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.

ppb = µgL

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

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp. Or if you need more Ksp practice, you can also practice Ksp practice problems.

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Based on our data, we think this problem is relevant for Professor Cabirac's class at ASU.