For preparation of 4N solution of sulphuric acid
Dissolve 196 gm H2SO4 in 1000 ml DM water.
Calculation
N E V
Weight = ------------
1000
Where
N= Normality
E= Equivalent weight
V= Volume
To prepare 0.1 N sulphuric acid, you can dilute concentrated sulphuric acid with water in a specific ratio. For 0.1 N solution, you would mix 1.4 ml of concentrated sulphuric acid (98% H2SO4) with water to make 1 liter of solution. Remember to add acid to water slowly while stirring to avoid splattering.
normality of A = #gram equivalent weights A divided by #litres of solution
thus: measure a gram equivalent of H2SO4 (49g) and add to 1000ml volumetric flask that has 500ml deionized distilled H2O. stopper flask, mix by swirling, open flask and fill to 1000ml mark, thoroughly mix
OR
1N H2SO4 = 0.5M H2SO4
volumetrically measure 500ml 1M H2SO4
volumetrically transfer to 1000ml volumetric flask (using DDH2O)
fill to 1000ml mark with DDH2O
mix
OR
1) Measure 28ml Sulphuric Acid (95% reagent grade)
2) Transfer all into voulmetric flask (contain 500ml Carbon dioxide free distilled water)
3) Mix by swirling
4) Fill up to 1000ml mark with CO2 free distilled water.
Sulphuric acid Equivalent weight = 49
Normality you can decided i.e. you prepare 0.1N
water 1 lit of water
First = Eq.wt x 0.1 N x 1 lit of water
= 49 x 0.1 x 1= 4.9 g
Sulphuric acid you only measure only ml
so you put = gram / (Specific Gravity x Percentage Concentration)
= 49 / (1.83x97)
= 49/177.51
= 2.76 ml of Sulphuric acid you take one litre of water
0.01 N sulphuric acid means 0.01 equivalents dissolved in 1 litre of water.
Nomality = Molarity x n-factor
=> molarity= normality /n-factor
molarity = 0.01/2=0.005 M
[ n-factor of sulphuric acid is 2]
Thus, a 0.01N solution of sulphuric acid contains 0.005 moles of sulphuric acid in 1 litre.
0.005 moles=0.005 x 98 = 0.49 grams.
=> Dissolve 0.49 grams of sulphuric acid in 1 litre water to make a 0.01N solution
The normality of sulphuric acid in the bottle is 36N
But we dont know how much ml we have to take from the bottle.
to make clear go through the calculation....
preparing 0.01 N in 1000ml
X * 36N =0.01 *1000ml
x=0.27 ml (but it is very difficult to measure,,,so you first prapare 10N of sulphuric acid
X * 36N = 10N *100ML
X=27.7 ml of sulphuric acid and add 73.3 ml of water to makeup for 100ml(10N SULPHURIC ACID)
FROM the 10N
X* 10N = 0.01N *1000
X=1ml of sulphuric acid mixed in 999ml of water
Add one mole of sulphiric acid to one liter of water.
The concentrated available has a normality of 36. so when you need to prepare 0.01 N Sulfuric acid calculate accordingly.
20 ml 2 normal dilute sulphuric acid means?
7 N h2s04
how do prepare 0.1 N Oxalic acid
To prepare N-phenylanthranilic acid indicator, dissolve 0.1 g of N-phenylanthranilic acid in 100 ml of ethanol or methanol. This will create a stock solution of the indicator that can be diluted further as needed for specific applications.
To prepare 0.02 N sulfuric acid, dilute concentrated sulfuric acid with water in a specific ratio. For example, to prepare 100 ml of 0.02 N sulfuric acid, you would mix 0.4 ml of concentrated sulfuric acid (98% purity) with 99.6 ml of water. It's crucial to handle concentrated sulfuric acid with caution due to its corrosive nature.
To prepare a 60% sulfuric acid solution, you would mix 60 parts of concentrated sulfuric acid (usually 98% purity) with 40 parts of water. Always remember to add acid to water slowly while stirring continuously and handle with care due to the corrosive nature of sulfuric acid.
Octyl benzoate can be formed by reacting octanol (alcohol) and benzoic acid in the presence of a catalyst like sulfuric acid. The reaction will produce octyl benzoate and water as byproduct.
yes
how do prepare 0.1 N Oxalic acid
when we add water n sulphuric acid then dilute sulphuric acid is formed. But we have to mix concentrated acid to water not water to acid otherwise the container in which u r mixing may explode because this reaction is highly exothermic.
The acid-catalyzed dehydration of tertiary butanol is faster than that of n-butanol because the tertiary carbocation intermediate formed in the reaction is more stable than the secondary carbocation formed in the dehydration of n-butanol due to greater hyperconjugation and steric hindrance. This stability facilitates the elimination reaction leading to a faster overall reaction rate.
Yes
Yes, mixing Strip-n-All with sulfuric acid can be dangerous as it can release harmful gases and potentially cause a chemical reaction that produces heat or even an explosion. It is not recommended to mix these two substances.
Yes, mixing Strip-N-All with sulfuric acid can produce toxic gases due to the reaction between the ingredients. This combination should be avoided as it can lead to the release of harmful fumes and pose serious health risks.
Different types of urine preservatives are boric acid, tartaric acid, thymol, clorhexidine/ n-propyl gallate and sulphuric acid.
To prepare N-phenylanthranilic acid indicator, dissolve 0.1 g of N-phenylanthranilic acid in 100 ml of ethanol or methanol. This will create a stock solution of the indicator that can be diluted further as needed for specific applications.
To prepare 0.02 N sulfuric acid, dilute concentrated sulfuric acid with water in a specific ratio. For example, to prepare 100 ml of 0.02 N sulfuric acid, you would mix 0.4 ml of concentrated sulfuric acid (98% purity) with 99.6 ml of water. It's crucial to handle concentrated sulfuric acid with caution due to its corrosive nature.
To prepare a 60% sulfuric acid solution, you would mix 60 parts of concentrated sulfuric acid (usually 98% purity) with 40 parts of water. Always remember to add acid to water slowly while stirring continuously and handle with care due to the corrosive nature of sulfuric acid.
Octyl benzoate can be formed by reacting octanol (alcohol) and benzoic acid in the presence of a catalyst like sulfuric acid. The reaction will produce octyl benzoate and water as byproduct.