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2014-03-12 16:44:06
2014-03-12 16:44:06

Exactly how you prepare will depend on what you are starting with. Typically to make a 1 M HCl solution, you will be starting with a stock solution of more concentrated HCl that you will then dilute.

See the Related Questions for complete instructions on how to prepare a solution by diluting a stock solution.

1M HCl Solution*Concentrated HCl. its 37.5%.

*The density of concentrated HCl is 1.189g/ml we will need this number as well, and of course the atomic mass of HCl 36.46

* Calculation=((37.5/100)(1000)(1.189))/36.46 = 12.2M

*If HCl concentrated is 12.2 M then to make a 1L solution of 1M HCL

(12.2) x = 1(1)

x = 1(1)/(12.2)

x=0.082ml/ml of water

x = 82mL HCl per liter


Related Questions

How to prepare 2M HCl solution from con HCl

To prepare a .1 M solution, the ratio would be .1 moles of HCl per liter of water. This is equal to 3.65 grams HCl.

10N HCl is equivalent to 10 M HCl and the solution will contain 10 moles of HCl per 1 liter or solution. Depending on the volume of solution, the preparation will vary. To prepare 1 liter, place 360.5 g of HCl in a total volume of 1 L. To prepare 1 L from concentrate HCl (12.1 M) dilute 833 ml of conc. HCl to 1 L.

Prepare HCl 1 M by HCl concentration 37 % HCl concentration 37 % have density =1.19 g/ml HCl 1 M use HCl 37 % 82.81 ml make volume with water to 1 liter

one mole of HCl in one litre of water, result in 1M HCl

0.25 N HCl is the same as 0.25 M HCl which is 0.25 moles HCl/liter of solution.

8.3ml HCl from 37% v/v stock bottle is required to prepare 0.1 M HCl solution.(answered by Prof.WASEEM UR RAHMAN KHAN)

You're going to dilute the 1 M HCl in water to get a less concentrated 0.25 M HCl. First determine the amount of moles in the final 10 mL 0.25 M HCl. 10 mL = .01 L × .25 moles/L = .0025 moles HCl Now you work backwards with the concentrated solution. 1 mol/L × (volume) = .0025 moles HCl Volume = .0025 liters = 2.5 mL You need to prepare a 10 mL aqueous solution containing 2.5 mL of 1 M HCl.

dilute your HCl solution to 0.2 M HCl solution and then follow above mentioned link :

Look at the bottle of HCl. It gives a molarity. then dilute to 0.25 M.

To prepare a 5M HCl solution, you need to know the concentration of your source of HCl. Then you can use this proportion C1V1=C2V2, where C=Concentration in M(moles/liter) and V=Volume(liters).

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.

Molarity = moles of solute/Liters of solution ( 50 mL = 0.05 Liters )1 M HCl = X moles HCl/0.05 Liters= 0.05 moles HCl (36.458 grams/1 mole HCl)= 1.8 grams HCl============Add this mass HCl to your 50 mL opf solution.

You mean 0.1 M HCl? -log(0.1 M HCl) = 1 pH

33.3 ml of 3.0 M HCl should be filled up and mixed with water up to 100.0 ml of a 1.0 M HCl solution.

0.05 M means 0.05 mol of HCl in 1 Litter of solution

0.2 N HCl solution means 0.2 equivalents of HCl dissolved in 1 litre of water. Normality = Molarity x n-factor => Molarity =Normality/n-factor=0.2/1=0.2 M 0.2 moles should be present in 1 litre of solution. 0.2moles =0.2 x 36.5 = 7.3 grams of HCl =>Dissolve 7.3 grams of HCl in 1 litre if water to get a 0.2N solution.

You should also know the density of the 32 %(m/m) HCl.Maybe found answer in 'Related questions':"How do you prepare a_solution of 1 M HCL using 35 percent HCL", a link is just below this answer.


4.01 is the amount of pH in a 1.5 M HCl solution.

Molarity gives the no. of moles of solute per litre of the solutionFor instance, 1 M HCl means 1 mole of pure HCl in 1 L of water

The answer is 19,67 mL HCl 6,1 M to obtain 1 L of HCl 0,12 M.

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