You titrate a 20.00-mL solution of sulfiric acid, H2SO4, with your standardized sodium hydroxide solution (0.2011 M). The titration required 44.23 mL of your sodium hydroxide to reach the endpoint. What is the concentration (molarity) of the sulfuric acid? Include the balanced chemical equation for the titration reaction in your answer.

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Deanna HettingerLv2

20 Feb 2019

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In an acid base titration a 25mL portion of a solutioncontaining sulfuric acid (H2SO4) was titrated with a 0.200MNaOH(aq).

a. write the chemical equation for this particular titration

b. if titration required the addition of 4.32 mL of NaOH titrantto reach the end point what is the concentration in Molarity ofsulfiric acid in the sample solution?

c. pH at end point?

fuchsiacricket302

You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1920 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 mL. You then take a 10.00 mL sample of the dilute acid solution and titrate it with the standard solution. You need 19.18 mL of the standard solution to reach the endpoint. What is the concentration of the original acid solution?