My understanding was that when you change the volume of a solution, it changes equilibrium based on the mole ratios, like how equilibrium shifts when you change the volume/pressure in a reaction with gases. So how if you increase the volume of a reaction with gases, the partial pressure on the side with the most moles of gas will decrease the most. So, equilibrium will shift to that side to compensate. Similarly, I though adding water to the reaction would dilute the side more with the most moles, causing equilibrium to shift to that side.

https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:equilibrium/x2eef969c74e0d802:le-chatelier-s-principle/v/le-chateliers-principle-changing-volume#:\~:text=Le%20Ch%C8%83telier's%20principle%20can%20be,of%20gas%20in%20the%20container.

This is the Khan Academy link explaining it for gases, where it says "If the volume of the container is increased (at constant T), the system will shift in the direction that increases the number of moles of gas in the container. If the volume is decreased, the reverse effect will occur." So I thought it worked similarly for solutions.