Ksp Video Lessons

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# 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

###### FREE Expert Solution

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