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In the space provided, write the balanced IONIC and NET IONIC equation. 3. HNO, + Al(OH), -> H2O + Al(NO,)) Str. elect. ionic, insol. ionic, sol. IONIC: NET IONIC: 4. HCI + _Mg(C2H,O2)2 _MgCl2 + HC,H,O2 Str. Elect. ionic, sol. ionic, sol. wk. Elect. IONIC: 10 of 12 CHM1045L Exp. #5: ELECTROLYTES AND NONELESTROIXTES NET IONIC:

In the space provided, write the balanced IONIC and NET IONIC equation. 3. HNO, + Al(OH), -> H2O + Al(NO,)) Str. elect. ionic, insol. ionic, sol. IONIC: NET IONIC: 4. HCI + _Mg(C2H,O2)2 _MgCl2 + HC,H,O2 Str. Elect. ionic, sol. ionic, sol. wk. Elect. IONIC: 10 of 12 CHM1045L Exp. #5: ELECTROLYTES AND NONELESTROIXTES NET IONIC:

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I. Electrolytes and Non-electrolytes Using the conductivity meter, record the reading for each of the substances and mixtures listed on Data Sheet 1. Make all measurements in 30- or 50 mL beakers. Always rinse the electrodes of the conductivity meter and all reaction containers with distilled water. Ensure that all flasks are completely dried before measuring the conductivity of any solid material. Use approximately 15 mL of each liquid. While stirring with electrodes, press the high scale setting on the meter (if applicable) and record the conductivity. From the conductivity meter: A reading of zero indicates non-conductive A reading of one through seven indicates weak to moderate conductivity A reading greater than seven indicates strong conductivity. Next to the conductivity reading on your data sheet, indicate the specific ions or molecules that gave rise to the observed reading. In the last column, explain the source of these ions and/or molecules (for example, the complete, partial or absence of ionization of a covalent compound in water). II. Typical Ionic Reactions You will experiment with a number of ionic type reactions to determine their essential nature. By conductivity tests of the separate reactants and the mixture after reaction, discover whether the acids, bases and salts are highly conductive, weak to moderate conductive or non- conductive. a. While stirring with the electrodes, carefully pour the 0.1M HCI solution into the 0.1M NaOH solution. Measure and record the conductivity of the products of the reaction. b. Measure the conductivity of the 15 mL sample of 0.1M H2SO, and 0.1M Ba(OH)2 solutions separately. Add one or two drops of phenolphthalein to the acid solution. While stirring with the electrodes, carefully pour the base solution into the acid solution (slowly). Add more base slowly until a permanent faint pink end-point is reached. Measure and record the conductivity of the products of the reaction (at the end-point). c. While stirring with the electrodes, carefully pour the 0.1M HC2H3O2 (acetic acid) solution into the 0.1M NH,OH solution. Measure and record the conductivity of the products of the reaction.
Transcribed Image Text:I. Electrolytes and Non-electrolytes Using the conductivity meter, record the reading for each of the substances and mixtures listed on Data Sheet 1. Make all measurements in 30- or 50 mL beakers. Always rinse the electrodes of the conductivity meter and all reaction containers with distilled water. Ensure that all flasks are completely dried before measuring the conductivity of any solid material. Use approximately 15 mL of each liquid. While stirring with electrodes, press the high scale setting on the meter (if applicable) and record the conductivity. From the conductivity meter: A reading of zero indicates non-conductive A reading of one through seven indicates weak to moderate conductivity A reading greater than seven indicates strong conductivity. Next to the conductivity reading on your data sheet, indicate the specific ions or molecules that gave rise to the observed reading. In the last column, explain the source of these ions and/or molecules (for example, the complete, partial or absence of ionization of a covalent compound in water). II. Typical Ionic Reactions You will experiment with a number of ionic type reactions to determine their essential nature. By conductivity tests of the separate reactants and the mixture after reaction, discover whether the acids, bases and salts are highly conductive, weak to moderate conductive or non- conductive. a. While stirring with the electrodes, carefully pour the 0.1M HCI solution into the 0.1M NaOH solution. Measure and record the conductivity of the products of the reaction. b. Measure the conductivity of the 15 mL sample of 0.1M H2SO, and 0.1M Ba(OH)2 solutions separately. Add one or two drops of phenolphthalein to the acid solution. While stirring with the electrodes, carefully pour the base solution into the acid solution (slowly). Add more base slowly until a permanent faint pink end-point is reached. Measure and record the conductivity of the products of the reaction (at the end-point). c. While stirring with the electrodes, carefully pour the 0.1M HC2H3O2 (acetic acid) solution into the 0.1M NH,OH solution. Measure and record the conductivity of the products of the reaction.
In the space provided, write the balanced IONIC and NET IONIC equation. 3. _HNO, + Al(OH); H20 + Al(NO3); Str. elect. ionic, insol. ionic, sol. IONIC: NET IONIC: 4. HCI + Mg(CH3O2)2 -> MgCl2 + HC,H;O2 Str. Elect. ionic, sol. ionic, sol. wk. Elect. IONIC: 10 of 12 CHM1045L Exp. #5: ELECTROLYTES AND NONELESTROLYTES NET IONIC:
Transcribed Image Text:In the space provided, write the balanced IONIC and NET IONIC equation. 3. _HNO, + Al(OH); H20 + Al(NO3); Str. elect. ionic, insol. ionic, sol. IONIC: NET IONIC: 4. HCI + Mg(CH3O2)2 -> MgCl2 + HC,H;O2 Str. Elect. ionic, sol. ionic, sol. wk. Elect. IONIC: 10 of 12 CHM1045L Exp. #5: ELECTROLYTES AND NONELESTROLYTES NET IONIC:
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