How many grams of HCl need to be dissolved in 0.5L of water to prepare a solution of pH 1.5?
Does anybody know how to work this out?
Thanks :)
To determine the grams of HCl needed to prepare the solution, we need to use the concept of molarity (M) and the volume of the solution. Here are the steps to calculate the grams of HCl:
1. Determine the molarity required for a pH of 1.5.
pH is a measure of hydrogen ion concentration. In a solution, pH represents -log[H+], where [H+] is the hydrogen ion concentration. A pH of 1.5 means that the hydrogen ion concentration is equal to 10^(-1.5) M.
2. Calculate the moles of HCl required.
The mole is a unit of measurement used in chemistry. To convert from molarity (M) to moles (mol), we multiply the molarity by the volume in liters. In this case, the volume is given as 0.5 L.
Moles of HCl = Molarity (M) x Volume (L)
Moles of HCl = 10^(-1.5) M x 0.5 L
3. Calculate the grams of HCl.
The molar mass of HCl is approximately 36.5 g/mol. Therefore, to convert moles to grams, we multiply the moles of HCl by the molar mass.
Grams of HCl = Moles of HCl x Molar mass of HCl
Grams of HCl = (10^(-1.5) M x 0.5 L) x (36.5 g/mol)
By following these steps, you can determine the grams of HCl needed to prepare a solution of pH 1.5.