If the initial volume reading for the first titration was 0.32 mL and the final volume reading was 8.64 mL, what volume of iodine solution was used in your first titration (in mL)?

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…

By titration it is found that 35.7 mL of 0.101 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.

If your first titration yielded a concentration of 0.4 mg/mL and your second titration yielded a concentration of 0.54 mg/mL, what was the average concentration for your two titrations (in mg/mL)? Include the unit and two decimal places in your answer.

CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) 25.00 mL of a solution of phosphoric acid, H3PO4, was titrated with 0.500 M NaOH. a) Write the balanced chemical equation for this reaction.b) If 35.92 mL of NaOH solution were needed to reach the end point in the titration, what is the molarity of the H3PO4 solution?c) How many grams of H3PO4 were present?

A strong acid-strong base titration was performed as follows: 10.00 mL of 0.10M HCl were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to HCl. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.)What is the pH of the solution in the Erlenmeyer flask after adding 10.20 ml of 0.100M NaOH?   Question 4 options:

Consider the titration of 25.00 mL of Sprite with 0.050 M NaOH. Using the following data, determine the citric acid concentration in Sprite (g/L). Take the molar mass of citric acid to be 192.124 g/mol. Give your answer to one decimal place. initial volume (mL) final volume (mL) Buret reading (mL) 1.75 14.32

what is the volume of a NaOH solution added during a titration experiment is the initial buret reading was 12.50 mL and the final buret reading was 37.25 mL?

4. A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of the phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain qalb ribidw qid edini olddud ris ogrel s znisimos tund entd nousu 5. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 9no vino to beateni nolusius to alsid sigulum ob of insttoqmi ti al VW S

An aqueous solution of barium hydroxide is standardized by titration with a 0.180 M solution of hydrochloric acid.If 28.0 mL of base are required to neutralize 26.4 mL of the acid, what is the molarity of the barium hydroxide solution?