Commercially available conc. HCl contains 38% HCl by mass. (a) What is the molarity of this solutions. The density is 1.10 g ML-1? (b) What volume of conc. HCl is resumed to make 1.00 L of 0.10 M HCl?

Conc. HCl is 38% HCl by mass. What is the molarity of this solution is d=1.19 g cm^(-3) ? What volume of conc. HCl is required to make 1.00 L of 0.10 M HCl?

Commercially availiable concentrated hydrochloric acid contains 38% HCl by mass. (a) What is the molarity of this solution? The density is 1.19g mL^(-1) ? (b) What volume of concentrated HCl is required to make 1.00 "litre" of 0.10M HCl ?

Commercially available concentrated hydrochlorc acid contains 38% HCI by mass. (i) What is the molarity of this solution? The density is 1.19 g cm^(-3) . (ii) What volume of concentrated HCI is required to make 1.00 L of 0.10 M HCI?

Commercially available HCl contains 38% HCl by mass. Calculate molarity of solution if the density is 1.19 g/ml.

Commercially available concentrated hydrochloric acid contains 38 % HCl by mass. (i) What is the molarity of the solution if its density is 1.19 "g cm"^(-2) ? (ii) What volume of concentrated HCl is needed to make 1.0 L of 0.2 M HCl solution ?

Commercially available concentrated HCI contains 38.0% HCl by mass (density = 1.19 g mL^(-1) ). The molarity of the solution is