Question

25.0 ml of a 6.0 m hno3 stock solution is diluted using water to 100 ml. How many moles of hno3 are present in the dilute solution?

Answer 1

0.15 moles

Further explanation

Given:

• 25.0 ml of a 6.0 M HNO₃ stock solution is diluted using water to 100 ml.
• V₁ = 25.0 ml = 0.025 liters
• Volume of water = 100 ml = 0.1 liters

Question:

How many moles of HNO₃ are present in the dilute solution?

The Process:

Recall that the dilution equation works because the number of moles remains the same, both for the initial and final states.

Therefore we can calculate the number of moles of HNO₃ are present in the dilute solution based on the initial conditions.

$\boxed{ \ Concentration \ (M) = \frac{moles \ (n)}{volume \ (V)} \ } \rightarrow \boxed{ \ n = MV \ }$

n = 6 x 0.025

n = 0.15 moles

Thus there is 0.15 mol of HNO₃ present in dilute solution.

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Notes:

• Dilution represents the addition of a solvent (water) without adding solutes. In dilution, the mole of the solute remains, so the concentration of the solution will drop.
• When calculating dilution factors, the units of volume and concentration must remain consistent.

Dilution calculations can be typically performed following the formula:

$\boxed{ \ M_1V_1 = M_2V_2 \ }$.

with,

• V₁ and V₂ as volume before and after dilution
• M₁ and M₂ as the molarity of the solution before and after dilution.

Once again as a reminder: the dilution equation works because the number of moles remains the same.

The equation which represents the correct way to find the concentration of the dilute solution (M₂) is

$\boxed{ \ M_2 = \frac{M_2V_2}{V_2} \ }$.

V₂ = V₁ + Volume of water

From our problem above, let us calculate the concentration of the dilute solution.

Prepare V₂ = 25 ml + 100 ml = 125 ml (or 0.125 liters)

$\boxed{ \ M_2 = \frac{6 \times 25}{125} \ }$.

Hence the concentration of the dilute solution is 1.2 M.

Now, let us check the number of moles of HNO₃ is present in the dilute solution (or based on final conditions).

n = M₂ x V₂

n = 1.2 x 0.125

n = 0.15 mol

Conclusion: n₁ = n₂ has been proven.

The dilution equation works because the number of moles remains the same.

_ _ _ _ _ _ _ _ _ _

Notes:

• A solution consists precisely of a solute and a solvent.  
• There are several ways to properly express the concentration of a solution, one of which is molarity. Molarity is also known as molar concentration with the symbol unit M or molar or mole/L.
• The molarity (M) of a solution is calculated by allowing the moles of solute and divided by the number of liters of solution.

$\boxed{ \ molarity = \frac{moles \ of \ solute}{liters \ of \ solution} \ }$

Learn more

1. To make a 0.500 M solution, one could take 0.500 moles of solute and add? brainly.com/question/10278982
2. An example of the dilution of a solution brainly.com/question/4516437  
3. How many liters of the  50%  solution and how many liters of the  90%  solution will be used? brainly.com/question/13034221

Answer 2

Answer:

The answer to your question is: 6 moles of HNO₃

Explanation:

Data

Volume = 25 ml

Concentration = 6 M HNO₃

Diluted 100 ml

Formula

Molarity = # moles / volume

# of moles = Volume x Molarity

Process

# of moles = 0.10 x 6

                 = 6 moles