Chem 111 1st Ediiton Lecture 9Outline of Last Lecture I. Redox ReactionsOutline of Current Lecture Current LectureHow to describe concentrations in solution?% (ex 30%H2O)Ppm (1 part per million)Molarity (this one we will use most)Molarity#of moles of solute/liter of solutionEx 4 moles of HCl dissolved into 2 L of solution: 4moles/2L=2M6 moles of Na2SO4 are dissolved in 2 L of solution. What is the concentration of SO4 ^2-?3MWhat is the concentration of Na+?6MPreparing a solution-direct methodTo make 2.0L of 1.5 M Na2SO4, how much Na2SO4 (in grams) do you add to 2L of water?1. Calculate # of moles needed to make it 1.5 M2.0Lx(1.5M/liter)=3.0 moles of Na2SO42. Convert to grams3.0molesx 142.0 g/mole=430gPreparing a solution-Dilution methodStart with a stock of .1 M Na2SO4 (100mM). What volume of this stock solution must be diluted to a final volume of .5 L to prepare a 1.5mM Na2SO4 solution?1. How many moles do we need?.5L x (1.5E-3mole Na2SO4/liter)=7.5E-4 moles Na2SO42. What volume of stock solution contains that many moles?7.5E-4 mol x(1 Liter/.1moles)=7.5E-3L=7.5mLSlightly faster wayC1V1=C2V2(moles/liter)xliters=moles100mM x V1= 1.5 mM x .5 LV1= .0075L=7.5mLYou mix 1L each of 2 M HCl(aq) and NaOH(aq). What are the final solution concentrations of Na+ and Cl-?Initial moles of Na+(aq) before mixing=2moles/L x 1L=2 molesThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.But all the Na+ (aq) are still there in the final total volume of 2LNa+ final= (2 moles Na+ (aq))/2L=1M60 mL .2 M KOH is needed to titrate 40 mL of H2SO4. What is H2SO4?1. Write a balanced equation2. Calculate # of moles of OH-3. Calculate # of moles of H2SO44. Calculate concentration of