The purpose of this experiment is to observe the reaction between magnesium (Mg) and a solution containing sodium chloride (NaCl), hydrogen peroxide (H2O2), and potassium hydroxide (KOH). This reaction is an example of a single displacement reaction in which the more reactive magnesium metal displaces the less reactive hydrogen in the solution, resulting in the formation of magnesium hydroxide (Mg(OH)2) and hydrogen gas (H2).
The materials required for this experiment include magnesium metal strips, a beaker or test tube, a solution containing NaCl, H2O2, and KOH, a balance, and a ruler. Additionally, safety equipment such as goggles and gloves should be worn when handling the materials.
The reaction between Mg (s) and NaCl+H2O2+KOH solution occurs through a redox reaction, where magnesium is oxidized and hydrogen is reduced. The magnesium metal reacts with the hydroxide ions (OH-) in the solution to form magnesium hydroxide and release hydrogen gas. The Cl- ions in the solution do not participate in the reaction, but rather act as spectators.
The rate of this reaction can be affected by several factors, including the surface area of the magnesium metal (smaller pieces will react faster), the concentration of the solution (higher concentration will result in a faster reaction), and the temperature of the solution (higher temperature will increase the reaction rate). Additionally, the presence of any impurities or inhibitors in the solution can also affect the reaction rate.
The potential hazards of this experiment include the use of chemicals such as NaCl, H2O2, and KOH, which can be corrosive and irritate the skin and eyes. Therefore, appropriate safety measures should be taken, such as wearing protective equipment and handling the chemicals with caution. Additionally, the reaction between Mg (s) and the solution can produce hydrogen gas, which is flammable and should be handled carefully.