New answers tagged aqueous-solution
-1
Per Science Direct on Baking Soda, to quote:
All baking powders on the retail market are formulated to yield at least 12% (required by law), usually more nearly 14%, carbon dioxide when water is added and heat is applied. Acid salts, being more stable than acids as such, are combined in proper proportions with sodium bicarbonate; corn starch is added for ...
1
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:
$$\ce{H2SO3 + ...
0
One direct argument supporting answer (a) is that aqueous aluminum ions, in the presence of nitrate anions, apparently can undergo polynuclear hydrolysis liberating $\ce{H+}$, albeit as a function of the solution's pH and concentration.
Per of an article 'Hydrolysis of aluminum(III) ion in sodium nitrate medium', to quote from an abstract:
At a definite ...
1
According to a relevant reference (Ref.1) Following reactions happen when sodium hypochlorite and sodium dichloro-s-triazinetrione dissolve in water, respectively:
$$\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(...
0
$1$ mole of sodium dichloro-s-triazinetrione weighs $220$ g, and is able to liberate $2$ moles of $Cl_2$ in water. If you use the same substance as dehydrate, one mole will weigh $256$ g.
By comparison, $1$ mole of bleach $NaClO$ ($74.5$ g) is able to yield $1$ mole $Cl_2$ in water.
So if you know the mass m of $NaClO$ that you are adding to your water, ...
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.
3
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 ...
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