Titration of a 11.0 mLmL solution of HClHCl requires 32.4 mLmL of 0.11 MM NaOHNaOH. What is the molarity of the HClHCl solution? Express your answer using two significant figures.

For their first trial, a student pipettes 5.00 mL of a vinegar solution into an Erlenmeyer flask. The student titrates the vinegar with standardized NaOH with a molarity of 0.437 M. The volume of titrant used was recorded in the table above. Calculate the molarity of the vinegar solution for this trial. Enter a number without units.

A chemistry student weighs out 0.212 g of lactic acid (HC,H,03) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1000 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. mL ola Ox10 Ar ?

A titration is a procedure for determining the concentration of a solution by allowing it to react with another solution of known concentration (called a standard solution). Acid-base reactions and oxidation- reduction reactions are used in titrations. For example, to find the concentration of an HCl solution (an acid), a standard solution of NaOH (a base) is added to a measured volume of HCI from a calibrated tube called a buret. An indicator is also present and it will change color when all the acid has reacted. Using the concentration of the standard solution and the volume dispensed, we can calculate molarity of the HCl solution. A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H₂SO4). What was the molarity of the KOH solution if 13.2 mL of 1.50 M H₂SO4 was needed? The equation is 2KOH(aq) + H₂SO4 (aq)→K₂SO4 (aq) + 2H₂O(1) Express your answer with the appropriate units. ► View Available Hint(s) molarity = Submit…

An analytical chemist weighs out 0.138 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 0.0600M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 25.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. 0 mol X S 629 OL A

What volume, in mL, of 0.1126 M sodium hydroxide (NaOH) is required to titrate 15.00 mL of 0.1012 M acetic acid (HC₂H₂O₂)? Be sure your answer has the correct number of significant digits. mL X

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.   A.) 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!)   B.) 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.   C.) 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.

A 28.00 mL sample of an unknown HClO4 solution requires titration with 20.42 mL of 0.2100 MNaOH to reach the equivalence point. What is the concentration of the unknown HClO4  solution? The neutralization reaction is HClO4(aq)+NaOH(aq)→H2O(l)+NaClO4(aq) Express your answer using four significant figures.

An analytical chemist weighs out 0.087 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 5.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.

You perform a titration between Sodium hydroxide (NaOH) and Carbonic Acid (H₂CO3). The NaOH is in the burette and the H₂CO3 is in the Erlenmeyer Flask. 42.5 mL of 0.50 M NaOH was added to 25.6 mL of H₂CO3, what is the concentration of the H₂CO3? Give your answer to 2 decimal places..