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Why are ions much more efficient than electrons at beam-induced deposition? |
Does the pyrolysis of $\ce{CaCl2 · 2 H2O}$ give $\ce{CaCl2 + 2 H2O}$ or $\ce{Ca(OH)2 + 2 HCl}?$ |
I am trying to find a way to separate my PLA samples and ABS samples. Last night I've observed:
- When soaked in Ethyl Acetate:
- ABS disintegrates in about an hour,
- PLA loses "fancy" properties, ( such as green/yellow color-changing filament, went blue. )
- All PLA, fancy or standard, turns very flexibl... |
$$\pmb {\underline {\text {Background}}}$$
Recently I have been studying about the states of matter and came to the topic of ideal gases and real gases and the laws related to them. While studying it from my textbook I saw the plot of pressure Vs volume for real and ideal gas. The problem is that the interpretation ... |
$$\pmb {\underline {\text {Background}}}$$
Recently I have been studying about the states of matter and came to the topic of ideal gases and real gases and the laws related to them. While studying it from my textbook I saw the plot of pressure Vs volume for real and ideal gas. The problem is that the interpretation ... |
Is there a way to dehydrate hydrated aluminum chloride for use as a Lewis acid? |
Does Mg(OH)2 form or what? I'm qurious, because Wikipedia says that it decomposes to release HCl gas. |
$$\pmb {\underline {\text {Background}}}$$
Recently I have been studying about the states of matter and came to the topic of ideal gases and real gases and the laws related to them. While studying it from my textbook I saw the plot of pressure Vs volume for real and ideal gas. The problem is that the interpretation ... |
The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 moles litre^-1}$ and $Pka$ of $\ce{H2SO3}$ is 1.92, Estimate $pH$ of rain on that day. 10 ppm means there is 10^-2 grams of SO2 in 1 litre of air. This accounts to... |
When magnesium chloride hydrate is heated, does $\ce{Mg(OH)2}$ form or what? I'm curious, because Wikipedia says that it decomposes to release $\ce{HCl}$ gas. |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
$$\pmb {\underline {\text {Background}}}$$
Recently I have been studying about the states of matter and came to the topic of ideal gases and real gases and the laws related to them. While studying it from my textbook I saw the plot of pressure Vs volume for real and ideal gas. The problem is that the interpretation ... |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
> The concentration of $\ce{SO2}$ in the atmosphere over a city on a certain day is $\pu{10 ppm}$. Given that solubility of $\ce{SO2}$ in water is $\pu{1.3653 mol L-1}$ and $\mathrm{p}K_\mathrm{a}$ of $\ce{H2SO3}$ is $1.92,$ estimate $\mathrm{pH}$ of rain on that day.
$\pu{10 ppm}$ means there is $\pu{10^-2 g}$ of $... |
It would be burnt outside in the forest at about 2 degrees Celsius with about 75 percent air humidity. I'm not sure how good its quality might be, but it looks fine, pretty much like this [here][1]. It took me way too long to find out how to produce it and even longer to get to such an amount. It would be a shame if th... |
Why lithium looses electron more easily than sodium according to electrode potential values? |
In my school science textbook, written more than twenty years ago, it said that *pure* iron does not rust. Accompanying was a photograph of an ancient iron statue situated outside, which had not rusted.
Is this correct? |
Does pure iron not rust? |
"I am trying to understand why Nitrogen in Ammonia is a proton acceptor."
I am going to modify your question slightly: it is a proton acceptor in aqueous solution. Water, being the solvent of life and being very common on Earth, is generally the most pertinent solvent. Ammonia is a proton acceptor, or if you pref... |
I mean doesn't every compound has its own different reduction and oxidation potential ? Or its just one potential that can be compared to understand which one will get reduced and which one will get oxidised ? |
Is redox potential a valid term? |
There is the table of **standard electrode potentials**. These are values which is relative to **the standard hydrogen electrode**. They were measured at certain, constant for all, conditions.
To measure actual potentials one can use Nernst equation
Last night I've observed:
- When soaked in Ethyl Acetate:
- ABS disintegrates in about an hour,
- PLA loses "fancy" properties, ( such as gr... |
I work as an RA in an academic lab. I've been working with FCS fitting for an experiment, and took FCS curves for fluorescein and calmodulin, displayed with residuals below:
[![fluorescein FCS curve[![\]\[1\]][1]][1]][2]
[1]: https://i.stack.imgur.com/TGmPj.png
[2]: https://i.stack.imgur.com/2rxlN.png
I... |
> Is redox potential a valid term?
Yes it is a valid thermodynamic term. Also oxidation potential is a valid term. After a century of arguments, electrochemical societies decided to write all the half cells as reduction e.g., $\ce{Fe^{3+} + e- -> Fe^{2+}}$ and call the potential of this reaction as the reduction p... |
I want to heat the air with Non-aqueous, non-toxic and non-solvable-in-air liquid (with very low relative pressure in air). Is there any such liquid exists?
It would be great if the boiling point of the liquid would be 110 C. |
Is there any non-toxic and non-solvable-in-air liquid? |
I want to heat the air with non-aqueous, non-toxic and non-solvable-in-air liquid (with very low relative pressure in air). Is there any such liquid exists?
It would be great if the boiling point of the liquid would be 110 C. |
I want to heat the air with non-aqueous, non-toxic and non-solvable-in-air liquid (with very low relative pressure in air). Is there any such liquid exists?
It would be great if the boiling point of the liquid would be 110 °C. |
If I try to find the concentration of citric acid through back titration or reverse titration, the base I would use, like NaOH, would react with both acids to form sodium citrate and sodium tartrate, which are both white compounds that are colourless in aqueous form. How do I find the concentration of citric acid? |
I have a solution of citric acid, tartaric acid, water and glucose. How do I find the concentration of the citric acid present in the solution? |
i have read that aniline does not undergo friedel crafts because it complexes with lewis acid AlCl3, will it also react with FeBr3 during bromination (to recive a 3 bromo substituted benzene)? |
I have read that aniline does not undergo Friedel–Crafts reaction because it complexes with Lewis acid $\ce{AlCl3}.$ Will it also react with $\ce{FeBr3}$ during bromination (to receive a 3-bromo substituted benzene)? |
Does aniline react with other Lewis acids besides AlCl₃? |
Recently, I have seen room temperature listed at 20 and 25 degrees Celsius. My question is simply which one is more accurate for use in chemistry problems? |
What is considered room temperature in Celsius? |
> Is redox potential a valid term?
Yes it is a valid thermodynamic term. Also oxidation potential is a valid term. *These terms differ only by a sign*. If a reduction potential of a given half cell is -0.73 V with respect to hydrogen cell. its oxidation potential is +0.73 V. So you have to stick to one term for co... |
> I mean doesn't every compound has its own different reduction and oxidation potential ? Or its just one potential that can be compared to understand which one will get reduced and which one will get oxidised ?
A compound has neither. You need to specify the half reaction. For example, take an aqueous solution of $... |
$$\pmb {\underline {\text {Background}}}$$
Recently I have been studying about the states of matter and came to the topic of ideal gases and real gases and the laws related to them. While studying it from my textbook I saw the plot of pressure Vs volume for real and ideal gas. The problem is that the interpretation ... |
Recently, I have seen room temperature listed at 20 °C and 25 °C. Which one is more accurate for use in chemistry problems? |
Does aniline react with FeBr₃? |
Why is it when you heat and pressurize CO and H2 it converts to methane? Is it because when you heat the molecules the bonds get weaker and the pressure breaks the bonds and allows them to flow and create new molecule?
Thank you |
We were taught in chemistry that:
- Formal charges can be determined by drawing the Lewis dot structure, then subtracting the nonbonding electrons and half of the bonding electrons from the number of electrons ordinarily in that atom's valence.
- Molecules tend to be in the state with the lowest formal charge on ... |
Why are only two bond structures considered for ozone and not three? |
We were taught in chemistry that:
- Formal charges can be determined by drawing the Lewis dot structure, then subtracting the nonbonding electrons and half of the bonding electrons from the number of electrons ordinarily in that atom's valence.
- Molecules tend to be in the state with the lowest formal charge on ... |
Coupled cluster is a non-variational method, meaning that it can give energies that are below the true FCI energy (the "variational limit" for variational methods).
Often coupled cluster still gives energies far above the true FCI energy, and sometimes it gives energies that dip below the variational limit.
Is th... |
Is there a rule of thumb to predict when coupled cluster might dip below the variational limit? |
I have three histidine residues that are next to each other in a protein. When I compute the fraction of un-protonated states for each individual histidine as a function of pH my titration curve has a non-Henderson Hasselbalch shape. Hence I can't fit it using the HH equation for 1 site:
${1}/{1+10^{n(pKa-pH)}}$ in ... |
I have three histidine residues that are next to each other in a protein. When I compute the fraction of un-protonated states for each individual histidine as a function of pH my titration curve has a non-Henderson Hasselbalch shape. Hence I can't fit it using the HH equation for 1 site:
$${1}/{1+10^{n(pKa-pH)}}$$
... |
You are correct that there are aspects to consider:
- The increase of *pressure* equates to more particles per unit of volume. It is like filling a metro with more and more people during rush hour, the propability of collisions increases.
- The increase of *temperature* equates to a higher kinetic energy of the... |
On a chemistry homework, we're asked to draw the Lewis structure of $\ce{N3-}$.
My answer:
- Nitrogen ordinarily has five electrons in its valence; $\ce{N-}$ has six. This makes a total of 16 electrons overall.
- If we place the negative charge on the central atom, we get a structure of $\ce{N={N^-}=N}$
- ... |
What is the Lewis structure of $\ce{N3-}$? |
Actually, there is little to no reaction of vinegar on copper metal. The Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of the copper metal with O2 subject to an inception pe... |
Actually, there is little to no reaction of vinegar on copper metal. The Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of the copper metal with O2 subject to an inception pe... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
On a chemistry homework, we're asked to draw the Lewis structure of $\ce{N3-}$.
My answer:
- Nitrogen ordinarily has five electrons in its valence; $\ce{N-}$ has six. This makes a total of 16 electrons overall.
- If we place the negative charge on the central atom, we get a structure of $\ce{N=N^-=N}$
- Th... |
What is the Lewis structure of the azide ion? |
I am reading a textbook that mentions the molecule 1,2-diphenylethane, $C_{14}H_{14}$. A Google search leads to [this][1] page, where it is mentioned that the IUPAC name for the molecule is 2-phenylethylbenzene. I'm trying to understand how one names the molecule, using IUPAC nomenclature. However, I'm struggling to fi... |
I am reading a textbook that mentions the molecule 1,2-diphenylethane, $\ce{C14H14}$. A Google search leads to [PubChem][1], where it is mentioned that the IUPAC name for the molecule is 2-phenylethylbenzene. I'm trying to understand how one names the molecule, using IUPAC nomenclature. However, I'm struggling to find ... |
How to arrive at the preferred IUPAC name for 1,2-diphenylethane? |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
I recall a paper where heating the hydrate in a stream of HCl gas avoided the formation of a basic salt.
This may work for hexahydrate AlCl6⋅6H2O also.
Quick search returned this ebook reference https://books.google.com/books?id=Pef47TK5NfkC&pg=PA1147&lpg=PA1147&dq=dehydration+with+a+stream+of+HCl&source=bl&ots=W... |
Your proposed structure is wrong. Nitrogen does not exceed the octet in any of its known compounds (and even if $\ce{NF5}$ will be discovered it will not exceed the octet according to everything we know now). However, if you have a formal negative charge that means an additional electron added to the 5 nitrogen usually... |
In the center of the chamber on the photo below you can see the hexagonally-shaped [Macor glass-ceramic](https://en.wikipedia.org/wiki/Macor) consisting of
- Silicon dioxide $\ce{SiO2}~46\%$
- Magnesium dioxide $\ce{MgO}~17\%$
- Aluminum oxide $\ce{Al2O3}~16\%$
- Potassium oxide $\ce{K2O}~10\%$
- Boron... |
I have three histidine residues that are next to each other in a protein. When I compute the fraction of unprotonated states for each individual histidine as a function of $\mathrm{pH}$ my titration curve has a non-Henderson–Hasselbalch (HH) shape. Hence I can't fit it using the HH equation for 1 site:
$$\frac{1}{1 ... |
The data look as if you have simply done a titration of histidine, with a first pKa at around 6, and another one at around 8.5 - 9. This is exactly what is expected from the tabulated values for histidine : pKa = 6.04 and 9.09. Why are you not satisfied about these measurements ? Your results are in perfect agreement w... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
When we find the pH of a solution, do we use Normality or Molarity? My teacher said that if the compound is present by itself, we can use normality but in all other cases we should use Molarity. Can you explain why? |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
When we find the pH of a solution, do we use normality or molarity? My teacher said that if the compound is present by itself, we can use normality but in all other cases we should use molarity. Can you explain why? |
I don't really like parts of this explanation (was hoping to find a better one here actually), but it's the best I know. I'll build on suggestions by @michielim and @vrtcl1dvoshun.
(Note: I think most of this argument can be transposed to the orbital overlap picture of bonding, but it might be slightly trickier to ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing Cu2O coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical attack of ... |
Actually, there is little to no reaction of vinegar on copper metal (hence, the copper wire in solution is clear). Existing $\ce{Cu2O}$ coating will be slowly attacked, forming a cuprous acetate which in air/oxygen creates soluble cupric acetate. The latter serves as a weak electrolyte for a further electrochemical att... |
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