How do we make a #1*L# volume of a solution that is #0.5*mol*L^-1# with respect to #HCl# from a solution that is #10.6*mol*L^-1# with respect to #HCl(aq)#?

1 Answer
Jun 15, 2017

Answer:

Given proper attire, with conc. acid THE PRIMARY PRACTICAL CONSIDERATION IS #"ADD YOUR ACID TO WATER"# and NEVER #"VICE VERSA"#. We need approx. a #50*mL# volume of conc. acid.

Explanation:

And why so?

#"Because if you spit in acid, it spits back!"# I kid you not......

See this older answer.

And other practical considerations. Wear a pair of SAFETY SPECTACLES to protect your mince pies; and wear a lab coat to protect your clothing......You should do this automatically in a lab (if you are a speccy, your prescription glasses are an adequate protection). Most chemists upon entering a lab will IMMEDIATELY put on a pair of safety spex from a tray, or put on the safety spec that they carry in their pocket. This is certainly a habit to develop.

And to make a #1*L# volume of #0.5*mol*L^-1# #HCl#; we use the relationship.....

#C_1V_1=C_2V_2#, and we solve for #V_1#.....

#V_1=(C_2V_2)/C_1=(0.5*mol*L^-1xx1*L)/(10.6*mol*L^-1)~=50*mL#.

And remember to add the #"WATER to YOUR ACID..............."#