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50.0 cm³ of 0.100 mol l⁻¹ ammonia solution was transferred to a 250 cm³ volumetric flask - Scottish Highers Chemistry - Question 23 - 2022

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Question 23

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50.0 cm³ of 0.100 mol l⁻¹ ammonia solution was transferred to a 250 cm³ volumetric flask. The flask was made up to the mark with deionised water. The final concentr... show full transcript

Worked Solution & Example Answer:50.0 cm³ of 0.100 mol l⁻¹ ammonia solution was transferred to a 250 cm³ volumetric flask - Scottish Highers Chemistry - Question 23 - 2022

Step 1

Calculate the number of moles of ammonia

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Answer

To find the number of moles of ammonia in the original solution, use the formula:

n=CimesVn = C imes V

Where:

  • ( n ) = number of moles
  • ( C ) = concentration (0.100 mol l⁻¹)
  • ( V ) = volume (50.0 cm³ = 0.0500 l)

Thus, n=0.100×0.0500=0.00500 molesn = 0.100 \times 0.0500 = 0.00500 \text{ moles}

Step 2

Calculate the final concentration in the 250 cm³ flask

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Answer

The final volume in the flask is 250 cm³, which is 0.250 l. The final concentration can be determined using:

Cf=nVfC_f = \frac{n}{V_f}

Substituting the values calculated:

Cf=0.005000.250=0.0200 mol l⁻¹C_f = \frac{0.00500}{0.250} = 0.0200 \text{ mol l⁻¹}

Expressing this in scientific notation gives us: Cf=2.0×10−2 mol l⁻¹C_f = 2.0 \times 10^{-2} \text{ mol l⁻¹}

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