badwolfblue
Answered

A 25 mL sample of 0.100 M HNO3 completely reacts with NaOH according to this equation:


HNO3(aq) + NaOH (aq) ⟶ NaNO3(aq) + H2O(l)


How many moles of HNO3 are in the sample?

⇒ 0.0025 mol HNO3



What volume of 0.0500 M NaOH solution is required to completely react with the HNO3?


If someone could teach me how to do this, it would be awesome

Verified Answer :

taskmasters

It is a good thing that you already have answered the first question. Now, moving on to the second question, there exist an equation for the neutralization of acid by a base that is shown below,
                                          M₁V₁ = M₂V₂
Now, all the variables in the equation are given except for our unknown which is the V₂. Substituting the known values from the given above,
                                       (0.1 M)(25 mL) = (0.05 M)(V₂)
The value of V₂ from the equation above is 50 mL. Therefore, 50 mL of 0.05 M NaOH solution will be needed to completely react with HNO3.

CintiaSalazar

Taking into account the definition of molarity and reaction stoichiometry:

  • there are 0.0025 moles of HNO₃ in the sample.
  • the volume of 0.0500 M NaOH solution required to completely react with the HNO₃ is 50 mL.

Definition of molarity

Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.

The molarity of a solution is calculated by dividing the moles of solute by the volume of the solution:

\(Molarity=\frac{number of moles}{volume}\)

Molarity is expressed in units \(\frac{moles}{liter}\).

Moles of HNO₃ in the sample

In this case, you have a 25 mL sample of 0.100 M HNO₃. Being 1000 mL=1 L, then 25 mL= 0.025 L.

Replacing in the definition of molarity:

\(0.100 M=\frac{number of moles}{0.025 L}\)

Solving:

number of moles= 0.100 M×0.025 L

number of moles= 0.0025 moles

Finally, there are 0.0025 moles of HNO₃ in the sample.

Reaction stoichiometry

The balanced reaction is:

HNO₃ + NaOH ⟶ NaNO₃ + H₂O

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • HNO₃: 1 mole
  • NaOH: 1 mole  
  • NaNO₃: 1 mole
  • H₂O: 1 mole

Volume of 0.0500 M NaOH solution required

You can apply the following rule of three: If by reaction stoichiometry 1 mole of HNO₃ reacts with 1 mole of NaOH, 0.0025 moles of HNO₃ react with how many moles of NaOH?

\(amount of moles of NaOH=\frac{0.0025 moles of HNO_{3}x1 mole of NaOH }{1 mole of HNO_{3}}\)

amount of moles of NaOH= 0.0025 moles

You have a 0.0500 M NaOH solution. Replacing in the definition og molarity:

\(0.0500 M=\frac{0.0025 moles}{volume}\)

0.0500 M×volume= 0.0025 moles

volume= 0.0025 moles÷ 0.0500 M

volume= 0.05 L= 50 mL

Finally, the volume of 0.0500 M NaOH solution required to completely react with the HNO₃ is 50 mL.

Learn more about

molarity:

brainly.com/question/9324116

brainly.com/question/10608366

brainly.com/question/7429224

reaction stoichiometry

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