A student begins a titration experiment by filling her first buret with unknown acid to the 1.12 mL level.  She fills her second buret with base, NaOH, and records an initial volume of 0.08 mL.  At the end of the titration experiment and after the pale pink endpoint is obtained, she records her final volume of acid in the buret as 18.85 mL, and the final volume of base in the second buret as 28.74 mL.  In the first blank below, please indicate the volume of acid used in her experiment.  In the second blank, please indicate the volume of base used.  For both answers, please report your answer WITH the correct number of significant figures or decimal places, and WITHOUT a unit.    Question 1 options: ___________ answer #1   ___________answer #2

A 25.0 mL sample of phosphoric acid requires 22.5 mL of 1.1 M sodium hydroxide for complete neutralization. What is the molarity of the phosphoric acid? The neutralization reaction : H3PO4 + 3NaOH ----> Na3PO4 + 3H2O Write your numerical answer without unit inside the box. The answer should be in Two Significant figures and in standard, not scientific notation.

In a lab, you diluted a sample of bleach to 1/10 concentration in a 250 volumetric flask. Then quantitatively transferred 25 ml of the 1/10 concentration diluted bleach into a beaker and titrated it with a standard sodium thiosulfate solution that has a molarity of 0.1215M. You repeated this 3 times. The data below is the amount of sodium thiosulfate that was titrated in the 3 runs. Calculate the molarity in each run of the diluted bleach and the concentration of undiluted bleach sample. Titration 1: 45.55 ml Titration 2: 45.67 ml Titration 6: 45.58 ml

An analytical chemist weighs out 0.159 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 25.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol

Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.

An analytical chemist weighs out 0.061 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1900 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 3.3 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits. g 0 x10 mol C X Ś 2.

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You perform a titration between Sodium Hydroxide (NaOH) and Hydrochloric Acid (HCI). NaOH is in the burette and the HCI is in the Erlenmeyer Flask. 34.3 mL of 0.5 M NaOH was added to 37mL of HCI, what is the concentration of the HCI? Give your answer to 2 decimal places.