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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.
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How many moles of sulfur are present in 5 moles of H2So4?
There are 5 moles of sulfur in 5 moles of H2SO4, as there is 1 mole of sulfur in each mole of H2SO4.
How do you prepared 0.02 n from 0.1 n h2so4?
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.
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.
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.
What is the normality of a 6.35 M H2SO4 is?
0.08 n
What is 5 percent of 71000?
N x 5% = N/20.71000/20 = 3550.
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.
How many moles of sulfur are present in 5 moles of H2So4?
There are 5 moles of sulfur in 5 moles of H2SO4, as there is 1 mole of sulfur in each mole of H2SO4.
How do you prepared 0.02 n from 0.1 n h2so4?
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.
What number is 5 percent of 75?
75 = 0.05 * n 75/0.05 = n n = 1500
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.
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.
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.
If 15 percent of a number n is 0.3 what is 45 percent of N?
If 15 percent of a number N is 0.3 what is 45 percent of N
How many equivalent of H2SO4 are contained in 200ml of a 0.2 N solution?
a lot
How do you calculate 20 percent of 100?
20%= .2, n*.2= n/5, 100*.2=100/5, 100/5=20 20% of 100 is 20
