Question

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In the following table, record the conductivity measured for each solution. The electrolyte type I should be strong, weak or non-electrolyte according to the table given previously. The species in solution should be a listing (in order of decreasing concentration) of the components of the solution. Ask your instructor if you need to list water as a species in solution. Species in Solution (In order of decreasing concentration) Electrolyte Type (SE, WE, NE) Conductivity Solution Deionized water Ethanol(1) (CH3CH2OH) 13.5 Ethanol (aq) (CH3CH2OH) lem 11.0 0.1 M acetic acid(aq) (HC2H3O2) 51D lam Sucrose(aq) (C12H22O11) 24.1 slan 13 000 us/om 0.1 M NaCl(aq) 55,900slom 0.1 M HCl(aq) 3,500 JUSCM 0.1 M NaOH(aq) 443 0.1 M NH3(aq) Ctr Chemistry 125 Laboratory Manual - 2019 Page 101 H의 Which acid reacted more rapidly? II Which acid had the higher conductivity (from Part I)? Explain why conductivity and reactivity should be related. III. A. Conductivity of acetic acid (from Part I) Conductivity of ammonia (from Part I) 3,90s/o Conductivity of mixture Did the conductivity increase or decrease after reaction? Write a balanced chemical equation for the reaction that occurred when the solutions were mixed: Based on your reaction, explain the results you observed for the conductivity change. III. B. This part of the experiment will be done by your instructor. You will record the results here Conductivity of sulfuric acid 49,300 24,400 Conductivity of barium hydroxide 7 Conductivity of mixture Did the conductivity increase or decrease after reaction? Write a balanced chemical equation for the reaction that occurred when the solutions were mixed: Based on your equation, explain the results observed for the conductivity change.

Answer 1

II . From part 1, we can clearly see that HCl has the highest conductivity(=55,400 $\mu$S/cm)

$\rightarrow$ Conductivity and reactivity should be related. The reason being that, both the properties are dependent on the ions present in the solution. Now if we consider a strong acid like HCl, it easily dissociates into its respective ions upon dissolution in water and hence it is highly reactive.Same goes for conductivity also. Since it easily dissociates into ions, the solution easily provides large number of electrons for the current flow and hence is bound to have a higher conductivity .

III.A From part 1, we can clearly see that the conductivity of acetic acid is 510 $\mu$S/cm and

For Ammonia, the conductivity value is 443 $\mu$S/cm .

$\rightarrow$There is a clear increase in conductivity after reaction.

$\rightarrow$ CH₃COOH + NH₄OH $\rightarrow$ CH₃COONH₄ + H₂O

$\rightarrow$ The reason for an increased conductivity is due to the fact that, although both Ammonia and Acetic acid are weak electrolytes but their reaction in aqueous solution renders the formation of Ammonium Acetate,which is a strong electrolyte.Due to this reason, the conductivity increases sharply after reaction.

III.B The conductivity of the solution decreased after reaction .

$\Rightarrow$ Ba(OH)₂ + H₂SO₄$\rightarrow$ BaSO₄ + 2 H₂O

$\rightarrow$ Initially, Sulfuric acid and Barium hydroxide are both strong electrolytes.Their reaction is bound to produce a nearly neutral solution due to the reason that, both are highly opposite in nature ( Ba(OH)₂ is a very strong base & H₂SO₄ is a very strong acid) . Therefore there is a sharp decrease in conductivity after reaction between the two.