[tvtokyo]

If I have a salt KHC4H4O6 of Mr = 188.2
and given the solubility of the salt is 3.6485 × 10^3 kgsalt/kgwater
How do I convert it to mol/dm^3 ?
Thanks!

[Borek]

In general - you can't without knowing the density of the solution.

the solubility of the salt is 3.6485 × 10^3 kgsalt/kgwater

Really? Over three metric tons per kg of water?

[tvtokyo]

Yes I attached the image , what if we assume the density of water being 1000kg/m^3

[Borek]

Perhaps it should read 10^-3 kg/kg of water, potassium hydrogen tartrate solubility is so low it precipitates out from the wine, that wouldn't be possible with solubility in the given range.

Assuming density of 1 kg/1L just convert mass of the tartrate dissolved per 1 kg of water to moles and that will be your reasonably accurate molar concentration.

[mjc123]

The table says 10³ S = 3.6485 kg/kg. That means S = 3.6485 x 10^-3 kg/kg

[Borek]

The table says 10³ S = 3.6485 kg/kg. That means S = 3.6485 x 10^-3 kg/kg

Thanks, you are probably right.

I think I can think of a more confusing way of expressing this information, but I don't see a single reason to do so