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HClO4   +NaOH   ----->  NaClO4  +  H2O
moles  of  NaOH =  (0.0832  x  50 ) /1000=  4.16 x10^-3  moles
since  the  mole  ratio  of  HClO4  to  NaOH  is  1:1   the  moles  of  HClO4  is also  4.16  x  10^-3  moles

volume  of   HClO4  is therefore =  moles/ molarity
  that  is   4.16  x  10^-3mol/  0.167 mol/L=  0.0249L
multiply  by  1000  to  convert  to  ml
0.0249  x 1000=  24.9  ml

The volume of in milliliters of the HClO₄ needed to neutralize the NaOH solution is 24.9mL

Stoichiometry

From the question, we are to determine the volume of HClO₄ needed to neutralize the NaOH solution

First, we will write the balanced chemical equation for the reaction

The balanced chemical equation for the reaction is

HClO₄ + NaOH → NaClO₄ + H₂O

This means

1 mole of HClO₄ is required to neutralize 1 mole of NaOH

Now, we will determine the number of moles of NaOH present in the solution

From the given information

Volume of NaOH = 50.00 mL = 0.05 L

Concentration of NaOH = 0.0832 M

Using the formula,

Number of moles = Concentration × Volume

Then,

Number of moles of NaOH present = 0.0832 × 0.05

Number of moles of NaOH present = 0.00416 mole

Now,

Since 1 mole of HClO₄ is required to neutralize 1 mole of NaOH

Then,

0.00416 mole of HClO₄ will be required to neutralize the 0.00416 mole of NaOH

Thus, the number of moles of HClO₄ required is 0.00416 mole

Now, for the volume of HClO₄ required

From the formula,

[tex]Volume = \frac{Number\ of\ moles }{Concentration}[/tex]

Then,

Volume of HClO₄ needed = [tex]\frac{0.00416}{0.167}[/tex]

Volume of HClO₄ needed = 0.0249101 L

Volume of HClO₄ needed = 24.9101 mL

Volume of HClO₄ needed ≅ 24.9 mL

Hence, the volume of in milliliters of the HClO₄ needed to neutralize the NaOH solution is 24.9mL

Learn more on Stoichiometry here: https://brainly.com/question/10382262

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