In this experiment an EDTA titration was performed. Another common type of titra

Question

In this experiment an EDTA titration was performed. Another common type of titration is an acid-base titration. Specifically, a neutralization titration can be used to determine the concentration of a strong acid if it is titrated with a strong base whose concentration is known. This method uses stoichiometry to determine the unknown acid’s concentration. Let’s say a student had 1.0 M sodium hydroxide (NaOH) and found a solution of sulfuric acid (H2SO4) whose label had faded. She took 10.0 mL of the H2SO4, added phenolphthalein as an indicator, and titrated the solution. It took 25.8 mL of the NaOH to complete the titration. What was the concentration of the H2SO4? The neutralization reaction is below: H2SO4 (aq) + 2 NaOH (aq) --> 2 H2O (l) + Na2SO4 (aq)

Explanation / Answer

H2SO4 (aq) + 2 NaOH (aq) --> 2 H2O (l) + Na2SO4 (aq)

1 mole of H2SO4 requires 2 moles of NaOH for neutralisation

so given no. of moles NaOH = Molarity of NaOH*Vol in lt of NaOH consumed

                                          = 1*0.0258 = 0.0258 moles

According to balanced equation

2 moles of NaOH requires ............... 1mole of H2SO4

0.0258 moles of NaOH ............................?

       = 0.0258/2 = 0.0129 moles of H2SO4

Molarity of H2SO4 = no.of moles/Vol.in lt = 0.0129/0.01 = 1.29M

so the concentration of H2SO4 is 1.29M or 1.3 M

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