How do you prepare 1N solution of 35.4 percent HCl?

Answer 1

As it is in the form of liquid dilute it with water for eg.,to make 10 ml of 5% H CL Take 0.5 ml of H CL and add 9.5 ml of water. this is based on the calculation Volume percent is a common expression of a solution,s concentration It is defined as:

Answer 2

you are not mentioned the desired volume.

for example you want to prepare 0.25 M HCl in 100 ml. To make a 0.25 M solution, slowly add 2.207 mL of your stock (HCl) solution to 25 mL deionized water. Adjust the final volume of solution to 100 mL with deionized water.

Answer 3

From interpolation of table values: (between 34% and 36%)

35.4 %(m/m) HCl = Concentration 416 g HCl/L = 21.7 oBaume = density 1.176 kg/L = molarity 11.42 mol/L

[cf. link to in Related links on: Concentration table of concentrated HCl solutions]

To prepare an 1.0 N HCl (= 1.0 Molar) solution you take

• 10.0 mL of the original and add up the volume to exactly 114.2 mL.

  Or you take

• 100/11.42 mL, which is 8.76 mL, and add up to 100 mL

Answer 4

From interpolation of table values: (between 34% and 36%)

35.0 %(m/m) HCl => Concentration 413 g HCl/L => density 1.174 kg/L => molarity 11.27 mol/L

[cf. link to in Related links on: Concentration table of concentrated HCl solutions]

To prepare an 1.0 M HCl (= 1.0 Molar) solution you take

• 10.0 mL of the original 35%HCl and add up the volume to exactly 112.7 mL.

  Or you take

• 100/11.42 mL, which is 8.87 mL, and add up to 100 mL

Answer 5

In order to prepare a 1 percent HCl solution, a specific ratio of the 35 percent solution must be added per liter. This ratio is 29.5 milliliters of stock solution per liter of water.

Answer 6

In order to concentrate hydrochloric acid solution, the mixture would need to be distilled.

Answer 7

Add solvant.

Answer 8

yes