Student Successfully Prepares 150.0 mL of 1.40 M HCl Solution for Laboratory Use
A student prepares 150.0 ml of 1.40 M HCl, a highly corrosive and dangerous chemical, with great care and precision. The process involves several steps to ensure the accuracy of the concentration and the safety of the person conducting the experiment. In this article, we will explore the details of this procedure, the importance of maintaining the correct concentration, and the potential risks associated with handling such a potent substance.
The first step in preparing the 1.40 M HCl solution is to gather all the necessary equipment and materials. This includes a 150.0 ml volumetric flask, a graduated cylinder, a pipette, and the concentrated hydrochloric acid. The student must wear appropriate personal protective equipment (PPE), such as gloves, goggles, and a lab coat, to minimize the risk of exposure to the acid.
Next, the student measures out the appropriate amount of concentrated HCl using the graduated cylinder. The concentration of the concentrated acid is typically around 36.5% by weight, which corresponds to approximately 12.1 M. To achieve the desired 1.40 M concentration, the student must dilute the concentrated acid with water. The calculation for the required volume of concentrated acid is as follows:
M1V1 = M2V2
12.1 M x V1 = 1.40 M x 150.0 ml
V1 = (1.40 M x 150.0 ml) / 12.1 M
V1 ≈ 18.0 ml
Therefore, the student needs to measure out approximately 18.0 ml of the concentrated HCl using the pipette and transfer it to the 150.0 ml volumetric flask.
After adding the concentrated acid to the flask, the student carefully adds distilled water to the flask while swirling it gently to ensure thorough mixing. The student must be cautious not to exceed the marked volume on the flask, as this could lead to an inaccurate concentration. Once the water reaches the mark, the student stops adding water and continues to swirl the flask for a few minutes to ensure the solution is homogeneous.
The importance of maintaining the correct concentration of HCl cannot be overstated. HCl is a strong acid that can cause severe burns and respiratory irritation. The concentration of the acid determines its potential to cause harm, and a miscalculation could lead to dangerous consequences. In addition, the reaction between HCl and certain substances can produce toxic gases, such as hydrogen chloride, which can be harmful if inhaled.
In conclusion, the process of preparing 150.0 ml of 1.40 M HCl requires careful attention to detail and adherence to safety protocols. The student must ensure the accuracy of the concentration and take appropriate precautions to protect themselves and others from the potential dangers associated with handling such a potent chemical. By following the proper procedures, the student can safely conduct experiments and contribute to the advancement of scientific knowledge.
