New answers tagged aqueous-solution
9
It is rather:
$$\ce{2 Al + 6 H2O + 2 OH- -> 2 [Al(OH)4]^- + 3 H2 ^}$$where $\ce{OH-}$ comes either from hydroxide dissociation, either from carbonate hydrolysis.
$$\ce{CO3^2- + H2O <=> HCO3- + OH-}$$
The reaction with carbonate would gradually slow down as the carbonate/bicarbonate buffer will kick in.
Initial $\mathrm{pH}$ is ( see notes below ...
-2
Firstly ethanol being an organic compound, tends to dissolve less in polar compounds. But it can form numerous hydrogen bonds in water and hence is soluble in most aqueous solutions.
NaOH is a often considered a moderate base in organic chemistry. If you dissolve ethanol in aq.NaOH , it tends to oxidize the alcohol into its aldehyde which further undergoes ...
2
Sodium bicarbonate is a ionic compound with quite limited solubility in water. Ethanol is worse solvent to dissolve ionic compounds than water is, as it is less polar. Therefore salts have generally worse solubility in ethanol than in water.
0
Molx's answer is very good. However, the way I learned it was a little different and may make more sense to some people. Instead of using 444g of HCl, which is perfectly fine, we can assume we have a sample of 100 g, much like we do in empirical formula calculations as to have every percent be out of 100.
To start, just like Molx mentioned, the maximum ...
0
Displacement reaction of copper by sodium will work well if ethanol is used to precipitate the sodium sulfate. Copper chloride is soluble in ethanol (>50 g/100 mL) while sodium sulfate is not. A mixture of concentrated salts in water, followed by dilution with fair amounts of ethanol will allow recovery of high-purity copper chloride dihydrate after proper ...
0
Sodium trioxocarbonate (iv) pentahydrate, a.k.a washing soda, is an efflorescent crystal containing 10 molecules of water of crystallization in its molecular formula.The molar mass of washing soda comprises a:
carbonate portion of 106 g + pentahydrate portion of 180 g = 286 g/mol.
i.e. 1 mole or 286 g of washing soda contains 106 g
of ...
0
The molar mass of copper (ii) sulfate penta-hydrate is $\pu{249.69 g/mol}$ and that for anhydrous copper(ii) sulfate is $\pu{159.61 g/mol}$. Thus, in $1$ mole of the hydrated substance there are $\pu{159.61 g}$ of copper (ii) sulfate and $5 \times \pu{18.00 g}$ (i.e. $\pu{90.00 g}$) of molecules of water of crystallization.
$\pu{5M}$ copper (ii) sulfate ...
-7
$\ce{OH-}$ can't be reduced. It may only be oxidized by giving an electron at the anode, while $\ce{H+}$ is reduced instead of $\ce{OH-}$.
Secondly, the reducing property of $\ce{H2O}$ is greater than that of $\ce{H+}$ ion. Moreover, it is greater in number than other ions like $\ce{H+}$ ions etc. So it will be preferentially discharged although it is ...
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