2. What type of reaction occurs by mixing barium sulfide and sulfuric acid? brainly.com/question/5464325

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: KCl, PbCl2, white solids, precipitate, water, solubility rules, soluble, insoluble, dissolving, salts, chlorides, sulfates, bromide, iodide, carbonates, hydroxides.