That approach is similar to that used for using a calcium hydroxide solution. Keep excess solids in the solution and the supernatant will be at its saturation limit. The only problem is that the dissolved content varies with temperature.
Thanks for good feedback:
Yes that's true the solubility change with temp, but the solution will remain saturated as long as the crystal layer is intact.
Solubility for CaCl2 is equal 74.5 g/100 mL at 20 °C and 100g/100 mL at 30 °C.
I do not have detailed values between 20C and 30C. Maybe you have Martin?
Due to lack of detailed data between 20C & 30C we can assume the following:
The solubility function for CaCl2 in water is a curved function with respect to temp.
For the sake of simplicity we can assume that the function is linear, to get a estimate that is
good enough for home brewing:
Y=kx + A where A=23,5 & k=2,55 between 20C and 30C
20 Celcius: 74,5g = (2,55g/C)*20C + 23,5g
25 Celcius: 87,25g = (2,55g/C)*25C + 23,5g
30 Celsius: 100g = (2,55g/C)*30C + 23,5g
I forgot to mention that as long as the crystal layer is intact, it will also take care of eventually CO2 seeping into the solution.
I hope it is not improper to ask you to read a thread recently I started regarding "pH creep during mashing" at this forum.
I'm very interested to hear your thoughts.