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What is the molarity of 70 grams of sulfuric acid in 280 mL solution.?
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What is molarity of 2m acetic acid?
(.05)X(grams of total solution) = grams of acetic acid (grams of acetic acid)/ (mol. wt. of acetic acid(=60g/mol)) = mol. acetic acid (mol. acetic acid)/ (Liters of total solution) = molarity(M)
A volume of 40.0g of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid. What was the molarity of the solution if 25.7g of 1.50M was needed?
M = n ÷ V M-Molarity (mol/l) n- moles V- volume in liters. Volume cannot be expressed in grams....
What is the molarity of a solution formed by mixing 20.0 g sulfuric acid with enough water to make 500.0 mL of solution?
0.408 M
What is normality of sulfuric acid when molarity is 4m?
8N
How many moles of sulfuric acid are present in 0.550 L of a 0.150 M sulfuric acid solution?
.150 M is the molarity of the solution, which is the number of moles per liter. So all you need to do is multiply the molarity by the number of liters. So .150 moles/liter x .550 L = .0825 moles
How many grams of sulfuric acid H2SO4 are in 45.0 ml of a 6.5 M solution?
This solution contain 2,89 g sulfuric acid.
What is molarity of 2m acetic acid?
(.05)X(grams of total solution) = grams of acetic acid (grams of acetic acid)/ (mol. wt. of acetic acid(=60g/mol)) = mol. acetic acid (mol. acetic acid)/ (Liters of total solution) = molarity(M)
What is the molarity of a solution formed by mixing 20.0 g sulfuric acid with enough water to make 500.0 mL of solution?
0.408 M
A volume of 40.0g of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid. What was the molarity of the solution if 25.7g of 1.50M was needed?
M = n ÷ V M-Molarity (mol/l) n- moles V- volume in liters. Volume cannot be expressed in grams....
What is normality of sulfuric acid when molarity is 4m?
8N
How many moles of sulfuric acid are present in 0.550 L of a 0.150 M sulfuric acid solution?
.150 M is the molarity of the solution, which is the number of moles per liter. So all you need to do is multiply the molarity by the number of liters. So .150 moles/liter x .550 L = .0825 moles
How many moles of sulfuric acid are in 500 mL of 0.324 M sulfuric acid solution?
Molarity = moles of solute/volume of solution 0.324 M H2SO4 = moles H2SO4/500 ml 162 millimoles, or, more precisely to the question 0.162 moles H2SO4
What is the ph number for sulphric acid?
The pH value of any acidic solution depends on the strength of the acid in the particular solution. In this instance, a dilute sulfuric acid solution shows a higher value of pH whereas the concentrated acid shows a very low value.
The formula for sulfuric acid is H2SO4 A mole of sulfuric acid would have a mass of grams?
It would be 98 grams.
How many grams of sulfuric acid in 0.400 L of battery acid if the solution has a density of 1.28 g per ml and is 39.1 percent sulfuric acid by mass?
512 GRAMS Divide the quantity by the SG: EG1000 litres divide by 1.28 = 781.25 litres per tonne. dumb*** has to use percent sulfuric acid .4*.391=.1564 *1000=156ml of sulfuric acid 156*1.28=200.2 grams H2SO4 in .4L and is 5.1M
Is sulfuric acid a heterogeneous mixture?
No, a sulfuric acid solution in water is homogeneous
Is sulfuric acid an element a compound a solution or a heterogeneous?
Sulfuric acid is a compound.
