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Alina [70]
2 years ago
7

1A: Consider these compounds:

Chemistry
1 answer:
Setler [38]2 years ago
4 0

Solution :

Compound                      Ksp

$PbF_2$                               $3.3 \times 10^{-8}$

$Ni(CN)_2$                        $3 \times 10^{-23}$

FeS                                $8 \times 10^{-19}$

$CaSO_4$                           $4.93 \times 10^{-5}$

$Mg(OH)_2$                      $5.61 \times 10^{-12}$

Ksp of $Ni(CN)_2 and both compounds dissociate the same way. Hence $Mg(OH)_2$ is more soluble than $(B). \  Ni(CN)_2$

$Mg(OH)_2$  is less soluble than $(A). \ \ PbF_2 \ ()Ksp \  PbF_2 > Ksp \ \text{ of } \ Mg(OH)_2$

It is not possible to determine CD - $FeS \text{ or} \ CaSO_4$  is more or less soluble than $Mg(OH)_2$  as though they have a different Ksp values their molecular dissociation is also different and they may have a close solubility values.

$Ni(OH)_2$  can be directly compared with PbS, $AlPO_4, MnS$

$\text{For } \ Ni(OH)_2$

$AB_2(s) \rightarrow A^{2+} + 2B^{-}$

$Ni(OH)_2(s) \rightarrow Ni^{2+} + 2OH^-$

100

1-s s 2s

Ksp = [A2+][B-]^2 = s \times (2s)^2 = 4s^3

Hence they can be directly compared by Ksp values, smaller the Ksp, smaller the solubility.

For Silver Chloride

$AB(s) \rightarrow A^{x+}+B^{x-}$

$AgCl(s) \rightarrow Ag^+ + Cl^-$

1 0 0

1 - s s s

Ksp $=[A^{x+}][B^{x-}]=s \times s = s^2$

Hence, they can be directly compared by Ksp values, smaller the Ksp, smaller the solubility.

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Mr. Ragusa asks Hassan to make silver crystals from the following reaction.
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Answer:

Percentage yield = 61.7%

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated:

2AgNO₃ + Cu —> Cu(NO₃)₂ + 2Ag

Next, we shall determine the mass of AgNO₃ that reacted and the mass of Ag produced from the balanced equation. This is illustrated below:

Molar mass of AgNO₃ = 108 + 14 + (16×3)

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Molar mass of Ag = 108 g/mol

Mass of Ag from the balanced equation = 2 × 108 = 216 g

SUMMARY:

From the balanced equation above,

340 g of AgNO₃ reacted to produce 216 g of Ag.

Next, we shall determine the theoretical yield of Ag. This can be obtained as follow:

From the balanced equation above,

340 g of AgNO₃ reacted to produce 216 g of Ag.

Therefore, 51 g of AgNO₃ will react to produce = (51 × 216)/340 = 32.4 g of Ag.

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Finally, we shall determine the percentage yield of Ag. This can be obtained as follow:

Actual yield = 20 g

Theoretical yield = 32.4 g

Percentage yield =?

Percentage yield = Actual yield /Theoretical yield × 100

Percentage yield = 20 / 32.4 × 100

Percentage yield = 61.7%

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