Mayhem said:set up and ICE table for the chemical equation of ##\mathrm{CaC_2O_4}##
Which is in your Relevant Equation. So can start. Wonder what's taking?Borek said:Hint: only concentration of (COO-)2 counts.
Borek said:Taking into account I is zero I don't think that will help much.
Yes. My mistake. My brain completely skipped over important parts of the question.Borek said:Taking into account I is zero I don't think that will help much.
Solubility is the measure of the maximum amount of a substance that can dissolve in a given solvent at a specific temperature and pressure.
When a common ion is present, it decreases the solubility of a substance due to the common ion effect. This is because the common ion competes for the available space in the solvent, making it more difficult for the substance to dissolve.
To calculate the solubility of a substance in the presence of a common ion, you must first determine the solubility product constant (Ksp) of the substance. Then, use the common ion effect equation to calculate the solubility.
A buffered solution is a solution that resists changes in pH when small amounts of acid or base are added. It contains a weak acid and its conjugate base, or a weak base and its conjugate acid, which work together to maintain the pH of the solution.
A buffered solution can affect the solubility of a substance with a common ion by reducing the effect of the common ion. This is because the buffer can bind with the common ion, preventing it from competing with the substance for space in the solvent.