Very carefully, under a hood, using proper protective equipment, if the acid/ bases are relatively strong and concentrated.
If they are known to be in a very diluted state, perhaps use of a hood would not be needed, such as when titrations are carried out.
Obviously, in this case, sodium hydroxide neutralization would require that considerably more care be taken than for the neutralization of the much weaker, acetic acid.
I guess I forgot to state the obvious, which is, bases are used to neutralize acids, while acids are used to neutralize bases.
Very carefully, under a hood, using proper protective equipment, if the acid/ bases are relatively strong and concentrated.
If they are known to be in a very diluted state, perhaps use of a hood would not be needed, such as when titrations are carried out.
Obviously, in this case, sodium hydroxide neutralization would require that considerably more care be taken than for the neutralization of the much weaker, acetic acid.
I guess I forgot to state the obvious, which is, bases are used to neutralize acids, while acids are used to neutralize bases.
How do you neutralize acetic acid with sodium hydroxide…?
Well take 1 equiv acetic acid, and add 1 equiv of sodium hydroxide … we follow the equation…
[math]NaOH(aq) + HO(O=)CCH_{3}(aq) longrightarrow ^{+}Na^{-}O(O=)CCH_{3}(aq)+H_{2}O(l)[/math]
And given 1:1 reaction, the solution of sodium acetate will be SLIGHTLY basic…why so?
How do you neutralize acetic acid with sodium hydroxide…?
Well take 1 equiv acetic acid, and add 1 equiv of sodium hydroxide … we follow the equation…
[math]NaOH(aq) + HO(O=)CCH_{3}(aq) longrightarrow ^{+}Na^{-}O(O=)CCH_{3}(aq)+H_{2}O(l)[/math]
And given 1:1 reaction, the solution of sodium acetate will be SLIGHTLY basic…why so?
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Very carefully, under a hood, using proper protective equipment, if the acid/ bases are relatively strong and concentrated.
If they are known to be in a very diluted state, perhaps use of a hood would not be needed, such as when titrations are carried out.
Obviously, in this case, sodium hydroxide neutralization would require that considerably more care be taken than for the neutralization of the much weaker, acetic acid.
I guess I forgot to state the obvious, which is, bases are used to neutralize acids, while acids are used to neutralize bases.
Very carefully, under a hood, using proper protective equipment, if the acid/ bases are relatively strong and concentrated.
If they are known to be in a very diluted state, perhaps use of a hood would not be needed, such as when titrations are carried out.
Obviously, in this case, sodium hydroxide neutralization would require that considerably more care be taken than for the neutralization of the much weaker, acetic acid.
I guess I forgot to state the obvious, which is, bases are used to neutralize acids, while acids are used to neutralize bases.
More
VOTE