NH2 HSPh 1. Ph₂CuLi 2. H₂O

5. Calculate the concentration of the hydrochloric acid if a 20.00 mL sample is titrated with standard sodium carbonate solution. 2 HCI (aq) + Na₂CO3(aq) → H₂O (1) + CO₂(g) + 2 NaCl (aq) The titration required 10.00 mL of 0.250 mol/L sodium carbonate to neutralize the acid. rn Lakes College

it is time for the titration.  You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask.  Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask.  You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint.  At the endpoint, the solution in the flask turns light pink.  You repeat the titration two additional times for a total of three trials.  H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l)                                                (I)              (II)                (III) Volume of H2C2O4 used  15.00 mL   15.00 mL   15.00 mL Initial Buret Reading        0.00 mL    0.05 mL         0.10 mL Final Buret Reading           14.45 mL     14.38 mL    15.40 mL Volume NaOH used           ________mL          ________mL        ______mL Moles NaOH                     _______M      ________M    _________M…

A railroad tank car carrying 1.5  103 L of concentrated sulfuric acid derails and spills its load. The acid is 93.2% H2SO4 by mass and has a density of 1.84 g/mL. How many kilograms of sodium carbonate (soda ash) are needed to neutralize the acid? (Hint: What is the neutralization reaction?)