In one trial determination of the concentration of NaOCl in the diluted bleach sample, 10.00 mL of the diluted bleach solution required 23.32 mL of 0.0195 M Na2S2O3 titrant to reach the endpoint. What is the molar concentration of NaOCl in the diluted bleach solution?

The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?

An impure sample of the monoprotic acid benzoic acid (C6H5COOH, 122.12 g/mol) is titrated with 0.9855 M NaOH. A 3.412-g sample requires 24.43 mL of the NaOH solution to reach the endpoint. Calculate the percent by mass of benzoic acid in the sample.  thank you!

A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted to lead(II).  This reaction is facilitated by the presence of sulfuric acid, H2SO4 , as shown by the reaction Pb+PbO2+2H2SO4→2PbSO4+2H2O Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4.  What will be the concentration of H2SO4 in the battery after 3.40 A of current is drawn from the battery for 5.00 hours?

A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Given that 0.00966 mol of HNO₃ are used in the titration, how many moles of Ca(OH)₂ had to be present in the initial reaction?

A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca  C) The percentage of CaO

Ca(OH)2​(aq)+2HCl(aq)CaCl2​(aq)+H2​O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration.   A. How many moles of base were required to react completely with the acid in this reaction?   _____mol Ca(OH)2      B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HCl

Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution.  From the procedure, find:  Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84     average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)

A 27.56 mL portion of a 0.337 M solution of hydrochloric acid, a monoprotic acid, is to be titrated with a standarized 0.411 M solution of KOH. What is the expected volume in milliliters of the KOH solution needed to reach the phenolphthalein end point? Report your answer with a precision of two decimal places.

A 10.00 mL aliquot of vinegar (acetic acid, CH3COOH - 60.08 g/mol) was diluted in a 100.00 mL volumetric flask and made up with distilled water. An aliquot of 10.00 ml was pipetted into an erlenmeyer flask, to which two drops of phenolphthalein were added. This solution was then titrated with 0.1006 mol/L NaOH. i) Considering that the volume of NaOH consumed was 8.28 mL, what is the molar concentration of acid in dilute solution? ii) What is the acidity percentage of vinegar? iii) Whereas the expected concentration of the acetic acid solution was equal to 0.0830 mol/L, calculate the volume of NaOH needed to reach the point of equivalence. iv) Based on the volume calculated in the previous item and the volume indicated in item (i), calculate the titration error.