A student performs an experiment in which the conductivity of a solution of Ba(O

Question

A student performs an experiment in which the conductivity of a solution of Ba(OH)2 is monitored as the solution is titrated with 0.10 M H2S04. The original volume of the Ba(OH)2 solution is 25.0 mL A precipitate of BaSO4 (Ksp= 1.0 x I0-10) formed during the titration. The data collected from the experiment are plotted in the graph above As the first 30.0 mL of 0.10 M H2SO4 are added to the Ba(OH)2 solution, two types of chemical reactions occur simultaneously. On the lines provided below, write the balanced net-ionic equations for the neutralization reaction and the precipitation reaction Equation for neutralization reaction: Equation for precipitation reaction:

Explanation / Answer

answers:

1) net ionic- neutralisation reaction

   H+ (aq) + OH- (aq) ----------------------> H2O (l)

2) net precipitation reaction

Ba+2(aq) + SO4-2 (aq) --------------------------> BaSO4 (s)

Explanation:

here H2SO4 is strong acid and Ba(OH)2 is strong base . the reaction between strong acid and strong base leads to form salt and water.

here to get net equation we have to consider and take H+ from acid and OH- from base.

so net ionic neutrlised equation    H+ (aq) + OH- (aq) ----------------------> H2O (l)

and spectator ions are Ba+2 and SO4-2 ions form salt . this is solid or precipitate

so net precipitatation reaction

Ba+2(aq) + SO4-2 (aq) --------------------------> BaSO4 (s)

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