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egoroff_w [7]
3 years ago
15

opper(I) ions in aqueous solution react with NH 3 ( aq ) according to Cu + ( aq ) + 2 NH 3 ( aq ) ⟶ Cu ( NH 3 ) + 2 ( aq ) K f =

6.3 × 10 10 Calculate the solubility (in g·L−1) of CuBr ( s ) ( K sp = 6.3 × 10 − 9 ) in 0.10 M NH 3 ( aq ) .
Chemistry
1 answer:
Y_Kistochka [10]3 years ago
5 0

Answer:

55.373g/l

Explanation:

The dissolved amount of sparingly soluble salts is interlinked with a unitlesss quantity called as solubility product. It is a fixed quantity that only increases with the rise in temperatures and is used to predict the salting out of compounds. If the value of ionic product (Q) is larger than (Ksp), precipitation of compound occurs.

Given:

The solubility product of CuBr is 6.3×10−9.

The concentration of NH3 is 0.10 M.

Formula and Calculations:

The dissolution reaction (I) of CuBr is shown below.

The reaction showing dissolution of CuBr in NH3 is shown below.

The above reaction can be obtained by adding reaction (I) and (II) as shown below.

The equilibrium constants will get multiplied.

Suppose the solubility of CuBr is “s”.

It is given that concentration of NH3 is 0.10 M.

The equilibrium constant expression for the above reaction is as follows,

Here,

The concentration of pure solids is 1 M. Thus, the concentration of CuBr is 1 M.

As calculated, the value of Ksp is 396.9.

Substitute all the required values in above formula.  

On further solving above equation,

Therefore, the solubility of CuBr in ammonia is 0.386 M.

The formula to calculate solubility

Solubuility (g/l)= Molarity(M) x Molarmass

Chemistry homework question answer, step 2, image 10

The molar mass of CuBr is 143.45 g/mol.

The formula to calculate solubility in g/L is given below.

The molar mass of CuBr is 143.45 g/mol.

therefore,

solubility = 0.386M x 143.45g/mol

where (M = mol/l)

solubility = 55.375g/l

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Answer:

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Explanation:

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Using the chemical equation in the picture, if you have 1.5 grams of Fe, how many moles of Fe would you have? (Round answer to 2
gavmur [86]

0.019moles

Explanation:

Given parameters:

Mass of Fe₂O₃ = 1.5g

Unknown:

Number of moles of Fe produced = ?

Solution:

To solve this problem, we must work from the known to the unknown. The known specie here is the mass of Fe₂O₃.

First inspect the equation and balance it;

     2Fe₂O₃  +    3C    →    4Fe   +    3CO₂

Now find the number of moles of Fe₂O₃

Number of moles of Fe₂O₃ = \frac{mass}{molar mass}

 molar mass of Fe₂O₃ = 2(56) + 3(16) = 112 + 48  = 160g/mol

 Number of moles = \frac{1.5}{160} = 0.009375moles

 From the equation, we see that;

   2 moles of Fe₂O₃ produced 4 moles of Fe

   0.009375 moles of Fe₂O₃ will produce \frac{0.009375 x 4}{2} = 0.01875‬moles of Fe

To 2 decimal places;

     0.019moles

learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly

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