When acetone is added to saturated sodium chloride, the equilibrium shifts toward the right. What is the role of acetone in shifting the equilibrium toward the right? any help would be appreciated. My TA is of no use in explaining our lab experiments. thanks
To be quite honest about it, this is a new one on me; however, I would think that the answer is that acetone is much more soluble in water than NaCl (acetone is miscible in all proportions with water) so there is "less water available to dissolve the salt." Does that sound logical?
Yes, it does. Thank you!
When acetone is added to saturated sodium chloride (NaCl), it does not directly affect the equilibrium between sodium chloride and its ions. The role of acetone in shifting the equilibrium toward the right in this specific case is related to its ability to solvate the sodium and chloride ions present in the solution.
Acetone is a polar solvent that can interact with the sodium and chloride ions through dipole-dipole interactions and ion-dipole interactions. As a result, the solubility of the sodium chloride increases in the presence of acetone, allowing more sodium and chloride ions to dissolve.
By increasing the concentration of dissolved sodium and chloride ions, the equilibrium shifts toward the right to replenish the ions in solution and maintain the saturation. In other words, to counteract the increase in dissolved ions, more solid salt will dissolve until a new equilibrium is established.
It is important to note that the effect of acetone on shifting the equilibrium depends on the specific system and conditions being investigated. In some cases, acetone may have little to no effect on the equilibrium, while in others, it may have a more significant impact.
If you have any further questions, feel free to ask!
In order to understand the role of acetone in shifting the equilibrium toward the right when added to saturated sodium chloride, we need to consider a few concepts.
Firstly, let's clarify the terms "equilibrium" and "saturated sodium chloride". In a chemical reaction, equilibrium occurs when the forward and reverse reactions are happening at the same rate, resulting in no net change in the concentration of reactants and products over time. On the other hand, saturated sodium chloride refers to a solution that contains the maximum amount of dissolved sodium chloride at a given temperature, where no more can dissolve.
Now, when acetone is added to saturated sodium chloride, it can affect the equilibrium by what is called the "common ion effect". Acetone, which is a solvent, can dissociate ionic compounds such as sodium chloride, breaking them apart into their individual ions. Sodium chloride dissociates into sodium ions (Na+) and chloride ions (Cl-).
By adding acetone, which contains no common ions with sodium chloride, the concentration of chloride ions in the solution is decreased. According to Le Chatelier's principle, the equilibrium will shift to the right to counteract this decrease in chloride ion concentration.
In this case, shifting the equilibrium to the right means that more sodium chloride will dissolve to produce more sodium ions and chloride ions. This helps to restore the concentration of chloride ions back to its original value, counteracting the effect of acetone.
To summarize, when acetone is added to saturated sodium chloride, it decreases the concentration of chloride ions in the solution. This change in concentration triggers the equilibrium to shift to the right, causing more sodium chloride to dissolve and restoring the concentration of chloride ions back to its original value.
I hope this explanation helps you understand the role of acetone in shifting the equilibrium toward the right. If you have any further questions, please feel free to ask.