A stock 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 M subscript i V subscript i equals M subscript f V subscript f. And Molarity equals StartFraction moles of solute over liters of solution EndFraction. 0. 400 M 1. 60 M 5. 00 M 10. 0 M.

Calculate the ratio of h+ ions to oh– ions at a ph = 7. find the concentration of h+ ions to oh– ions listed in table b of your student guide. then divide the h+ concentration by the oh– concentration. record this calculated ratio in table a of your student guide. compare your approximated and calculated ratios of h+ ions to oh– ions at a ph = 7. are they the same? why or why not? record your comparison in table a. what is the concentration of h+ ions at a ph = 7? mol/l what is the concentration of oh– ions at a ph = 7? mol/l what is the ratio of h+ ions to oh– ions at a ph = 7? : 1