I have liquid concentrated HCl (37%w/w)
To prepare 100ml of 10g/L HCl as a solvent medium, is it acceptable to just weigh 1g of liquid conc HCl and dilute to 100ml with water?
What volume of conc HCl should we use to make 100ml of 10g/L HCl?
I don't think so. 37% w/w HCl has a density of 1.19 (you can look on the bottle for specific gravity and it may be listed as 1.18 or so). So you have
1000 mL x 1.19 g/mL x 0.37 = approximately 440 g in that 1 L.
If you weigh 1 g of the concd acid that will give you 0.37 g HCl and that isn't the equivalent of 10 g HCl/L.
If 45.5 mL of He at 25.0°C and 101.3 kPa were heated to 75.0°C, what would be the volume?
To determine the volume of concentrated HCl needed to make 100ml of a 10g/L HCl solution, you need to consider the concentration of the liquid concentrated HCl (37% w/w) and the desired concentration of the final solution (10g/L).
To calculate the amount of HCl needed, you can use the following equation:
(Concentrated HCl volume) x (Concentrated HCl concentration) = (Final solution volume) x (Final solution concentration)
Let's solve it step-by-step:
1. Convert the concentration of the liquid concentrated HCl from w/w (weight/weight) to g/ml (gram/milliliter).
To do this, you need to know the density of the concentrated HCl. For this example, let's assume it's 1.18 g/ml. Multiply the concentration by the density:
37% x 1.18 g/ml = 0.37 g/ml
2. Substitute the known values into the equation and solve for the concentrated HCl volume:
(Volume of concentrated HCl) x (0.37 g/ml) = 100 ml x 10 g/L
(Volume of concentrated HCl) x (0.37 g/ml) = 1000 g
3. Solve for the volume of concentrated HCl:
(Volume of concentrated HCl) = 1000 g / (0.37 g/ml)
Volume of concentrated HCl = 2702.70 ml
So, you would need approximately 2702.70 ml (or 2.7 liters) of the liquid concentrated HCl to prepare 100 ml of a 10g/L HCl solution.
Therefore, weighing just 1g of the concentrated HCl and diluting it with water to make 100 ml would not result in a 10g/L HCl solution.