Given 100 mL of pure water at 40C, what volume of a solution of
hydrochloric acid, with a density of 1.175 g/mL and containing 34.4% HCI by weight, could be prepared?
4 answers
Sidney, I don't understand the question. Are you sure you have posted all of the problem?
yes! Given 100 mL of pure water at 4°C, what volume of a solution of
hydrochloric acid, with a density of 1.175 g/mL and containing 34.4% HCI by weight, could be prepared?
hydrochloric acid, with a density of 1.175 g/mL and containing 34.4% HCI by weight, could be prepared?
Sidney, I may be missing something but I don't think you can prepare any solution using pure water that contains HCl of any density/percent by mass.
The common manufactured stock of HCl from commercial producers is 35% and has a density of 1.175 g/ml. Practical applications typically extract a specific volume of the concentrated HCl and dilute to a desired volume. A more practical problem would read...
What volume of 5.25M can be prepared from a manufactured stock of HCl(35
%) having a solution density of 1.175 g/ml. (A stock of HCl(35%) is ~12M).
(Molarity x Volume)concentrate = (Molarity x Volume)diluted solution
(12M)(V) = (5.25M)(100 ml)
(Vol) of HCl(35%)
= [(5.25M)(100 ml)]/(12M)
= 43.75-ml of HCl(35%)
Mixing:
1st (for safety) add the 43.75-ml of stock concentrated HCl into a quantity of water less than 100ml such that after adding you still have less that 100 ml total mix. The purpose of this is to prevent acid flashing when adding a large quantity of water into concentrated HCl(35%).
The ionization rate will be so fast that sufficient heat buildup could cause acid flashback the is dangerous event. To moderate the rate of ionization of the concentrated acid is to slowly add the 43.75 ml of acid concentrate into about 25 to 30 ml of pure water. After preparing the premix, transfer the mix into a volumetric flask and then add the remaining amount of water up to but not to exceed the desired final volume. Always wear protective clothing, and appropriate eyewear when working with caustic systems.
What volume of 5.25M can be prepared from a manufactured stock of HCl(35
%) having a solution density of 1.175 g/ml. (A stock of HCl(35%) is ~12M).
(Molarity x Volume)concentrate = (Molarity x Volume)diluted solution
(12M)(V) = (5.25M)(100 ml)
(Vol) of HCl(35%)
= [(5.25M)(100 ml)]/(12M)
= 43.75-ml of HCl(35%)
Mixing:
1st (for safety) add the 43.75-ml of stock concentrated HCl into a quantity of water less than 100ml such that after adding you still have less that 100 ml total mix. The purpose of this is to prevent acid flashing when adding a large quantity of water into concentrated HCl(35%).
The ionization rate will be so fast that sufficient heat buildup could cause acid flashback the is dangerous event. To moderate the rate of ionization of the concentrated acid is to slowly add the 43.75 ml of acid concentrate into about 25 to 30 ml of pure water. After preparing the premix, transfer the mix into a volumetric flask and then add the remaining amount of water up to but not to exceed the desired final volume. Always wear protective clothing, and appropriate eyewear when working with caustic systems.