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?

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

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the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.