I had conducted an experiment to figure out the percent by mass of baking soda in a mixture by titration. I had to standardize 1.0M HCl. Through the standardization process and the titration curve of the primary standard and the HCl, the molarity has to be found, but is this step really necessary since the molarity of Hcl is 1.0M?
Yes, unless you were told that the HCl you had was 1.000 M. Usually you are given instructions for preparing 1M HCl but those instructions only get a solution that is close to being 1.00M. You must standardize to find out EXACTLY what it is such as 0.1011M or 0.09876M
The step of standardizing the 1.0M HCl solution is necessary to ensure accuracy in your titration experiment. Although you are starting with a 1.0M HCl solution, it is important to determine the precise concentration because variations in concentration can occur due to factors such as impurities, evaporation, or dilution during storage.
To standardize the HCl solution, you need to titrate it against a primary standard, which is a substance with a known concentration that is stable and easy to handle. This allows you to determine the exact concentration of your HCl solution.
During standardization, you perform a titration with a known amount of the primary standard and the HCl solution. By comparing the volumes used and applying the stoichiometry of the balanced equation, you can calculate the precise concentration of the HCl solution.
Once the HCl solution is standardized, you can be confident in using it to titrate your mixture and determine the percent by mass of baking soda accurately. Without this step, potential errors in concentration could lead to incorrect results in your final calculation.