what mass of calcium oxalate can be dissolved in 180 ml of distilled water before a precipitate forms?

Melissa you should probably just ask Mr Earls because apparently anyone doing the question has no idea what to do

ksp = [Ca][C2O4]

2.3*10^(-9) = x^
4.8*10^-5 = x
now sub that in as C in n = cv
then convert that answer to mass (m = n*Mm)
and that's the final answer

1.105*10^-3 g

that's the final answer

To determine the mass of calcium oxalate that can be dissolved in 180 mL of distilled water before a precipitate forms, we need to know the solubility of calcium oxalate in water. The solubility of a compound is typically given in terms of grams of solute that can dissolve in a given amount of solvent (in this case, water).

Unfortunately, the solubility of calcium oxalate is not provided in the question. As an AI, I don't have real-time access to databases or the internet, so I can't provide you with the specific solubility value for calcium oxalate. However, I can guide you through the general process to determine the solubility and subsequently the mass that can dissolve.

1. Look for the solubility of calcium oxalate in water. You can check chemical databases, reference books, or reliable online sources such as scientific journals or websites of reputable institutions. Search for the solubility value specifically for calcium oxalate, as it may differ from other oxalates.

2. Once you find the solubility value, it may be given in either grams per liter (g/L) or grams per milliliter (g/mL). If it is given in g/L, convert it to g/mL. Divide the given solubility value by 1000 since there are 1000 mL in a liter.

3. Use the solubility value you found to calculate the maximum mass that can dissolve in 180 mL of distilled water. Multiply the solubility (in g/mL) by the volume of water (180 mL). This will give you the maximum mass that can dissolve in the given volume.

Keep in mind that this calculation assumes ideal conditions and does not account for factors like temperature or the presence of other solutes that may affect solubility. It's always advisable to consult reliable sources for accurate solubility information in specific experimental conditions.