Question

1. will the concentration of the h₂c₂o₄ solution increase or decrease if the solution is stored in a clear bottle in a lighted room? briefly explain.

Explanation:

$H_2C_2O_4$ (oxalic acid) is photosensitive, meaning it can decompose when exposed to light. Storing it in a clear bottle in a lighted room allows light to reach the solution, causing the oxalic acid to decompose (e.g., into $CO_2$, $CO$, and $H_2O$). As the amount of $H_2C_2O_4$ solute decreases while the volume of the solution (solvent) remains relatively constant (assuming no significant evaporation), the concentration (amount of solute per unit volume of solution) will decrease.

Answer:

The concentration of the $H_2C_2O_4$ solution will decrease. This is because oxalic acid ($H_2C_2O_4$) is photosensitive and decomposes when exposed to light. Storing it in a clear bottle in a lighted room exposes the solution to light, causing the solute ($H_2C_2O_4$) to decompose, reducing the amount of solute while the solvent volume remains relatively constant, thus lowering the concentration.