Chemical Equation: Dissociating PbBr2 - Ksp of 6.3E-6

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In summary, the Ksp of lead (II) bromide is 6.3E-6. When a large amount of PbBr2 is placed in water, it will dissociate into lead and bromine ions. The chemical equation for this dissociation is PbBr2 (s) ⇌ Pb2+ (aq) + 2Br- (aq). The Ksp applies to this equilibrium, which is reached when the amount of dissolved Pb2+ and Br- ions reaches a certain concentration. Therefore, to solve this problem, you would need to calculate the concentration of these ions at equilibrium using the Ksp value.
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kokenwa
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the Ksp of lead (II) bromide is 6.3E-6. A large amount of PbBr2 sits at the bottom of a beaker with water above it. Equilibrium is reached. Write the chemical equation fo rthe dissociation of lead II bromide as it dissolves for which the Ksp applies.


-How would i go about solving this problem?
 
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What are the ions in PbBr2?
 
  • #3
there are none. it just shows PbBr2
 
  • #4
kokenwa, rethink eli64's question. PbBr2 is an ionic compound, so you should be able to answer his question. Also, PbBr2 is slightly soluble, therefore you should think through to your original question.
 

FAQ: Chemical Equation: Dissociating PbBr2 - Ksp of 6.3E-6

What is the chemical equation for dissociation of PbBr2?

The chemical equation for the dissociation of PbBr2 is PbBr2 ⇌ Pb2+ + 2Br-.

What is the meaning of Ksp in relation to PbBr2?

Ksp, or the solubility product constant, is a measure of the maximum amount of a substance that can dissolve in a solvent at a particular temperature. In the case of PbBr2, Ksp is 6.3E-6, indicating that it has a low solubility in water.

How is Ksp calculated for PbBr2?

The Ksp for PbBr2 can be calculated by multiplying the concentrations of the dissociated ions, Pb2+ and Br-, raised to their respective stoichiometric coefficients. In this case, it would be [Pb2+][Br-]2 = 6.3E-6.

What factors can affect the solubility of PbBr2?

The solubility of PbBr2 can be affected by factors such as temperature, pH, and the presence of other ions. For example, an increase in temperature can increase the solubility of PbBr2, while the presence of other ions can decrease its solubility.

What is the significance of the Ksp value for PbBr2?

The Ksp value for PbBr2 gives us important information about its solubility in water. A lower Ksp value indicates a lower solubility, meaning that PbBr2 is less likely to dissolve in water. This information is useful for predicting the behavior of PbBr2 in various solutions and reactions.

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