Question

con Experiment 5 Data and Report Name: Charene Lab Section (Day): Wednesday Partner: Troter A. Electrolytes and Nonelectrolytes 1. Classify the substances and solutions as nonelectrolytes (lowest values), weak electrolytes middle values), or strong electrolytes highest values Important: Make sure conductivity meter is set to appropriate sensitivity range. Strong Non- electrolyte (no lons) Weak electrolyte (few lons) electrolyte (many lons) Distilled H,00 Conductivity (units: 63.903 390 10.01 Tap H,0 Methanol, CH,OH(1 Aqueous methanol, CH,OH(aq) Glacial acetic acid CH,COOHO Aqueous acetic acid, CH,COOH(aq) Hlaa) doo 55 Aqueous sucrose, C2H2O(aq) NaCl(aq) 22823 Caso (aq) 0.1 M HCl(aq) 0.1 M NaOH(aq) 30 657 11.573 5-7

there is more than one question and more than one part, and i put pictures of the data in there too

there is more than part and more than one picture

Answer 1

4.Balanced Chemical reaction (based on observation)

• CH₃OH + H₂O $\rightarrow$  CH₃OH(aq) : No Ionization
• CH₃COOH + H₂O $\rightleftharpoons$  CH₃COO^- (aq) + H₃O⁺ (aq)
• C₁₂H₂₂O₁₂ + H₂O $\rightarrow$ C₁₂H₂₂O₁₂(aq)   : No Ionization
• NaCl + H₂O $\rightarrow$ Na⁺(aq) + Cl^-(aq)
• CaSO₄ + H₂O $\rightarrow$ Ca⁺⁺ (aq) + SO₄ 2^- (aq)
• HCl + H₂O $\rightarrow$ H₃O⁺+ Cl^-(aq)
• NaOH + H₂O $\rightarrow$ Na⁺(aq) + OH^-(aq)

2.Correlating chemical and conductivity behaviour :

• CaCO₃ (s) + 2 HA  $\rightarrow$ CaA₂ (aq) + CO₂ (g)+ H₂O(l)
• Zn (s)  + HA  $\rightarrow$ ZnA₂  (aq) + H₂ (g)
• Reaction with much more faster 6M HCl than 6M Acetic acid , because HCl is a strong acid and completely ionized in water (evident from conductivity).Rate if reaction depends on concentration of H⁺ , which are much more for 6M HCl . Reaction with HCl produces more bubbles , beacause reaction proceeds faster towards completion, thus more evolution of gases.
• There is a strong correlation in conductivity and rate of reaction, from conductivity it ia known that Acetic acid is a weak electrolyte and HCl is strong electrolyte, thus difference in ionization is marked in rate of reactions.

B.

(a)

• Reactants are strong electrolyte, these exists as ions.
• Conductivity change indicates decrease in the Number of ions, due to formation of water molecule.

Total ionic equation : H⁺(aq) + Cl^–(aq) + Na⁺(aq) + OH^–(aq) Na⁺(aq) + Cl^–(aq) + H₂O(l)

• Net ionic equation : H⁺(aq) + OH^–(aq)   H₂O(l) (ions present on both sides get cancelled)
• Solution of HCl is more conductive than of NaOH (same no. of ions, difference due to different ionic mobilities). After mixing conductivity is lesser than both reactant solution due to depletion in number of ions, and also due to absence of fast moving  H⁺.

(b)

• Reactants are weak electrolyte, these exists as both molecules and ions.

CH₃COOH + H₂O $\rightleftharpoons$  CH₃COO^- (aq) + H₃O⁺ (aq)

NH₃ + H₂O $\rightleftharpoons$ NH₄+(aq) + OH^-(aq)

• Conductivity change indicates increase in the Number of ions.

• Total ionic equation :

CH₃COO^- (aq) + H₃O⁺ + NH₄+(aq) + OH^-(aq) CH₃COO^- (aq) + NH₄+(aq)​​​​​​​ + 2H₂O(l)

• Net ionic equation : H₃O⁺ (aq)​​​​​​​+ OH^–(aq)   H₂O(l) (ions present on both sides get cancelled)
• Solution before mixing are less conductive than After mixing. After mixing reaction forms Ammonium acetate , which is salt (strong electrolyte); thus No. of ions increased, results in more conductivity after mixing.

CH₃COONH₄ + H₃O   CH₃COO^- (aq) + NH₄+(aq)​​​​​​​