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Ignoring activities, activity coefficients, ionic strength effects, and so on, I get a pH of around 9.3. Given the 1 M concentration, I would not bet a lot of money on this, though. My solution, assuming a more typical solution concentration, is given in the two figures below. Sorry these are figures rather than proper formatting: I have been away for 3 ...


1

According to a relevant reference (Ref.1) Following reactions happen when sodium hypochlorite and sodium dichloro-s-triazinetrione dissolve in water, respectively: $$\ce{NaOCl + H2O -> HOCl + NaOH} \tag {1}$$ $$\ce{NaCl2(NCO)3 + 2 H2O <=> 2 HOCl + NaH2(NCO)3} \tag {1}$$ Hence it is safe to assume that you need only $\pu{0.5 mol}$ of $\ce{NaCl2(...


1

A test kit means a set of solutions for repeated use until the are spent. How many analysis can be done should be noted on the kit package. Paper strips are easier to use, but may not be better for result.


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I agree with Buck Thorn's explanation on $\ce{SO2}$ concentration in aqueous phase. Thus, when dissolve in water (or when is added to water), the initial reaction of $\ce{SO2}$ with water is shown in the following reaction (Ref.1): $$\ce{SO2 (g) + H2O (l) -> H2SO3 (aq)}$$ Then, formed $\ce{H2SO3}$ would stabilize following equilibrium: $$\ce{H2SO3 + ...


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