How do I calculate what volume of water should be added to 10.0 mL of 6.00 M HCL to produce a 0.500 M HCl solution?
We have 10mL of 6.00 M HCL.
6.00M HCl means 6 moles of HCl are present in 1000 ml of its solution.
Thus , in 1ml of its solution 0.006 moles of HCl are present.
This implies , in 10ml 0.06 moles of HCl are present.
We want 0.5 M HCl which means we want 0.5 moles of it in 1000ml of its solution.
We have 0.06 moles of HCl .
Thus , volume of required to make it 0.5M is given by: moles of HCl / molarity of solution
Thus , volume of solution should be 0.12L = 120 ml.
Volume of Water to be added = total final volume - initial volume
= 120 - 10 = 110 ml