Chem question help asap!!

the solubility of barium oxalate in water at 25 C is 0.090 grams per liter of water. If you shake 10 mg of barium oxalate with 100 ml of water at 25 C, would the resulting solution be saturated, supersaturated or unsaturated? Explain this answer



ok so im thinking it supersaturated, but what confuses me is the temperature ? can you have a supersaturated solution , which means holding more than the maximum amount, without it being heated ? a little confused about this specifically. Rationally i wouldnt think its saturated because saturated means holding the maximum amount, and i think the calculations reveal the ratios;
0.10g:1L to 0.090g:1 L <---- which shows more than the solubility

i have an exam on monday (tomorrow) so someone please explain with clarity!!
thank you so much <3

Your basic question concerns 10mg BO shaken with 100 mL H2O

Atomic weights: Ba=137, C=12, O=16, BaC2O4=225

Let barium oxalate be called BO. 1 L H2O = 1000 mL H2O Then the solubility is 0.090gBO/1000mLH2O. In that case, 1000mgBO/1gBO and the solubility is 90mg/1000mL.

So, if you shake 10 mg BO with 100 mL H2O, there will be 100 mg/1000 mL. But the solubility is 90mg/1000mL so saturated.

You can't supersaturate a solution just by shaking stuff. So this solution is saturated, with stuff lying on the bottom.