Astock solution is made by dissolving 66.05 g of (nh4)2so4 in enough water to make 250 ml of solution. a 10.0 ml sample of this solution is then diluted to 50.0 ml. given that the molar mass of (nh4)2so4 is 132.1 g/mol, what is the concentration of the new solution? use mc022-1.jpg and mc022-2.jpg. 0.400 m 1.60 m 5.00 m 10.0 m

first the stock solution is prepared

we need to calculate the molar concentration of (NH₄)₂SO₄

mass of (NH₄)₂SO₄ added - 66.05 g

number of moles of (NH₄)₂SO₄ - 66.05 g / 132.1 g/mol = 0.5 mol

volume of the solution - 250 mL

molarity of solution is - number of moles / volume of solution

molarity of (NH₄)₂SO₄ - 0.5 mol / 0.250 L = 2 mol/L

10.0 mL of the stock solution is taken and diluted upto 50.0 mL

the dilution formula is used

c1v1 = c2v2

where c1 - concentration and v1 - volume of stock solution

c2 - concentration and v2 is volume of the diluted solution

substituting the values

2 mol/L x 10.0 mL = C x 50.0 mL

C = 0.4 mol/L

concentration of new solution is 0.4 M

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year