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First, the alloy $(0.5$ to $\pu{2 g})$ should be treated by $\pu{10 mL}$ nitric acid $32\,\%.$ All metals will get dissolved, except tin and silicon, which will be transformed into insoluble dioxide $\ce{SnO2}$ or $\ce{SiO2}$. Dilute in $\pu{100 mL}$ hot water. $\ce{SiO2 + SnO2}$ will make a gelatinous precipitate, that can be eliminated by filtration. Add $\...
14
The state of a compound, solid, liquid, or gaseous is a property which is unrelated to the property / strength of a Brønsted or Lewis acid of said compound. Thus, you can not infer from its physical appearance if an acid is safe enough to be touched by skin; it may be irritant / corrosive even in absence of water (e.g., p-TsOH as a solid acid, triflic acid ...
6
The problem is that there are not many alkaline stains you will find on household objects. Professor Robert Winston just did a demo for attracting attention of the public towards science (so-called outreach experiments). He simply used an acid-base indicator, perhaps thymolphthalein, which is blue in basic medium and colorless in slightly acidic or even in ...
5
Boric acid is a very weak acid with a $\mathrm{p}K_\mathrm{a}$ value of 9.2 and does not dissociate in aqueous solution as a Brønsted acid. Yet, in aqueous solutions, it acts as a Lewis acid by accepting a hydroxyl ion to form the tetrahydroxyborate ion $(\ce{B(OH)4-})$, as confirmed by Raman spectroscopy (Ref.1):
$$\ce{B(OH)3 + 2H2O <=> B(OH)4- + H3O+}...
3
During neutralization of the buffer by a strong base solution, there are ongoing three reversible reactions, maintaining three equilibria:
$$
\begin{align}
\ce{H2O + A- &<=> OH- + HA} &\quad K_\mathrm{b} &= \frac{\ce{[OH-][HA]}}{\ce{[A-]}} \tag{1}\\
\ce{H2O &<=> OH- + H+} &\quad K_\mathrm{w} &= \ce{[H+][OH-]} \tag{2}\\
\...
2
Fresenius' analytical scheme is also one possibility, although it is not as direct. More information can be found in Harvey's Analytical Chemistry 2.1 Libretext. I bring this up to highlight that even though this is a classical technique, it is still mentioned in some analytical textbooks still in active use.
2
I do not see any reason why the following reaction cannot take place, which will consume $\ce{[B(OH)4]-}$ and the concerned reaction will move in forward direction to increase the acidity of orthoboric acid$^1$.
According to wikipedia, "With polyols containing cis-vicinal diols, such as glycerol and mannitol, the acidity of the boric acid solution is ...
1
Which of these functional groups is soluble in aqueous HCl and/or NaOH?
Functional groups don't have solubility. Their presence in a compound, however, can have an effect on solubility.
My approach before was this : Esters do not dissolve in cold aqueous bases or acids, nor do amides or alcohols. Amines dissolve in aqueous acids. Phenols and Carboxylic ...
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