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Hx (aq) + NaOH --> H2O (l) + Nax(aq) Calculate number of moles of NaOH that was needed to neutralize all of the acid.  Use stoichiometry to determine how many moles of acid must have been present in the titration experiment. Use the mass of the acid and the moles of the acid present in the titration to determine the molar mass. Calculate the molar mass.   Mass unknown = 0.3089g concentration NaOH = 0.3089M intial mL in buret = 1.44 end point mL in buret = 13.72

Hx (aq) + NaOH --> H2O (l) + Nax(aq) Calculate number of moles of NaOH that was needed to neutralize all of the acid.  Use stoichiometry to determine how many moles of acid must have been present in the titration experiment. Use the mass of the acid and the moles of the acid present in the titration to determine the molar mass. Calculate the molar mass.   Mass unknown = 0.3089g concentration NaOH = 0.3089M intial mL in buret = 1.44 end point mL in buret = 13.72

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.104QE: A 10.00-mL sample of a 24.00% solution of ammonium bromide (NH4Br) requires 23.41 mL of 1.200 molar...
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Hx (aq) + NaOH --> H2O (l) + Nax(aq)

Calculate number of moles of NaOH that was needed to neutralize all of the acid. 

Use stoichiometry to determine how many moles of acid must have been present in the titration experiment.

Use the mass of the acid and the moles of the acid present in the titration to determine the molar mass.

Calculate the molar mass.  

Mass unknown = 0.3089g

concentration NaOH = 0.3089M

intial mL in buret = 1.44

end point mL in buret = 13.72

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