If 10.0 mL of 0.20 M NaOH is added to 50.0 mL of 0.10 M HCl, what will be the pH of the resulting solution?
NaOH= 10.0ml of 0.20M
number of moles of NaOH= 0.20M x 0.010L= 0.002 moles
HCl= 50.0 mL of 0.10M
number of mole of HCl = 0.1M x0.050L= 0.005 moles
number of moles of HCl is more than that of NaOH
So , the resultant solution has acidic in nature.
Remaining number of moles of Acid = 0.005 - 0.002 = 0.003 moles
number of moles of H+ ion = 0.003 moles
Total volume of the solution = 10.0+50.0= 60.0mL= 0.060L
Concentration of the resultant solution = number of moles/volume in L = 0.003/0.060= 0.05M
[H+] = 0.05M
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