All Questions
Tagged with ionic-compounds water
17
questions
-2
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1
answer
227
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Calculating salinity from sodium and chloride in water [closed]
let me start by saying that I am definitely no chemist, so this question might (or might not) seem trivial to all you professionals out there.
I have recently found a brand of carbonated water here in ...
4
votes
0
answers
75
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Dielectric constant for gases possessing van der Waals forces [closed]
I've learnt that water can dissolve ionic bonds because it possesses a high dielectric constant.
In the cases of covalent compounds (especially the non-polar covalent compounds), where the molecules ...
- 65
2
votes
1
answer
970
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Order of solubility of sodium halides and potassium iodide
Order the following ionic compounds in decreasing order according to their ease to dissolve in water.
a) NaBr; b) KI; c) NaF; d) NaCl.
d > a > b > c
a > b > c > d
b > c > d &...
- 57
0
votes
1
answer
167
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When converting between a hydrated electrolyte amount in mass and in milliequivalents (meq), why are the water molecules taken into account?
A textbook I'm reading called "Ansel's Pharmaceutical Calculations, 13th edition" defines the milliequivalent (meq) thus (p. 187):
This unit of measure is related to the total number of ...
- 1,410
8
votes
1
answer
464
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What would superionic water ice look like?
Phys.org's Giant lasers crystallize water with shockwaves, revealing the atomic structure of superionic ice links to
Nature Physics: Experimental evidence for superionic water ice using shock ...
- 5,900
7
votes
4
answers
1k
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Why does the Leidenfrost effect (seemingly) not apply to the case of molten NaCl when it is poured into water?
On pouring molten sodium chloride into water you can see that when molten $\ce{NaCl}$ (table salt, i.e. sodium chloride) is poured into water ($\ce{H2O}$), the Leidenfrost effect appears to be ...
- 160
1
vote
1
answer
495
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Why are ionic reactions very fast in aqueous medium? [closed]
(No, I am not talking about why Ionic Reactions are faster than Covalent reaction.)
This question has me stumped. I mean, at first it looks obvious; water is polar in nature, but what exactly does ...
- 147
6
votes
4
answers
510
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Is it possible to freeze water by dissolving a salt?
Theoretically, by dissolving a salt in water the melting point lowers, approximately 1.86 K kg/mol, making it more difficult to freeze water. However, the process of dissolution of certain salts is ...
- 169
0
votes
1
answer
2k
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So, is baking soda actually a strong base? [duplicate]
Based on my recent thoughts, when baking soda ($\ce{NaHCO3}$) is dissolved in water, the following hydrolysis reaction occurs:
$$\ce{NaHCO3 + H2O <=> NaOH + H2CO3}$$
However,
$$\ce{H2CO3 -> ...
1
vote
1
answer
92
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Crystallisation and crystal surface
It is my understanding that if you put table salt (as an example of polar compound) in water, the Na+ and Cl- ions will freely move through the solution. They will make the solution conductive and ...
- 2,518
1
vote
1
answer
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How do hydrogen bonds break the ionic bonds of a crystal lattice? [duplicate]
In the case of water dissolving sodium chloride. I was under the impression that hydrogen bonds were much weaker than the ionic bonds in sodium chloride, so how do they overcome the ionic bond ...
- 51
-3
votes
1
answer
203
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Would distilling a sodium fluoride solution generate hydrogen fluoride to any noticeable extent?
If you have a solution of NaF, and you boil it (to get pure water by distillation) can the fluoride ions in water separate from sodium ions and combine with hydrogen ions to form HF? ...
7
votes
3
answers
2k
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In my homemade electrolysis setup, only the negative end bubbles?
I've created an electrolysis setup by connecting a $6~\mathrm{V}$ battery to a cup filled with saline water via pencils; I am confused as to why only the negative pencil bubbles though. After running ...
- 173
15
votes
4
answers
14k
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Why exactly does molten NaCl explode, when it is poured into water?
Why does molten $\ce{NaCl}$ explode, when it is poured into water?
$\ce{NaCl}$ has a high melting point, $1074\ \mathrm{K}$ ($801~\mathrm{^\circ C}$). $\ce{NaCl}$ has a molar mass of $58.44\ \mathrm{g/...
- 651
6
votes
3
answers
15k
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How can sodium chloride melt ice or keep it frozen?
In European countries, they use $\ce{NaCl}$ or $\ce{KCl}$ to melt ice during the winter season.
In Asian Countries, they use $\ce{NaCl}$ to keep the ice without melting, for example in ice cream and ...
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