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Results tagged with acid-base
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user 29775
This tag should be applied to questions concerning acid and base reactions. An acid is capable of donating a hydron/ proton (Brønsted acid) or capable of forming a covalent bond with an electron pair (Lewis acid). A base on the other hand is a chemical species/ molecular entity having an available pair of electrons capable of forming a covalent bond with a hydron/ proton (Brønsted base) or with the vacant orbital of some other species (Lewis base).
1
vote
Does the acid strength of hydrochloric and hydrofluoric acid correlate with the electronegat...
You are correct, HCl is a stronger acid than HF. Fluorine is both more electronegative and smaller than chlorine. Because fluorine is more electronegative, the bond between it and the hydrogen is more …
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0
votes
Relation between strength and proticity of an acid
I tend to think of acids as proton donators and bases as proton acceptors. You are correct that an acid is anything that increases the concentration of $\ce{H+}$ in solution. A general acid will have …
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2
votes
Accepted
Why is the pOH of 1M HCl 14?
In the moment from the video that you referred to, Sal was using the equation $\rm pK_w=pH+pOH$ to find the $\rm pOH$ of the solution. $\rm pK_w$ is equal to 14, since $K_w$ is equal to $1\times 10^{- …
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0
votes
Accepted
How can you change the proportions of reactants and products at equilibrium if Le Chatelier'...
The Henderson Hasselbalc equation is a good way to calculate both the pH and the concentration of acid/conjugate base in an equilibrium solution. According to it:
pH = pKa + log([A-]/[HA])
Since you …
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-1
votes
pH of Strong Acid (and why it seems like it should be zero)
One principle from mathematics is that you cannot say that two infinities are equal to one another. For example, while there are an infinite number of natural and real numbers, these two infinities ar …
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2
votes
Combining acid dissociation constants to determine pH of diprotic acid
While your method is correct for determining the number of protons produced by double dissociation, it overlooks all the protons released by single deprotonation, which should contribute significantly …
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2
votes
pH of aqueous very dilute hydrochloric acid
You are correct. The $\mathrm{pH}$ should be around six. The actual value can be found by calculating $-\log(1 \times 10^{-7} + 1\times 10^{-6})$, which gives me a final $\mathrm{pH}$ of 5.96. While y …
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3
votes
Accepted
Is H+ (in an aqueous solution) = H3O+?
When dealing with an aqueous solution, you are correct that the $\ce{H+}$ ion is equivalent to $\ce{H3O+}$ for all intents and purposes. Due to the abundance of water in solution, molecules of $\ce{H2 …
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6
votes
Why isn't CH3OH basic if it contains OH?
$\ce{CH3OH}$ is a compound known as methanol. Unlike the sodium found in $\ce{Na2CO3}$, the $\ce{CH3}$ group found in methanol will not separate from the $\ce{OH-}$. This means that the only way that …
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