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 withAgI

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We’re being asked to determine the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium with AgI.


Since the compound is an ionic compound, it forms ions when dissociating in water. The dissociation of AgI in water is as follows:


The iodide ion, I-, has a charge of -1. Silver then has a charge of +1:

AgI(s) Ag+(aq) + I-(aq)



We will do the following steps to solve the problem:

Step 1: Construct an ICE table

Step 2: Write the Ksp expression

Step 3: Calculate the equilibrium concentration

Step 4: Calculate the concentration in parts per billion

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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

AgI

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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.