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The (N) stands for Normal. 1 Normal is 28 ml of concentrated sulfuric acid added to deionized water for a final volume of 1 Liter (L). 18 N is roughly a 50 percent concentration sulfuric acid.
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∙ 9y ago
Wiki User
∙ 14y ago6 normal, which for sulfuric acid is 3 molar.
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What ratio of acid to water would you use to dilute 18M sulfuric acid to 6M?
Since the ratio of 18:6 is 3:1, to dilute 18M sulfuric acid to 6M, one would use 2 parts water and 1 part acid, a total of 3 parts.
What is the normality of concentrated sulfuric acid?
About 36 N, 36 mole H+/L. (It contains 18 mole/L H2SO4)
How much of an 18 percent solution of sulfuric acid should be added to 360 ml of a 10 percent solution to obtain a 15 percent solution?
600ml.
What is the normality of 96 percent solution of sulphuric acid of specific gravity 1.84?
To find the molarity, we can set up the following factor labeling problem. Note that a specific gravity of 1.84 can be treated as a density of 1.84 g/ml. The molar mass of sulfuric acid (H2SO4) is 98.079 g /molM(mol/l)= (1.84 g/ 1 ml)(1000 ml/1 l)(1 mol/98.079 g)(.96 purity)= 18 mol/l= 18 MThe molarity is 18 mol/l. The pH of this solution would be -1.26...VERY ACIDIC.
How do you prepare 1M sulfuric acid from concentrated sulfuric acid?
To prepare 1M sulphuric acid from concentrated sulphuric acid:First consider the molecular weight of H2SO4 = 98 g/mol, so you have to add 98g of conc. acid and make up to 1 liter of water (as pointed out at the 4thpoint).Considering that acid is a liquid, you should also consider density: where density = mass/volume, which is said on the bottle to be (about) 1.84 g/mL,so then you have: volume = 98g / 1.84(g/mL) = 53.2 mLNow you have to consider the acid purity, usually 98% then you have to do this: 53.2 mL if the acid were 100% pure convert in mL given with the purity of 98%, so 100% x 53.2 mL / 98% = 54.3 mL of (98%) concentrated acid.Finally CAREFULLY add this 54.3 mL (or 98 g, cf. first point) to about 0.9 L dist. water while continuously stirring (evolving heat!), and after that fill it up to 1.00 L with also dist. water. Never reverse this: DO NOT add water to concentrated fluids!
What has more mass water or sulfuric acid?
The molecular maass of sulfuric acid (98,08) is greater than the molecular mass of water (18).
What ratio of acid to water would you use to dilute 18M sulfuric acid to 6M?
Since the ratio of 18:6 is 3:1, to dilute 18M sulfuric acid to 6M, one would use 2 parts water and 1 part acid, a total of 3 parts.
What is the molarity of carborane superacid?
18 400 000 moles. it is also 1 million times stronger than sulfuric acid
What is the normality of concentrated sulfuric acid?
About 36 N, 36 mole H+/L. (It contains 18 mole/L H2SO4)
How much of an 18 percent solution of sulfuric acid should be added to 360 ml of a 10 percent solution to obtain a 15 percent solution?
600ml.
What is the normality of 96 percent solution of sulphuric acid of specific gravity 1.84?
To find the molarity, we can set up the following factor labeling problem. Note that a specific gravity of 1.84 can be treated as a density of 1.84 g/ml. The molar mass of sulfuric acid (H2SO4) is 98.079 g /molM(mol/l)= (1.84 g/ 1 ml)(1000 ml/1 l)(1 mol/98.079 g)(.96 purity)= 18 mol/l= 18 MThe molarity is 18 mol/l. The pH of this solution would be -1.26...VERY ACIDIC.
Can pH be a negative number?
Yes, if the concentration of hydrogen ions is above 1 M, then pH will be negative. An example is Sulfuric acid, which can get a proton concentration up to 18 M which would be a pH of -1.3.
How much pure acid is in 330 mL of a 18 percent acid solution?
18% of 330 = 59.4 So there are 59.3ml of pure acid in 330ml of 18% acid solution.
How do you prepare 1M sulfuric acid from concentrated sulfuric acid?
To prepare 1M sulphuric acid from concentrated sulphuric acid:First consider the molecular weight of H2SO4 = 98 g/mol, so you have to add 98g of conc. acid and make up to 1 liter of water (as pointed out at the 4thpoint).Considering that acid is a liquid, you should also consider density: where density = mass/volume, which is said on the bottle to be (about) 1.84 g/mL,so then you have: volume = 98g / 1.84(g/mL) = 53.2 mLNow you have to consider the acid purity, usually 98% then you have to do this: 53.2 mL if the acid were 100% pure convert in mL given with the purity of 98%, so 100% x 53.2 mL / 98% = 54.3 mL of (98%) concentrated acid.Finally CAREFULLY add this 54.3 mL (or 98 g, cf. first point) to about 0.9 L dist. water while continuously stirring (evolving heat!), and after that fill it up to 1.00 L with also dist. water. Never reverse this: DO NOT add water to concentrated fluids!
What mass of water is formed when 50 g of sulfuric acid reacts?
a/c to balanced equation .... 1 mole H2SO4 produces 2 mole H2O98 g H2SO4 produces 2 x 18 g H2O50 g H2SO4 produces 2 x 18 x 50 / 98 g H2O50 g H2SO4 produces 18.37 g H2O
How prepare 1N sulphuric accid?
It depends on what yo start with. If you start with concentrated sulfuric acid, it is usually about 18 M or 36 N. So, you would dilute it approximately 1:36 or 1 ml diluted up to 36 mls or any multiple of that. To get the exact dilution, you need to know the exact molarity. If you have some other molarity acid, then the calculations would vary accordingly.
When did Trent Acid die?
Trent Acid died on June 18, 2010 at the age of 29.
