Lab of Electrolytes

Topics: Potassium, Sulfuric acid, Sodium chloride Pages: 3 (608 words) Published: January 30, 2013
Analyzing electrolytes

I. Introduction

Ionic substances form when a metal reacts with a non-metal. They contain charged particles called ions. Those ionic substances are broken down by electrolysis. Electrolysis is the breakdown of a substance by electricity, and it only happens in liquids. The liquids that can be electrolyzed are called electrolytes. When said electrolyzed, means that the compounds in solutions are broken down when they conduct electricity. Its necessary the use of electrodes since it conducts the electricity to the solution. The electrodes are needed to be an anode, which receives the negative ions, and the cathode, which receives the positive ions.

II. Materials

* College power unit
* Black and red wires
* Beakers
* Carbon road
* 9 different solutions

III. Procedure

1. Separate each solution in different beakers.
2. Connect the black and red wires properly and turn on the college power unit. 3. Attach the wires to the carbon road that acts as electrodes, one for cathode one for anode. 4. Set up the circuit as shown for each substance and observe the results.

IV. Data table and observations

Potassium Chloride (KCl)| Yes| Bubbles | More bubbles than in anode | Glucose (C6H12O6)| No | Nothing changes| Nothing changes | Dilute Sulfuric Acid (H2So4)| Yes| Bubbles | Bigger bubbles | Sucrose (C12H22O11)| Yes| Light bubbles | Light but more visible bubbles and light brown liquid| Copper Sulfate (CuSo4)| Yes| Light bubbles| Changes color to brown and oxidation is observed | Ethanol (c2H5OH)| No| Nothing changes| Nothing changes| Calcium Hydroxide (Ca(OH)2)| Yes| Light bubbles | Light bubbles but more than in anode | Potassium Bromide (KBr2)| Yes| Produced yellow color and bubbles | Bubbles| Sodium Iodide (NaI)| Yes| Produced yellow brown and bubbles | A lot of...
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