You must have a table or graph (or something) in your text/notes that gives the solubility at 30 C and 60 C. I don't have those tables available. If you want to type that info in I can show you how to work the problem.
See your other post.
I would take the average of 0.084 and 0.057 and see if that gets close to pH = 2.5. Avg = about 0.07% = 0.007g/100g mols H3PO4 = 0.07/98 = about about 7E-4 and that in 0.1L (if density is about 1.0) that makes 7E-3M Then H3PO4 ==> H^+ + H2PO4^- I.....7E-3......0.......0 C.....
#eq = N x L = ? You would do well to post new questions at the top of the pager and not piggy back onto other questions. Most of the time those piggy-backed questions get lost in the shuffle.
volume of cylinder is pi*r^2*h mass H2O = volume x density mols H2O = mass H2O/molar mass H2O
Yes except when it is atomic O or ozone, O3. It is diatomic in its normal state at room T and P.
(H2O) = 1/11 = 0.0909M (CO) = 1/11 = 0.0909 (0.422/11) = 0.0384 ......CO(g) + H2O(g)<->CO2(g) + H2(g) I...0.0909...0.0909.....0 C....-x........-x.......x E....0.0909-x.0.0909-x..x The problems tells you that x = 0.0384. Use that to determine (CO) and (H2O) ast equilibriu...
See your SO2 problem.
Same as SO2 problem.
Substitute the equilibrium value into Kc and solve for the one unknown.