In: Chemistry
Starting with the 0.1250M Cu(NH3)+2 as the stock (concentration) calculate the following concentrations of the dilute solutions showing work:
15mL stock diluted to 20mL
10.0mL of stock solution diluted to 20.0mL
5.0mL of the stock solution diluted to 20.0mL
Concentration of the stock solution of Cu(NH3)2+ = 0.1250M
During diution we only add water. Hence the moles of Cu(NH3)2+ before and after dilution remains constant.
(a). 15mL 0.1250M Cu(NH3)2+ solution stock diluted to 20mL
moles of Cu(NH3)2+ before dilution = MxV = 0.1250Mx15x10-3 = 1.875x10-3 moles
moles of Cu(NH3)2+ after dilution = MxV = Mx20x10-3 moles
moles of Cu(NH3)2+ before dilution = moles of Cu(NH3)2+ after dilution
1.875x10-3 moles = Mx20x10-3 moles
M = 1.875x10-3 moles/20x10-3 moles = 0.09375 M (answer)
(b) 10.0mL of stock solution diluted to 20.0mL
We can calculate this in a similar manner as we did in (a). But here the initial volume is 10mL
moles of Cu(NH3)2+ before dilution = MxV = 0.1250Mx10x10-3 = 1.250x10-3 mol
moles of Cu(NH3)2+ after dilution = MxV = Mx20x10-3 mol
1.250x10-3 mol =Mx20x10-3 mol
M = 1.250x10-3 mol/20x10-3 mol = 0.0625M (answer)
(c) 5.0mL of the stock solution diluted to 20.0mL
similarly
moles of Cu(NH3)2+ before dilution = MxV = 0.1250Mx5x10-3 = 0.0625x10-3 mol
moles of Cu(NH3)2+ after dilution = MxV = Mx20x10-3 mol
0.06250x10-3 mol =Mx20x10-3 mol
M = 0.03125 M (answer)