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Sulphuric Acid requires, I believe 27.2ml to make a 1N solution.
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∙ 16y ago
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How do you prepare 2N H2SO4 and 2M H2SO4?
MW of H2SO4 is 98.08. 2M = 2 x 98.08 in 1 L of water (1 gram=1 ml). Take 500 ml water in a 1 L measuring cylinder. Add 196.16 ml slowly along the side into water in the measuring cylinder. Use 50 ml pipette with automated pipettor. If needed you may want to keep the cylinder in ice to take care of the heat generated. Then make up to volume to 1 L with water. Eq. wt for H2SO4 = 98.08/2 = 49.039. SO for 2N solution, 2 eq.wt in 1 L. 98.08 ml in 1 L water adopting the method cited above.
How do you prepare the 1.25 percent H2SO4 solution?
Concentrated H2SO4 is 96 %.( In laboratory ) As density of concentrated H2SO4 is 1.84gm/ml we will need this number as well, and as the atomic mass of H2SO4 is 98.08,as it is dibasic for normality it is 49 hence, Calculation=((96/100)(1000)(1.84))/49=36.04 If H2SO4 concentrated is 36.04 M then for make a 1L solution of 1M H2SO4 (36.04)X (x) = 1X(1) x = 1 X(1) / (36.04) x=0.0277gm/ml of water x = 27.7 mL of 36M H2SO4 per liter Hence for 1N H2SO4 dissolve 27.7ml of it to 1000ml of solvent(Water) that means for 0.1 N H2SO4 2.77 ml of it to 1000mL of solvent.
How do you prepare 60 percent sulphuric acid solution?
0.2g Na2CO3 dissolved into 25ml DI Water. Methyl Orange is used 2 to 3 drops is a indicator. then we take normal solution of 0.02N H2SO4 in beurate . note the volume consumed of H2SO4. put these value in formula formula N H2SO4= wt of Na2CO3 * volume of Na2CO3 used/ 53 * volume of H2SO4 consumed repeat this process
How do you make 0.02N sulfuric acid solution?
I would like to dilute some 5N sulfuric acid with water, and make 0.1N sulfuric acid solution. I want 1000ml of 0.1N . I think it's a 50 to 1 ration, but just want to make sure. <Volume of concentrated> x <Concentration of Concentrated> = <Volume of dilute> x <Concentration of dilute> Therefore, <Volume of concentrated> = <Volume of dilute> x <Concentration of dilute> / <Concentration of dilute> = 1000 mL x 0.1 N / 5N = 20 mL. Meaning: Dilute 20 mL of the 5N H2SO4 to 1000 mL in a volumetetric flask will give you 1000 mLs of 0.1 N H2SO4 (aq.).
How many milliliters of 0.200M H2SO4 will neutralize 40.0 mL of 1.50M KOH?
Let's solve this problem without using specific numbers as that's more instructive (and won't give away an answer to someone's homework problem).The question is:What volume Vacid of strong diprotic acid solution of molarity Macid is needed to neutralize a volume Vbase strong base solution of molarity Mbase?So, Macid, Vbase, and Mbase are known and we are asked to find Vacid.A strong base of the form BOH will completely dissociate in solution into B+ and OH- ions, so Mbase is the same as MOH- in this problem.A strong diprotic acid of the form AH2 will lose both of its protons in the presence of OH- ions to form A2+ and two H+ ions, so Macid is half of MH+ in this problem.Neutralization is the process of mixing an acidic solution with a basic solution in proportion such that the number of OH- ions in the basic solution is equal to the number of H+ ions in the acidic solution. To get the number, you must multiply the ions' molarity times there volumes.So, we need:MH+·Vacid = MOH-·Vbaseor2·Macid·Vacid = Mbase·Vbase (since Macid is half of MH+ and Mbase equals MOH-)solve for Vacid to obtainVacid = (Mbase·Vbase)/(2·Macid)
How do you prepare 2N H2SO4 and 2M H2SO4?
MW of H2SO4 is 98.08. 2M = 2 x 98.08 in 1 L of water (1 gram=1 ml). Take 500 ml water in a 1 L measuring cylinder. Add 196.16 ml slowly along the side into water in the measuring cylinder. Use 50 ml pipette with automated pipettor. If needed you may want to keep the cylinder in ice to take care of the heat generated. Then make up to volume to 1 L with water. Eq. wt for H2SO4 = 98.08/2 = 49.039. SO for 2N solution, 2 eq.wt in 1 L. 98.08 ml in 1 L water adopting the method cited above.
Is ionization endothermic or exothermic?
It is exothermic. Take for example H2SO4 H2SO4 -> H+ + HSO4- This is very exothermic
How do you prepare the 1.25 percent H2SO4 solution?
Concentrated H2SO4 is 96 %.( In laboratory ) As density of concentrated H2SO4 is 1.84gm/ml we will need this number as well, and as the atomic mass of H2SO4 is 98.08,as it is dibasic for normality it is 49 hence, Calculation=((96/100)(1000)(1.84))/49=36.04 If H2SO4 concentrated is 36.04 M then for make a 1L solution of 1M H2SO4 (36.04)X (x) = 1X(1) x = 1 X(1) / (36.04) x=0.0277gm/ml of water x = 27.7 mL of 36M H2SO4 per liter Hence for 1N H2SO4 dissolve 27.7ml of it to 1000ml of solvent(Water) that means for 0.1 N H2SO4 2.77 ml of it to 1000mL of solvent.
How do you prepare 60 percent sulphuric acid solution?
0.2g Na2CO3 dissolved into 25ml DI Water. Methyl Orange is used 2 to 3 drops is a indicator. then we take normal solution of 0.02N H2SO4 in beurate . note the volume consumed of H2SO4. put these value in formula formula N H2SO4= wt of Na2CO3 * volume of Na2CO3 used/ 53 * volume of H2SO4 consumed repeat this process
How do you make 0.02N sulfuric acid solution?
I would like to dilute some 5N sulfuric acid with water, and make 0.1N sulfuric acid solution. I want 1000ml of 0.1N . I think it's a 50 to 1 ration, but just want to make sure. <Volume of concentrated> x <Concentration of Concentrated> = <Volume of dilute> x <Concentration of dilute> Therefore, <Volume of concentrated> = <Volume of dilute> x <Concentration of dilute> / <Concentration of dilute> = 1000 mL x 0.1 N / 5N = 20 mL. Meaning: Dilute 20 mL of the 5N H2SO4 to 1000 mL in a volumetetric flask will give you 1000 mLs of 0.1 N H2SO4 (aq.).
How many milliliters of 0.200M H2SO4 will neutralize 40.0 mL of 1.50M KOH?
Let's solve this problem without using specific numbers as that's more instructive (and won't give away an answer to someone's homework problem).The question is:What volume Vacid of strong diprotic acid solution of molarity Macid is needed to neutralize a volume Vbase strong base solution of molarity Mbase?So, Macid, Vbase, and Mbase are known and we are asked to find Vacid.A strong base of the form BOH will completely dissociate in solution into B+ and OH- ions, so Mbase is the same as MOH- in this problem.A strong diprotic acid of the form AH2 will lose both of its protons in the presence of OH- ions to form A2+ and two H+ ions, so Macid is half of MH+ in this problem.Neutralization is the process of mixing an acidic solution with a basic solution in proportion such that the number of OH- ions in the basic solution is equal to the number of H+ ions in the acidic solution. To get the number, you must multiply the ions' molarity times there volumes.So, we need:MH+·Vacid = MOH-·Vbaseor2·Macid·Vacid = Mbase·Vbase (since Macid is half of MH+ and Mbase equals MOH-)solve for Vacid to obtainVacid = (Mbase·Vbase)/(2·Macid)
How much 100x TAE buffer will it take to make 500ml of 1x TAE solution?
to make 500ml of 1x TAE solution we have to take 5ml of 100x TAE solution. mix it in 495 ml of deionized water.
How much 1 M NaHCO3 solution does it take to fully react with 5 ml of a 1 M solution of HCl?
The answer is 5 m L sodium bicarbonate, 1 M solution.
How do you dilute and concentrate a solution?
To dilute a solution, add water to it. To concentrate a solution, take water out of it.
Why use sulphuric acid in redox titration?
H2SO4 is a strong acid and will deliver H(+) which will help to proceed the reaction much faster. Thereby, the sulphate-ions barely react in a redoxreaction. If we would take HCl for example, the Cl(-) ions can easily take part in a redoxreaction as a reductor.
Does it take longer to saturate a heated solution than a cold solution?
No, a heated solution will saturate faster.
Why is it important for an IV solution to have salts in it and what would happen if you were given pure water in an IV?
The solution must have the same percentage of water as healthy cells have, or the cells will take in too much water and be damaged/killed.
