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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 ...

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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.

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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 ...

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Consider (1) for $\ce{Mg(OH)2}$ dissolution equilibrium, (2) for ammonia acido-basic equilibrium. Combining both, you get required concentration of $\ce{NH4+}$. \begin{align} \mathrm{p}K_\mathrm{sp} &= \mathrm{pMg} + 2 \cdot \mathrm{pOH}\tag{1}\\ \mathrm{pOH} &= \mathrm{p}K_\mathrm{b, NH3} + \mathrm{pNH3} - \mathrm{pNH4+} \tag{2}\\ \mathrm{p}K_\...

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Well, acetone is at the same time polar (so it likes water) and lipophilic (so it likes fat). As such, it is a very good solvent.

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Poutnik has given an excellent answer in general for your question. Since you asked about Varsol™ in particular (not white spirit in general), I'd like to give an additional insights for your benefit. Yet you didn't mention the paticular Varsol™ brand so I'll give physical data for all 3 Varsol™ brands avilable. Varsol™ is an ExxonMobil Chemical brand for a ...

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Note that I have never heard about Varsol until now, living in the Central Europe. By searching Wikipedia ( what you could do as well before asking ), I realized the below: Varsol alias White spirit alias many other synonyms, used as a painting solvent, is based on C7-C12 oil hydrocarbons, with density 0.765(type T1), 0.780(type T2), 0.795(type T3) ( ...

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Probably not so much calcium hydroxide, but alkali metal hydroxides mixing with each other in the liquid phase. The pairs $\ce{LiOH-NaOH}$ and $\ce{KOH-NaOH}$ are not only fully miscible, they have been studied as fuel cell electrolytes. The picture below, from the referenced article, shows results for the a range of electrolyte compositions that imply the ...

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Actually, the textbook should remove this question. You should discuss this with your teacher. It will be a service to future students. The heavier elements of group II elements form insoluble sulfates, phosphates and carbonates. Now carbonates display another interesting phenomenon. If you keep bubbling carbon dioxide in into a group II carbonate solution (...

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If you know the phase diagram of the gas, and can calculate the exact pressure the gas should have given the volume outside of the molten salt, you can use the measured pressure/temperature to determine any difference in pressure. Then you can calculate the number of moles of gas that must be absorbed to generate the pressure difference. If the gas is ...

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The solubility data for MgCO3 and Mg(OH)2 are these: for MgCO3 0.01 g/100 mL cold H2O; for Mg(OH)2 0.0009 g/100 mL H2O @ 18C, 0.004 g/100 mL H2O @ 100C (CRC Handbook). The published Ksp data are all over the place: for MgCO3, I have found 10e-5, 6.8 x 10e-6, and 3.5 x 10e-8 (twice). For Mg(OH)2, in the same set of 4 documents, I have 1.8 x 10e-11 (twice), 1....

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