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Suppose you wanted to produce 1.00 L of 3.50 M solution of H2SO4. How
many grams of the solute are needed to make this solution?

Respuesta :

hekmatawalkhil

Answer:

343g H2SO4

Explanation

1. H2SO4 is the solute

2. Water is the solvent

3. Molarity = moles of solute / liter of solution = n / V

(Note the case of the letters is important in science. N stands for Normal in chemistry a type of concentration, n stands for the number of moles)

Rearrange the formula to find n

n = M x V

Here are the known values,

M = 3.5M

n = x mol

V = 1.00L

Plug it in and solve for n (the number of moles of H2SO4 in the solution)

n = 3.5M x 1.00 L = 3.50 mol of H2SO4

Molecular mass of H2SO4 is 1g/mole H x 2 + 32.1g/mol S + 16g/mol O x 4 = 98.1g/mol H2SO4

mass = number of mole x relative molecular mass

mass = n x 98.1g/mol

mass = 98.1g/mol H2SO4 x 3.50mol H2SO4

= 343g H2SO4 <-answer

samueladesida43

The mass of H2SO4 needed to make a 3.50M solution that has a volume of 1.00L is 343grams.

How to calculate mass?

The mass of a substance can be calculated by multiplying the number of moles of the substance by its molar mass.

However, the number of moles of the substance must first be calculated as follows:

Molarity = no of moles/volume

3.5M = n/1L

n = 3.5moles

molar mass of H2SO4 = 98g/mol

mass of H2SO4 = 98 × 3.5

mass of H2SO4 = 343g

Therefore, the mass of H2SO4 needed to make a 3.50M solution that has a volume of 1.00L is 343grams.

Learn more about mass at: https://brainly.com/question/19694949

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