Kevin Hendrick wrote:Rick F wrote:The last time I went to the chemical store to get HCI, I was told it's no longer sold to the public, but that I could buy Muriatic acid which was a little weaker solution. The label said 50% HCI.
So, it sounds like "hydrochloric" is "all (or mostly) acid", and "muriatic" is only "half acid" ...
If I went to a chemical supply house and ordered HCl, I would expect to receive a cylinder of hydrogen chloride gas. If I wanted the acid solution of HCl in water, I would specify "hydrochloric acid' and either the molar or mass concentration.
AFAIK, "muriatic acid" refers to any solution of HCl gas in water. What's sold as "concentrated" hydrochloric acid is about 12.4 M, or about 38% HCl by weight. Hardware-store muriatic acid is about 28% HCl by weight or about 9 M, so it's not
that dilute.
Of the common strong (meaning nearly-complete dissociation, not corrosiveness) inorganic acids, HCl is by far the least hazardous (this doesn't mean that you can be stupid, just that the acid's quite stable and generally, reaction products are relatively benign). Hydrochloric acid concentrations above 10% do tend to fume (i.e. give off gaseous HCl), which is why I recommended doing the mixing out-of-doors.
One of the classic freshman-chemistry experiment is to place a beaker of hydrochloric acid next to a beaker of ammonium hydroxide. Before long, a "cloud" of ammonium chloride (sal ammoniac) forms from the products of outgassing of both solutions.
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