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You will need to know the molarity of the solution you work from. Remember when working with acid - always put acid to the water, never vice versa.
If you have a 1M solution you will need to put 20 times the amount of water.
If you have a 5M solution you will need to 100 times the amount of water.
It is more difficult if the basic solution is given in percentage. In this case you have to calculate how much HCl the solution contains.
Eks::
A 37% HCl has a density of 1,19g/cm3 and a molarity of 12,1 (12,1M). so the amount of water will be 242 times more to get the specified solution.
Be very careful if you are working with this stuff - you could get injuries on you skin, eyes and lounges.
Wiki User
∙ 11y ago
Wiki User
∙ 11y agoWeigh accurately 0.5gm of Anhydrous Sodium Carbonate and dissolv in 20 ml of distilled water.
Titrate this solution with the prepared 0.5N Hydrochloric Acid using methyl orange as an indicator until the appearance of reddish-yellow color as end point. Boil for 2 minutes and continue the titration until the appearance of reddish-yellow color.
1ml of 0.5N Hydrochloric Acid is equivalent to 26.5 mg of anhydrous Sodium Carbonate.
CALCULATIONS:
Wt. of Anhydrous Sodium Carbonate in gm x 1000 x 0.5
A) Normality = ---------------------------------------------------------------------26.5 x Volume of 0.5N HCl consumed
Wiki User
∙ 10y ago0.05 M means 0.05 mol of HCl in 1 Litter of solution
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How do you prepare 0.2N HCl solution from 1.0N HCl?
Add 200 mls of the 1.0N HCl solution to a 1 liter volumetric flask. Make up to the mark with water. Standardize against a known weight of Sodium Carbonate.
Why do you need to standardize HCl solution?
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.
How much concentration HCl in HCl fuming 36 percent?
About 13M. You can assume it is 13M if you don't need an exact concentration (like if you need a ~1M HCl solution for an extraction or whatever) but if you need an exact concentration (for a titration, for example) then you will need to standardize your HCl first.
What happens when HCl is mixed with a solution that is not a buffer solution?
If the solution is not a buffer, the HCl will react with the solution to form a product.
How to prepare 1N HCl solution?
1N HCl is also 1M HCl because it is mono-protic. Therefore 36.5 g of HCl is required per liter or 3.65%. Simply take 100 g of 37% HCl and make up to the 1 liter mark on the volumetric flask. Check the value by titration against 1M NaOH. It should be perfect. If very slightly strong dilute very slightly (calculate) with water and re-standardize.
Why you need to standardize HCl solution?
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.
How do you prepare 0.2N HCl solution from 1.0N HCl?
Add 200 mls of the 1.0N HCl solution to a 1 liter volumetric flask. Make up to the mark with water. Standardize against a known weight of Sodium Carbonate.
Why do you need to standardize HCl solution?
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.
How much concentration HCl in HCl fuming 36 percent?
About 13M. You can assume it is 13M if you don't need an exact concentration (like if you need a ~1M HCl solution for an extraction or whatever) but if you need an exact concentration (for a titration, for example) then you will need to standardize your HCl first.
What happens when HCl is mixed with a solution that is not a buffer solution?
If the solution is not a buffer, the HCl will react with the solution to form a product.
How to prepare 1N HCl solution?
1N HCl is also 1M HCl because it is mono-protic. Therefore 36.5 g of HCl is required per liter or 3.65%. Simply take 100 g of 37% HCl and make up to the 1 liter mark on the volumetric flask. Check the value by titration against 1M NaOH. It should be perfect. If very slightly strong dilute very slightly (calculate) with water and re-standardize.
What is the molarity of an hcl solution if 7ml hcl solution is titrated with 27.6ml of 0.170m of naoh solution?
(7 mL)(X M HCl) = (27.6 mL)(0.170 M NaOH)7X = 4.692X = 0.7 M HCl==========
Is HCL acidic in aqueous solution?
If it is only HCL, yes.
What is hydrochloric acid and acid in a aqueous solution?
HCl is ionozed in aq solution HCl + H2O = H3O(+ CHARGE) + Cl (- CHARGE) HCl FORMULA WILL REAMAIN HCl OT WILL BOT CHANGE
What is the molarity of a solution in which 0.597 moles of HCl are dissolved in 0.169 liters of solution?
Molarity = moles of solute/liters of solution Molarity = 0.597 moles HCl/0.169 liters = 3.53 M HCl ------------------
Does a solution of HCl contain electrolytes?
Yes. HCl is a strong electrolyte.
How many moles of HCL is present in 1 liter of stomach solution that has a PH of 1?
In solution with a pH of 1 [H+] is 0.1M. Since HCl is a strong acid [HCl] will also be 0.1M. So, in 1 liter of solution you will have 0.1 mol of HCl.
