Write the total and net ionic equations for the reaction of this experiment? Exp

Question

Write the total and net ionic equations for the reaction of this experiment? Explain the relationship between conductivity and the presences/absence of ions in solution. Conductivity is measured in mu S/cm in this experiment, but also listed as ohm^-1 cm^-1 in your textbook? Do these different units measure the same quality? What is the difference if any? You will probably have to use outside resources to answer this question. Give a specific example of the following: Strong Electrolyte. Weak Electrolyte, and Nonelectrolyte. Explain why each example fits each category. In this experiment, you will monitor conductivity during the reaction between sulfuric acid, H_2 SO_4, and barium hydroxide, Ba(OH)_2. in order to determine the equivalence point. From this information, you can find the concentration of the Ba(OH)_2 solution. You will also see the effect of ions, precipitates, and water on conductivity. The equation for the reaction in this experiment is: Ba^2+ (aq) + 2 OH^- (aq) + 2 H^+ (aq) + SO_4^2- (aq) rightarrow BaSO_4 (s) + H_2 O (l) Before reacting, Ba (OH)_2 and H_2 SO_4 are almost completely dissociated into their respective ions. Neither of the reaction products, however, is significantly dissociated. Barium sulfate is a precipitate and water is predominantly molecular. As 0.02 M H_2 SO_4 is slowly added to Ba(OH)_2 of unknown concentration, changes in the conductivity of the solution will be monitored using a Conductivity Probe. When the probe is placed in a solution that contains ions, and thus has the ability to conduct electricity, an electrical circuit is completed across the electrodes that are located on either side of the hole near the bottom of the probe body. This results in a conductivity value that can be read by the interface. The unit of conductivity used in this experiment is micro siemens per centimeter, or mu S/cm.

Explanation / Answer

1) Ba(OH)2 (aq) + H2SO4 (aq) ------------> BaSO4 (s)+ 2H2O (l)
Net Ionic equation:
Ba2+(aq) + 2OH- (aq) + 2H+(aq) + SO42-(aq) ----------> BaSO4 (s) + 2H2O (aq)
2)Ions in the solution conduct the electricity when it is passed through it. If there are more ions in the
   aqueous solution then that implie that there is more concentration, hence they conductivity is more
   in such cases.
3) [1 ohm-1 m-1 = 1 S/m]
   Ohm-1 cm-1 and S/cm represent the same quantity i.e) conductivity
   Older conductivity meters represented Ohm-1 cm-1 units ( aka mho cm-1), Seimens is more like
   modern day unit.
4) Strong electrolytes like HCl, HBr - dissociate completely in the aqueous solution.
   Weak electrolytes like CH3COOH, H3PO4 - do not dissociate/ionize completely
   non-electrolytes benzene, ethanol etc - do not ionize at all

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