Preparation of 1000 ml of N/10 HCl acid solution
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PREPARATION OF 1000 ml of N/10 HCl ACID SOLUTION/font>
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- HCl is a monobasic acid and is aqueous anhydrous.
Equivalent weight of HCl = Molecular weight / 1 = (1+35.5) / 1 = 36.5 / 1 = 36.5 = 36 g (approx.)
Specific gravity (of the commercially available HCl) = 1.18 (1.18 g of HCl / 1000 ml) = 1180 g of HCl / 1000 ml
- We know that 36 g of HCl in 1000 ml = 1 N
- Then, 1180 g of HCl in 1000 ml will be = 1 x 1180 N /36 = 32.78 N
- But the assay (purity) of the commercially available HCl solution = 36%
- Therefore, the actual normality will be =(36/100) x 32.78 = 11.79 N.
- We are required to prepare 1000 ml of 0.1N HCl using this above 11.79 N HCl stock solution.
- Therefore, the Volume of Stock (Conc.) HCl required can be calculated by using the equation:
V1N1 = V2N2
- Where, N1 = Normality of the Conc. HCl = 11.79 N
- V1 = Volume of the Conc.HCl (Unknown)
- N2 = Normality of HCl to be prepared = 0.1 N
- V2 = Volume of HCl to be prepared = 1000 ml
- Substituting the Values, we get 11.79 N x V1 = 0.1 N x 1000 ml
- Then, V1= ((0.1 N x 1000 ml )/11.79N)=8.48ml
- Therefore, 8.48 ml of HCl is diluted with distilled water to make up the volume to 1000 ml.
Procedure
- The Commercially available Conc. HCl is approximately 11.79 N.
- Take 8.4 ml of the above HCl and initially dilute it by slowly adding drop by drop and stirring it in about 500 ml of distilled water.
- Then make up the volume to 1000 ml in distilled water.
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Last modified: Friday, 16 December 2011, 11:29 AM