show work Conductometric Titration - hydroxide solution titrated. Plotted on the

Question

show work Conductometric Titration - hydroxide solution titrated. Plotted on the y-axis is the conductivity and on the x-axis is the ml of 0.100 M Shown below are two conductometric titrations of barium solution by sulfuric ocid. In each trial 50.0 ml of barium hydroxide solution wos sulfuric acid added. Trial 1 - The end point is ind cated by the vertical dashed line at 9.62 ml. Trial 2 - The end point is indicated by the vertical dashed line at 9.25 ml. a. Calculate the [Ba(OH)] as determined in trial 1 b. Calculate the [Ba(OH)] as determined in trial 2 Write the balanced net ionic equation for the reaction of barium hydroxide with sulfuric acid. c.

Explanation / Answer

a. end point is reached when all the barium hydroxide molecules are completely react with H2SO4

V1xN1=V2xN2

9.62mlx0.100M=50mlxconcentration of Ba(OH)2

[Ba(OH)2]=0.01924M

b.

V1xN1=V2xN2

9.25mlx0.100M=50mlxconcentration of Ba(OH)2

[Ba(OH)2]=0.0185M

c.Net Ionic Reaction:
Ba2+ (aq) + 2 OH- (aq) + 2 H+ (aq) + SO42- (aq) ------> BaSO4 (s) + H2O (l)

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