Question

can someone show how this was solved?

what is the molarity of an HNO3 solution if 24.1 ml of a 0.250M Ba(OH)2 solution are needed to titrate a 15.0ml sample of the acid according to the equation below?

Ba(OH)2(aq) +2HNO3(a) 2H2O (l) + Ba(NO3)2 (aq)

Answer 1

The balanced reaction between HNO3 and Ba(OH)2 is

Volume of Ba(OH)2 solution used = 24.1 mL

Concentration of the Ba(OH)2 solution = 0.250 M = 0.250 mol/L.

Hence, number of moles of Ba(OH)2 in the 24.1 mL solution can be calculated as

Now according to the balanced reaction, 1 mol of Ba(OH)2 reacts with 2 moles of HNO3.

Hence, number of moles of HNO3 that will be neutralised by of Ba(OH)2 is

It is given that the volume of HNO3 that was titrated = 15.0 mL

Hence, 15.0 mL of HNO3 contains .

Hence, the concentration of HNO3 can be calculated as

Hence, the concentration of HNO3 is approximately 0.803 M.