The Handbook of Chemistry and Physics gives the following data for the solubilit

Question

The Handbook of Chemistry and Physics gives the following data for the solubility of lead (II) bromide in water. 0 degree C: 0.455 g per 100 ml solution 20 degree C: 0.844 g per 100 ml solution 100 degree C: 4.71 g per 100 ml solution What is the concentration of lead (II) bromide in moles per liter in each of these saturated solutions? Using the values from question 3, calculate the solubility product constants for lead(II) bromide at 0, 20, and 100 degree C. Using the values from question 4, calculate delta G for dissolving lead(II) bromide at 0, 20, and 100 degree C. What do the solubility's given in question 3 imply about the sign of delta H for the dissolving of lead(II) bromide? Explain.

Explanation / Answer

The question 3 represents as the temperature increases, the solubility of leadbromide in 100ml water increases.

Hence the solubility increases with temperature.

Hence it is endothermic in nature.

For endothermic reations deltaH is postive.

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