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To prepare 0.02N H2SO4 from 0.1N H2SO4, you can dilute the 0.1N H2SO4 by adding a calculated amount of water. To calculate the dilution factor, you can use the formula: C1V1 = C2V2, where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration (0.02N), and you can solve for V2 to find the volume of the 0.1N H2SO4 to be diluted with water to get 0.02N H2SO4.
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What is the molarity of a 0.050 N H2SO4 solution?
The molarity of a 0.050 N (normal) H2SO4 solution is 0.025 M (molar) since H2SO4 has a molar mass of 98.08 g/mol and dissociates into 2 H+ ions per molecule of H2SO4.
5 N H2SO4 What is percent?
To calculate the percent of a 5 N H2SO4 solution, you need to know the molarity (moles of solute per liter of solution) and the molecular weight of the solute. Once you have that information, you can use the formula: % = (molarity x equivalent weight) / 10. If you provide the molecular weight of H2SO4, I can help you calculate the percent.
What is the normality of a 6.35 M H2SO4 is?
0.08 n
What is the normality of a 1.25 M solution of H2SO4?
Sulfuric acid H2SO4 will give away 2 protons H+ for this reason its normality is 2 times its molarity. so for H2SO4 M = 2N For HCl M= 1N because HCl has only one proton H+ H3PO4 for example has 3N = M so for your case, 6M = 2N and N= 6/2 = 3.
Specific gravity equals 1.84 gram per milliliters and assay equals 97 percent How many milliliters of concentrated H2SO4 are required to prepare 10 L of 0.1 N H2SO4?
To prepare 10 L of 0.1 N H2SO4, you would need 0.1 moles/L x 10 L = 1 mole of H2SO4. Since the specific gravity is 1.84 g/mL, 1 litre of H2SO4 weighs 1.84 kg. This means 10 L would weigh 1.84 kg/L x 10 L = 18.4 kg. With an assay of 97%, the mass of pure H2SO4 is 0.97 x 18.4 kg = 17.848 kg. So, the volume of concentrated H2SO4 needed is 17.848 kg / (1.84 g/mL) = 9687 mL, or about 9.7 L.
How many moles Mg react with 0.20 moles H2SO4?
If you want all the H2SO4 to react, you first need a balenced chemical equasion. Mg + H2SO4 --> MgSO4 +H2 Then you calculate using mole ratios moles is expressed as n. n Mg/1 =n H2SO4/1 n Mg= 0.2mol It's the same because there are no coefficients in front of the reactants.
What is the molarity of a 0.050 N H2SO4 solution?
The molarity of a 0.050 N (normal) H2SO4 solution is 0.025 M (molar) since H2SO4 has a molar mass of 98.08 g/mol and dissociates into 2 H+ ions per molecule of H2SO4.
5 N H2SO4 What is percent?
To calculate the percent of a 5 N H2SO4 solution, you need to know the molarity (moles of solute per liter of solution) and the molecular weight of the solute. Once you have that information, you can use the formula: % = (molarity x equivalent weight) / 10. If you provide the molecular weight of H2SO4, I can help you calculate the percent.
What is the normality of a 6.35 M H2SO4 is?
0.08 n
What is the N in 2N h2so4?
N stands for molality and it indicates the number of moles of a substance in a unit mass of the solution.
When was N. Ravi born?
N. Ravi was born on 1948-01-01.
How many equivalent of H2SO4 are contained in 200ml of a 0.2 N solution?
a lot
What is the normality of a 1.25 M solution of H2SO4?
Sulfuric acid H2SO4 will give away 2 protons H+ for this reason its normality is 2 times its molarity. so for H2SO4 M = 2N For HCl M= 1N because HCl has only one proton H+ H3PO4 for example has 3N = M so for your case, 6M = 2N and N= 6/2 = 3.
When was Charles N. Felton born?
Charles N. Felton was born on 1832-01-01.
When was Shaji N. Karun born?
Shaji N. Karun was born on 1952-01-01.
Specific gravity equals 1.84 gram per milliliters and assay equals 97 percent How many milliliters of concentrated H2SO4 are required to prepare 10 L of 0.1 N H2SO4?
To prepare 10 L of 0.1 N H2SO4, you would need 0.1 moles/L x 10 L = 1 mole of H2SO4. Since the specific gravity is 1.84 g/mL, 1 litre of H2SO4 weighs 1.84 kg. This means 10 L would weigh 1.84 kg/L x 10 L = 18.4 kg. With an assay of 97%, the mass of pure H2SO4 is 0.97 x 18.4 kg = 17.848 kg. So, the volume of concentrated H2SO4 needed is 17.848 kg / (1.84 g/mL) = 9687 mL, or about 9.7 L.
How do make a 5.25N sulfuric acid solution from concentrated sulfuric acid solution?
To make a 5.25N sulfuric acid solution from concentrated sulfuric acid (98%), you would need to dilute the concentrated sulfuric acid with water in the correct proportions. Calculate the volume of concentrated sulfuric acid needed using the formula C1V1 = C2V2, where C1 is the concentration of the concentrated acid (98%), V1 is the volume of concentrated acid needed, C2 is the desired concentration (5.25N), and V2 is the final volume of the solution. Add the calculated volume of concentrated acid to a container and carefully add water to reach the final volume while stirring to mix thoroughly. Remember to always add acid to water and not the other way around for safety.
