The value of the Solubility Product Constant for lead hydroxide is Write the reaction that corresponds to this Ksp value
The Correct Answer and Explanation is :
The solubility product constant, ( K_{sp} ), for lead(II) hydroxide, ( \text{Pb(OH)}_2 ), can be expressed through the dissolution reaction:
[
\text{Pb(OH)}_2(s) \rightleftharpoons \text{Pb}^{2+}(aq) + 2\text{OH}^-(aq)
]
In this reaction, solid lead(II) hydroxide dissociates into lead(II) ions, ( \text{Pb}^{2+} ), and hydroxide ions, ( \text{OH}^- ), in aqueous solution. The ( K_{sp} ) value is a product of the concentrations of the ions produced, each raised to the power of their stoichiometric coefficients in the balanced equation:
[
K_{sp} = [\text{Pb}^{2+}][\text{OH}^-]^2
]
The solubility product constant is crucial in predicting the solubility of sparingly soluble salts and in analyzing precipitation reactions. It helps determine whether a precipitate will form under given conditions. In the case of ( \text{Pb(OH)}2 ), a low ( K{sp} ) value indicates that it is only sparingly soluble in water. The value of ( K_{sp} ) depends on temperature and the ionic strength of the solution but is generally very small for lead hydroxide, reflecting its limited solubility.
Understanding ( K_{sp} ) is essential in environmental chemistry and industrial processes where lead compounds are involved. For instance, knowing the solubility of lead hydroxide helps in treating and removing lead from wastewater to prevent pollution. In physiological conditions, it informs the risk assessment of lead exposure in human activities and its potential health impacts, such as lead poisoning, which can affect the nervous system and kidney function.
The ( K_{sp} ) also plays a role in the study of chemical equilibria and solubility equilibria, teaching about the dynamic balance between a solid and its dissolved ions and how this balance is influenced by changes in conditions such as pH, temperature, and the presence of other ions.
Now, let’s create an image that visually represents the dissolution of ( \text{Pb(OH)}_2 ) into ( \text{Pb}^{2+} ) and ( \text{OH}^- ) ions in solution.
Here is the prompt I will use for the image generation:
“Visualize the dissolution of lead(II) hydroxide, Pb(OH)2, in water. Show lead(II) hydroxide as a solid white compound at the bottom, gradually dissolving into colorless Pb2+ ions and slightly larger, pale blue OH- ions in a clear aqueous solution. The background should be transparent to emphasize the dissolution process, with annotations indicating the Pb2+ and OH- ions. The image should be detailed enough to use for educational purposes, showing a clear distinction between the solid and dissolved forms.”
Let’s generate this image.
Here is the visual representation of the dissolution of lead(II) hydroxide, ( \text{Pb(OH)}_2 ), in water, showing the transition from the solid compound to the dissolved ions ( \text{Pb}^{2+} ) and ( \text{OH}^- ). This image highlights the process clearly, suitable for educational purposes. You can view and use it to better understand the solubility behavior of lead hydroxide.
