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Sodium Sulphate crystallises out as Na2SO4.10H2O. It is prepared by titration. 25.0cm^3 aquas of NaOH solution having a concentration of 2.24 mol/dm^3 reacted with H2SO4 to give Na2SO4.10H2O. The molecular mass of Na2SO4.10H2O = 322 grams. Find the % yield of Na2SO4.10H2O.

Answers

Answer 1

Answer:

Assuming the mass of Na2SO4.10H2O obtained from the crystallization was: 8.5g

The % yield is 94.3%

Explanation:

Assuming the mass of Na2SO4.10H2O was:

Based on the reaction:

2NaOH + H2SO4 + 8H2O →Na2SO4.10H2O

Where 2 moles of NaOH reacts producing 1 mole of Na2SO4.10H2O

To solve this question we need to find the moles of NaOH added. With the moles and the reaction we can find the moles of Na2SO4.10H2O and its actual theoretical yield. Assuming the mass of Na2SO4.10H2O produced was: 8.5g

we can find the percent yield as follows:

Moles NaOH:

25.0cm³ = 0.0250dm³ * (2.24mol/dm³) = 0.056 moles NaOH

Moles Na2SO4.10H2O:

0.056 moles NaOH * (1mol Na2SO4.10H2O / 2mol NaOH) = 0.028 moles Na2SO4.10H2O

Mass Na2SO4.10H2O:

0.028 moles Na2SO4.10H2O * (322g / mol) = 9.016g Na2SO4.10H2O = Theoretical yield

Percent yield is 100 times the ratio between actual yield:

8.5g / 9.016g * 100 = 94.3%


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Answers

Explanation:

The steps given in the question are incorrect.

Step 1 should be convert atoms to moles (n). Step 2 should be convert moles (n) to mass (m).

Step 1

Use dimensional analysis to convert the number of atoms to moles.

1 mole atoms = 6.022 × 10²³ atoms

n(Ag) = 2.3 × 10²⁴ Ag atoms × (1 mol Ag/6.022 × 10²³ Ag atoms) = 3.8193 mol Ag

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Convert the moles of Ag to mass.

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Answer:

[tex]\boxed {\boxed {\sf 3.8 \ moles \ of \ sulfur}}[/tex]

Explanation:

We are asked to convert a number of atoms to moles.

We can convert atoms to moles using Avogadro's Number, which is 6.022 × 10²³. This is the number of particles (atoms, molecules, formula units, etc.) in 1 mole of a substance. In this problem, the particles are atoms of sulfur. There are 6.022 ×10²³ atoms of sulfur in 1 mole of sulfur.

We use dimensional analysis to convert atoms to moles. This involves setting up ratios. Use Avogadro's Number and the underlined information to make a ratio.

[tex]\frac {6.022 \times 10^{23} \ atoms \ S}{1 \ mol \ S}[/tex]

We are converting 2.3 ×10²⁴ atoms of sulfur to moles, so we multiply by this value.

[tex]2.3 \times 10^{24} \ atoms \ S *\frac {6.022 \times 10^{23} \ atoms \ S}{1 \ mol \ S}[/tex]

Flip the ratio. It is equivalent, but it allows the units of atoms of sulfur to cancel.

[tex]2.3 \times 10^{24} \ atoms \ S *\frac {1 \ mol \ S}{6.022 \times 10^{23} \ atoms \ S}[/tex]

[tex]2.3 \times 10^{24} *\frac {1 \ mol \ S}{6.022 \times 10^{23} }[/tex]

[tex]\frac {2.3 \times 10^{24} }{6.022 \times 10^{23} } \ mol \ S[/tex]

[tex]3.819329127 \ mol \ S[/tex]

The original measurement of atoms (2.3 ×10²⁴) has 2 significant figures, so our answer must have the same. For the number we calculated that is the tenths place. The 1 in the hundredths place to the right (3.819329127) tells us to leave the 8 in the tenths place (3.819329127).

[tex]3.8 \ mol \ S[/tex]

2.3 ×10²⁴ atoms of sulfur is equal to approximately 3.8 moles of sulfur.

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