Final answer:
The volume of concentrated HCl needed to make a 10 L solution with a pH of 2.10 is approximately 6.85 ml.
Step-by-step explanation:
This question involves solving a chemistry problem using molarity and density calculations. In this context, we are asked about the volume of concentrated HI solution, which is 36.0% HCl by mass and has a density of 1.179 g/ml, that should be used to make 10.00 L of an HCl solution with a pH of 2.10.
Firstly, it's important to note that pH is a measure of the hydrogen ion concentration in a solution. A pH of 2.10 indicates a HCl concentration of 10^-2.10 M, or 0.00794 M. Therefore, the number of moles of HCl needed in the 10.00 L solution is that value multiplied by 10.00 L, or 0.0794 mol.
From the given information, we know that the concentrated solution is 36.0% HCl by mass, which means that there are 360 g of HCl in every 1000 g of solution. The density of the solution is given as 1.179 g/ml, so in 1 ml of the solution, we have 1.179 g of total mass, from which 0.424 g is HCl (36.0% of 1.179 g).
Next, convert 0.424 g of HCl in every ml of solution into moles by dividing by the molar mass of HCl (36.46 g/mol), which results in 0.0116 mol/ml. Therefore, the volume of the concentrated solution required to make 10.00 L of a 0.00794 M HCl solution would be approximately 6.85 ml (0.0794 mol divided by 0.0116 mol/ml).
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