Question

5. Two burettes are set up. The first contains 0.15M NaOH and the second contains an HCI solution of unknown concentration. HCl is dispensed into the reaction flask and Phenolphthalein is added as an indicator. At the end of the titration, 22.2ml of NaOH and 9.45ml HCl were used. A. Write a balanced equation for the Acid-Base reaction. B. What is the total volume of NaOH used in the titration? Chem301_exam2_hmwk02_Sp20 due 4/2/20 C. How many moles of NaOH was used?

Answer 1

Date Page concentration of NaoH = 0.15M volume of Naoy used = 22.2ml Volume of He used = 9.45 ml NaOH + HCO Nach & H₂O Volume of NaoH used = 22.2ml es cof NaOH used : BM Concentration suggest that o. 15 mole of is present in 1000 ml. NaOH. 1600 ml 22.2 ml contain = contain = 0.15 mole. 0.15 x 22.2 1000 mole = 0.0033 moles consumed volume He used = 9.45 ml . 6 concentration of the solution VMI = V2 M2 (Naom) (Hill ) 2202 me x 0.15M = 9.45 ml X M2 M2 = 22.2 ml xo.15m 9. 45 mil M₂ = 0.35M