the new concentration is 12 / 250, *75 which is 3.6 (no rounding needed), and you NEED to include units, which are moles per litre
71.4mL of 1.75 M hydrochloric acid must be diluted with water to prepare 0.500 L of 0.250 M hydrochloric acid.
When a given solution is diluted, it concentration is usually lowered as well. The density of the given solution also changes when the solution is diluted.
The acid becomes diluted
The concentration of the diluted solution will be 15(300/1000) = 4.5 %, if the percent is expressed on a weight/volume basis.
Depending on concentration HCl is more dangerous when a small dose by oral intake at more than 0.1 mol/L HCl (or at about 3.6 g/L or 0.4% which is very diluted)
The solution becomes more diluted and the concentration gets higher.
71.4mL of 1.75 M hydrochloric acid must be diluted with water to prepare 0.500 L of 0.250 M hydrochloric acid.
yes. it contains very diluted hydrochloric acid.
I think you must mean aqueous HCl, which is aqueous hydrochloric acid, meaning the hydrochloric acid has been diluted with water.
One use, in its diluted form, is a cleaner/sterilizer.
When a given solution is diluted, it concentration is usually lowered as well. The density of the given solution also changes when the solution is diluted.
The acid becomes diluted
This depends on the desired concentration.
The concentration.
The concentration of the diluted solution will be 15(300/1000) = 4.5 %, if the percent is expressed on a weight/volume basis.
Depending on concentration HCl is more dangerous when a small dose by oral intake at more than 0.1 mol/L HCl (or at about 3.6 g/L or 0.4% which is very diluted)
The pH of basic solutions will drop (become less basic) as the solution is diluted. However, if the solution contains a buffer, the pH will remain nearly constant upon dilution.