Use this average in your calculations using the

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the 3 determinations. Use this average in your calculations using the sodium hydroxide solution.Part BTo find the molarity of the unknown solution use an autopipet to dispense 20.00mL of the unknown given to you into your 250mL Erlenmeyer flask. Repeat thesteps in Part A with this solution then repeat with a new 20.00mL of the unknown. The volume Vt of NaOH used in the 2 titrations should agree within 0.2mL, otherwise do it a third time. Calculate the molarity of the sulfuric acid solution for each titration as you did in Part A & report average molarity in your results & conclusion.Data & Results (Intermixed)Part A31mL NaOHVolume of the burette readings: 1.) .65mL, 2.) .53mL, 3.) .55mLWeighing Paper: 0.) 0.395g, +sulfuric acid: 1.395g, sulfuric acid: 1gWeighing Paper: 1.) 0.4014g, 2.) 0.4135g, 3.) 0.4017g+sulfuric acid: 1.) 0.6973g, 2.) 0.7809g, 3.) 0.7384gsulfuric acid: 1.) 0.2959g, 2.) 0.3674g, 3.) 0.3367gVolume of titrant after adding to the solution: 1.) 34.35mL, 2.) 39.95mL, 3.) 38.75mLTitrant volume (mL)/sulfuric acid mass (g): 1.) 116.0865, 2.) 108.7371, 3.) 115.0876Moles of sulfuric acid: 1.) .0041mol, 2.) .0080mol, 3.) .0076molMNaOH: 1.) 0.0035318, 2.) 0.007.3572, 3.) 0.0066037Part BUnknown #8: initial volume: .60g, after adding to solution: 31.18mLTitrant volume (mL)/sulfuric acid mass: 51.97Moles of sulfuric acid: 0.0061M: 0.2M sulfuric acidUnknown #24: initial volume: 0.45g, after adding to solution: 26.03mLTitrant volume (mL)/sulfuric acid mass: 57.8444Moles of sulfuric acid: 0.0046ML 0.18M sulfuric acid
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Discussion1.) Use your experimental results to calculate the number of grams of H2SO4in exactly 150 mL of your unknown solution.(4.0667)10-52.) Barium hydroxide is a strong base & can be used to titrate acids. The

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