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Reptile [31]
3 years ago
11

A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500 ml of solution. what is the calcium ion concentration in thi

s solution
Chemistry
1 answer:
Nataly_w [17]3 years ago
5 0

First calculate the number of moles of CaBr2 given the molar mass of 199.89 g/mol.

moles CaBr2 = 0.9182 g / (199.89 g / mol) = 4.60 x 10^-3 mol

 

We see that each CaBr2 contains only 1 mole of Ca, so the moles of Ca is also:

moles Ca+ = 4.60 x 10^-3 mol

 

So the molarity of this is:

Molarity Ca+ = 4.60 x 10^-3 mol / 0.500 L

<span>Molarity Ca+ = 9.19 x 10^-3 M</span>

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3 years ago
6.0 mol Al reacts with 4.0 mol O2 to form Al2O3.
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Answer:

3.0 moles Al₂O₃

Explanation:

We do not know which of the reactants is the limiting reactant. Therefore, you need to convert both of the given mole values into the product. This can be done using the mole-to-mole ratio made up of the balanced equation coefficients.

4 Al + 3 O₂ -----> 2 Al₂O₃

6.0 moles Al            2 moles Al₂O₃
----------------------  x  -------------------------  =  3.0 moles Al₂O₃
                                    4 moles Al

4.0 moles O₂           2 moles Al₂O₃
----------------------  x  -------------------------  =  2.7 moles Al₂O₃
                                    3 moles O₂

As you can see, O₂ produces the smaller amount of product. This means O₂ is the limiting reactant. Remember, the limiting reactant is the reactant which runs out before the other reactant(s) are completely reacted. As such, the actual amount of Al₂O₃ produced is 2.7 moles.

However, since this problem is directly addressing how much Al₂O₃ is produced from Al, the answer you most likely are looking for is 3.0 moles Al₂O₃.

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