For this pr H2 SO4(aq) + 2 N2OH(aq) → Na2 SO4(aq) + 2H20(1) A titration is performed on a sample containing sulfuric acid (H2SO4) to assess its concentration. 3.73 mL of this sample are used to perform the titration. If 13.5 mL of a 1.00 M NAOH solution are required to reach the endpoint of the titration (neutralize all of the sulfuric acid), what was the molarity of sulfuric acid in that sample?

A chemist titrates a 25.00 mL sample of 0.1041 M benzoic acid (C6H5COOH) against a 0.1000 M solution of NaOH.The overall reaction is shown by the equation below: C6​H5​COOH(aq)+NaOH(aq)C6​H5​COONa(aq)+H2​O(l) What volume of NaOH solution (in mL) is required to reach the equivalence point?  Which of the following quantities will be needed to calculate the pH at the equivalence point of the reaction?Choose one or more: total solution volume Kb for C6H5COO–[C6H5COOH]equivalencemoles C6H5COOHmoles C6H5COO– Using your answers to Parts 1 through 3, calculate the pH at the equivalence point of the reaction. Ka for C6H5COOH is equal to 6.28 × 10–5 and Kb for C6H5COO– is equal to 1.59 × 10–10. Give your answer to two places after the decimal.

A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown concentration. The student monitors the pH during the titration. The following titration curve was created using the experimental data. Write the balanced net ionic equation for the reaction that occurs when HC2H3O2(aq) and NaOH(aq) are combined.  2.Calculate the molar concentration of the NaOH(aq) solution. 3.Explain how the student can estimate the value of Ka for HC2H3O2(aq) using the titration curve.

By titration, it is found that 51.5 mL51.5 mL of 0.143 M NaOH(aq)0.143 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq).HCl(aq). Calculate the concentration of the HClHCl solution. [HCl]=[HCl]=   M

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250 mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.

The standardized NaOH was used to determine the unknown concentration of H3PO4. The standard NaOH concentrtion is 0.126M. The standard sulfuric acid concentration is 0.150M. 3 NaOH(aq) + H3PO4(aq) → Na3PO4(aq) + 3 H2O(l) Three flasks containing 25.00 mL H3PO4 each was titrated with NaOH. The data is below:                                    Titration 1       Titration 2.           Titration 3 Starting volume buret 2.62 mL           18.60 mL            1.20mL Buret volume at end 18.46 mL            34.40mL             16.84mL Calculate the concentration of H3PO4.

A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.

A CHM 125 student performed the "Redox Titration" procedure as given in the laboratory manual. In this experiment, the titrant solution of potassium permanganate (KMNO4) was used to determine the percentage of sodium oxalate (NazC2O4) in an unknown sample. The net ionic equation for the titration carried out was: 2MnO4 (aq) + 5C20,7(aq) + 16H*(aq) → 2MN²*(aq) + 10CO2(g) + 8H2O(£) The data provided in the table below was acquired. Complete the table and determine the percent of sodium oxalate in the unknown sample based on this one titration. Molarity of KMNO, Titrant Solution: 0.0203 M Trial 1 Weight of Oxalate 0.954 g Unknown Starting Buret Reading: 0.65 mL Ending Buret Reading: 34.85 mL of permanganate sl order to use 35.00 mL of Titrant Used: mmol of MnO4 mmol of 2- Weight of NazC204 in Unknown: Percent of Na,C204 in Unknown: You wer 4-

You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.8067 M NaOH and the equivalence point is reached by the addition of 17.31 mL of NaOH solution.  Using the balanced equation below, calculate the molartity of H2SO4 in the flask. Do NOT include units.  2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)

A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample?   H3PO4  +  2 NaOH --> Na2HPO4 + 2H2O   ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS