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:

\( \ce{H2C2O4} \) (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., \( \ce{H2C2O4 \xrightarrow{light} CO2 + CO + H2O} \) or other photodegradation reactions). As the solute (\( \ce{H2C2O4} \)) decomposes, its amount in the solution decreases while the solvent (water, assuming aqueous solution) remains relatively constant. Concentration is defined as the amount of solute per unit volume of solution (\( C=\frac{n}{V} \), where \( n \) is moles of solute and \( V \) is volume of solution). Since \( n \) decreases and \( V \) is approximately constant (neglecting small volume changes from decomposition - related effects), the concentration will decrease.

Answer:

The concentration of the \( \ce{H2C2O4} \) solution will decrease. This is because oxalic acid (\( \ce{H2C2O4} \)) 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 (\( \ce{H2C2O4} \)) to decompose. As the amount of solute decreases (while the volume of the solution remains relatively constant), the concentration (amount of solute per unit volume) decreases.