dissocation reactions are endothermic so the forward reaction is endo so the solubility increases when the temp increases as it shifts to the right (the endo reaction) because the solid ionic lattice (magnesium chloride) dissociates into its aqueous ions which increases the solubility. so idk how its a decrease haha
The question stated that solubility is defined as the amount of solid ready to dissolve in a solvent ( in this case, water). Hence as more MgCl2(s) is being produced, solubility increases.
Aqa were sly with this one like Q1A
What?? So solubility increases? I don't understand what you mean...?
Plot a graph of concentrations and absorption rates using known concentrations of KMnO4 Then set up colorimeter and place unknown sample and see what it's absorption rate is Use the absorption rate on the graph and go across until you find the concentration
first said about how MnO4- ions are coloured and the rest arent ( just as an intro). make up solutions of known conc. Measure absorption. plot graph of results, then use the absorption for the unknown conc one to work out the concentration ( extrapolation) .