[NYM]

If I add some more water to a beaker with water+a poorly soluble salt, what'll happen?

My suggestion: Nothing! But I can't quite explain why.
Just to make it easier, I choose AgCl as an example. Anyone?

[Borek]

Imagine you have 1.5 g of weekly soluble salt. Imagine this salt has solubility of 1 g/L. Now imagine you have put it into 1L of water - what happens? Now you pour 1 L of water more. What happens?

[NYM]

Hmm... When 1L of water is added to the salt initially, 1,0 g of the salt will dissolve. Then when I add another liter, all the salt dissolves because it has a solubility of 1g/L - or 2g/2L, right?

[NYM]

Oh I forgot, what if it's easily soluble salt?

[sdekivit]

when the salt is easily soluble than you won't see anything happen, but you must remember that when you add any volume of solvent then the concentration of the salt decreases:

c = n/V --> when V gets higer, c gets lower, thus less mol / L

[Borek]

when the salt is easily soluble than you won't see anything happen

Add two zeros to all numbers but the volumes (ie 100 g/L solubility, 200 g of salt) and think what will happen when you use 1L and 2L of solution. There is no difference between both situations, as even easily soluble salts have solubility limits. Just the final concentrations will be different.

[Donaldson Tan]

Imagine this salt has solubility of 1 g/L. Now imagine you have put it into 1L of water - what happens? Now you pour 1 L of water more. What happens?

1L of water dissolves up to 1g of salt. 2L of water dissolves up to 2g of salt. If you have more water, you can dissolve more salt.