Question
NaCl(s) + H2O(l) <--> Na(aq) + Cl(aq)
If you added chloride ions to the above equilibrium, what would happen to the concentration of the products, and the concentration of the reactants? I know the equilibrium would shift to the left, and I am guessing the concentration of the products will be greater than the reactants before equilibrium is reached?
If you added chloride ions to the above equilibrium, what would happen to the concentration of the products, and the concentration of the reactants? I know the equilibrium would shift to the left, and I am guessing the concentration of the products will be greater than the reactants before equilibrium is reached?
Answers
The answers to your question are yes and yes. I suppose my first question is to ask how you propose to add chloride? Will you add more sodium chloride to add chloride? Too much sodium chloride and you have a saturated solution.
I think the question was asking for the Cl (aq) ions
And my question is, "How do you add Cl^-?" You can't. You must add it with some cation.
that makes sense, thanks for your help
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