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ANEK [815]
3 years ago
7

A solution is prepared by adding 27.00 mL of 2.19 M MgCl2 to enough water to make 122.00 mL. What is the Cl- concentration of 40

.00 mL of the dilute solution?
Need help with this chemistry question that I'm unsure about with explanation please and thank you

DO NOT include units or chemical symbols in your answer
Chemistry
1 answer:
xeze [42]3 years ago
8 0

Answer:

<em>3.88x10⁻²</em>

Explanation:

First, the amount of moles initially in the volume of the concentrated MgCl2 solution is determined:

1000 mL solution ____ 2.19 moles of MgCl₂

27.00 mL solution _____ X = 5.91x10⁻² mol of MgCl₂

<em>Calculation:</em> 27.00 mL x 2.19 moles / 1000 mL = 0.05913 moles ≡ 5.91x10⁻² mol of MgCl₂

This is the amount of moles of MgCl₂ in both the initial and the diluted solution, since only water was added to the first solution, therefore, in 122.00 mL of the new solution, there are 5.91x10⁻² mol of MgCl₂. Now it is necessary to calculate the amount of moles in 40 mL of the new solution prepared:

122.00 mL of solution _____ 5.91x10⁻² mol of MgCl₂

40.00 mL of solution ____ X = 1.94x10⁻² of MgCl₂

<em>Calculation:</em> 40.00 mL x 5.91x10⁻² mol / 122.00 mL = 0.01939 moles ≡ 1.94x10⁻² MgCl₂

Now, when the MgCl₂ compound is in an aqueous solution, it dissociates into the ions that form it as follows:

MgCl₂ ⇒ Mg⁺² (aq) + 2 Cl⁻ (aq)

Therefore, for each mole of MgCl₂ that dissolves in water, it will dissociate producing two moles of Cl⁻ chloride ion. Mathematically:

1 mole of MgCl₂ ____ 2 moles of Cl⁻

1.94x10⁻² moles of MgCl₂ _____ X = 3.88x10⁻² moles of Cl⁻

<em>Calculation:</em> 1.94x10⁻² moles x 2 moles / 1 mole = 0.03877 ≡ 3.88x10⁻² moles of Cl⁻

Therefore, <em>in 40.00 mL of the new solution, there will be a concentration of 3.88x10⁻² moles of Cl⁻</em>

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