2006-10-31 01:16:17 · 7 answers · asked by Kate M 1 in Science & Mathematics ➔ Chemistry
Will it be weak aswell?
2006-10-31 04:10:42 · update #1
Yes that is dilute. A concentrated solution of HCl would be around 10 mol/dm3.
2006-10-31 02:44:43 · answer #1 · answered by Anonymous · 0⤊ 0⤋
Yes, it would be very dilute indeed. Ordinary 'bench' dilute HCl is between 1M and 2M. When used for titration, it tends to be about one-tenth as strong, i.e. 0·1M to 0·2M
If it's 0·001M, it would have a pH of 3 and you could drink it without any ill effect, although I seem to remember that it has a rather bitter taste. It would be less strongly acid than lemon juice and only slightly stronger than vinegar.
Allan Deeds
P.S. I'm sorry, EmoKite, but you are wrong: a solution can be dilute or concentrated in any solvent at all.
2006-10-31 12:31:42 · answer #2 · answered by deedsallan 3 · 0⤊ 0⤋
If it is assumed to be mostly water, then the density will be around 1 kg/dm3 at room temperature.
1 mole weighs 36.5 g, therefore 0.001M weighs 36.5mg. The rest is water, i.e. 1000 - 0.0365 = 999.9635 g. Hence, if my maths is correct, it is 0.00365% by weight. This is very dilute.
However, it is not classed as a weak acid. This is a different thing altogether, and is dependent on the type of acid, not the concentration. HCl, like sulphuric and nitric acid are classed as strong acids. Weak acids are generally organic acids, such as acetic acid (Vinegar), and citric acid.
2006-10-31 13:03:39 · answer #3 · answered by Trevor P 2 · 0⤊ 0⤋
Yes. It's a dilute solution.
2006-10-31 09:33:56 · answer #4 · answered by Lim 1 · 0⤊ 0⤋
Pure HCl is about 10 M . Your solution is 10,000 times weaker.
2006-11-02 10:11:53 · answer #5 · answered by lykovetos 5 · 0⤊ 0⤋
yes. it is much more dilute that 0.1 mol/dm3 you usually use in school.
2006-10-31 16:30:39 · answer #6 · answered by coy carp 3 · 0⤊ 0⤋
not if it's not in water. it needs to be in water to be diluted.
2006-10-31 09:32:31 · answer #7 · answered by Cookie Monster 3 · 0⤊ 0⤋