Question

(2) The student adds some dilute nitric acid to a burette and does the titration. The equation for the reaction is Ba(OH)₂ + 2HNO, → Ba(NO₂)₂ + 2H₂O The student finds that 21.50 cm' of nitric acid of concentration 0.600 mol/dm³ neutralises 25.0 cm³ of barium hydroxide solution. Calculate the concentration, in mol/dm³, of the barium hydroxide solution.​

Answer 1

0.0964, I worked out the moles of barium hydroxide and divided this by two and then divided that by the volume of nitric acid

Step-by-step explanation:

Answer 2

0.258 mol/dm3

Step-by-step explanation:

Ba(OH)2 + 2HNO3 ---------> Ba(NO2)2 +2H2O

1 : 2 : 1 : 2

0.00645 : 0.0129 : 0.00645 : 0.0129

Moles of Nitric Acid

Moles=Concentration X Volume(dm3)

0.600 X 0.0215

=0.0129 mol

Concentration= Moles/ Volume(dm3)

0.00645/0.025

= 0.258 mol/dm3