Problem: A concentration of 10-100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Using Ksp values from Appendix D in the textbook, calculate the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium withAgBr

FREE Expert Solution

We are being asked to calculate the equilibrium concentration of Ag+ in ppb that will exist in equilibrium with AgBr.

Recall: Parts per billion (ppb) is the number of units of mass of a solute per 1000 million units of total mass.

Its unit is in µg/L or micrograms per liter.

Since AgBr is an ionic compound, it forms ions when dissociating in water.

The dissociation of AgBr in water is as follows:

AgBr(s) ⇋ Ag+(aq) + Br-(aq)

We can construct an ICE Chart for the dissociation of AgBr.

Remember that solids are ignored in an ICE Chart.

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Problem Details

A concentration of 10-100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Using Ksp values from Appendix D in the textbook, calculate the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium with

AgBr