please me solve During an experiment to measure the efficacy of an antacid tablet, an antacid tablet was dissolved in deionized water. Then 75.0 milliliters of 0.268 M HCl solution were added to the flask containing the dissolved tablet. How many moles of HCl were added to the tablet?
mols HCl added = M x L = ?
To solve this problem, we need to use the concept of molarity and the equation of stoichiometry to determine the number of moles of HCl added to the antacid tablet.
First, we need to find the number of moles of HCl solution added to the flask. We can do this using the equation:
moles of solute = concentration x volume
In this case, the concentration of the HCl solution is 0.268 M and the volume is 75.0 milliliters. However, it is important to convert the volume to liters in order to use the correct units in the equation. So, 75.0 milliliters is equal to 0.0750 liters.
moles of HCl solution = 0.268 M x 0.0750 L = 0.0201 moles
Next, we need to understand the stoichiometry of the reaction between the antacid tablet and HCl. Typically, the active ingredient in an antacid tablet is a base, such as calcium carbonate (CaCO3), which reacts with the acid (HCl) to form carbon dioxide gas (CO2), water (H2O), and a salt. The balanced equation for this reaction is:
CaCO3 + 2HCl → CO2 + H2O + CaCl2
From the balanced equation, we can see that 2 moles of HCl react with 1 mole of CaCO3. So, 0.0201 moles of HCl will react with half that amount of CaCO3.
moles of HCl in the tablet = 0.0201 moles / 2 = 0.01005 moles
Therefore, 0.01005 moles of HCl were added to the antacid tablet.