What is the molar solubility of pbbr2 in 0.500 m kbr solution?

The molar solubility of PbBr₂ in 0.500 KBr solution is 2.64 × 10⁻⁵ M

PbBr₂ is an ionic compound that dissociates in water to produce lead ions and Bromine ions.

The dissociation reaction can be expressed  as:

The solubility product constant can be written as:

If  

where;

In a 0.500 kBr solution;

Assuming that x = 0; since it is too small than 0.500

∴

x = 2.64 × 10⁻⁵ M

Therefore, we can conclude that the molar solubility of PbBr₂ in 0.500 KBr solution is 2.64 × 10⁻⁵ M

Learn more about solubility product constant here:

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

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