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During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. How many moles of acid are present in 2.0 liters of this unknown solution?

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The moles of the acid in 2.0 liters of the unknown solution would be 8.0 moles

Since the acid is monoprotic, 1 mole of the acid will be required to stoichiometrically react with 1 mole of NaOH.

Using the formula:

   [tex]\frac{concentration of acid X volume of acid}{concentration of base X volume of base} = \frac{mole of acid}{mole of base}[/tex]

  • Concentration of acid = ?
  • Volume of acid = 10 mL
  • Concentration of base = 1.0 M
  • Volume of base = 40 mL
  • mole of acid = 1
  • mole of base = 1

Substitute into the equation:

[tex]\frac{concentration of acid X 10}{1.0 X 40} = \frac{1}{1}[/tex]

Concentration of acid = 40/10 = 4.0 M

To determine the number of moles of acid present in 2.0 liters of the unknown solution:

           Number of moles = Molarity x volume

                                   = 4.0 x 2.0 = 8.0 moles

More on stoichiometric calculations can be found here: https://brainly.com/question/8062886?referrer=searchResults

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