The reaction of Iron with Copper(II) Sulfate
Lab: STOICHIOMETRY
The reaction of Iron with Copper(II) Sulfate
Purpose: In this experiment we will use stoichiometric principles to deduce the appropriate equation for the reaction between metallic iron and a solution of copper (II) sulfate. This reaction produces metallic copper, which is seen precipitating as a finely divided red power.
Materials: Flask beaker Copper solution Balance Hot plate •150 ml beaker •1 gram of iron power •30 ml of CuSO₄
Procedure: Weigh a clean dry 150 ml beaker. Accurately weigh approximately 1 gram of iron power into the beaker. Do not exceed 1 grams. Measure 30 ml of 1 M. CuSO solution into a graduate cylinder. Pour it into an Erlenmeyer flask, and heat gently to almost boiling. Slowly add the hot CuSO solution to the beaker containing the iron power. Be sure the addition is slow to avoid excess frothing and possible loss of material. It will help to avoid frothing if a wood splint is placed in the beaker before adding the hot CuSO solution. Swirl the beaker to insure a complete reaction. When the reaction has ceased, allow the copper product to settle. Then carefully decant the liquid from the copper, ( pour off the liquid and leave the solid behind). You may observe a thin copper colored sheen on the surface of the liquid which does not settle out. You may ignore this. Dad about 10 ml of water to the solid copper in the beaker and swirl to wash any remaining ions from the copper. Decant the wash water from the copper and add 10 more ml of distilled water, swirl and decant again. Now add several ml of acetone (CAUTION Acetone is very flammable) to the copper. Swirl and allow to stand a few minutes and decant off the acetone. Repeat with a second portion of acetone. Discard the acetone in the organic Wastes beaker (in the fume hood). The acetone readily dissolves the water removes it.
The acetone is easily removed by gentle heating since acetone
The reaction of Iron with Copper(II) Sulfate
Purpose: In this experiment we will use stoichiometric principles to deduce the appropriate equation for the reaction between metallic iron and a solution of copper (II) sulfate. This reaction produces metallic copper, which is seen precipitating as a finely divided red power.
Materials: Flask beaker Copper solution Balance Hot plate •150 ml beaker •1 gram of iron power •30 ml of CuSO₄
Procedure: Weigh a clean dry 150 ml beaker. Accurately weigh approximately 1 gram of iron power into the beaker. Do not exceed 1 grams. Measure 30 ml of 1 M. CuSO solution into a graduate cylinder. Pour it into an Erlenmeyer flask, and heat gently to almost boiling. Slowly add the hot CuSO solution to the beaker containing the iron power. Be sure the addition is slow to avoid excess frothing and possible loss of material. It will help to avoid frothing if a wood splint is placed in the beaker before adding the hot CuSO solution. Swirl the beaker to insure a complete reaction. When the reaction has ceased, allow the copper product to settle. Then carefully decant the liquid from the copper, ( pour off the liquid and leave the solid behind). You may observe a thin copper colored sheen on the surface of the liquid which does not settle out. You may ignore this. Dad about 10 ml of water to the solid copper in the beaker and swirl to wash any remaining ions from the copper. Decant the wash water from the copper and add 10 more ml of distilled water, swirl and decant again. Now add several ml of acetone (CAUTION Acetone is very flammable) to the copper. Swirl and allow to stand a few minutes and decant off the acetone. Repeat with a second portion of acetone. Discard the acetone in the organic Wastes beaker (in the fume hood). The acetone readily dissolves the water removes it.
The acetone is easily removed by gentle heating since acetone