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iris [78.8K]
3 years ago
7

What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeCl3 is mixed with 200. mL of 0.182 M NaOH?

Chemistry
1 answer:
ratelena [41]3 years ago
7 0

Answer:

648.68 mg

Explanation:

The reaction that takes place is:

  • FeCl₃ + 3NaOH → Fe(OH)₃ + 3NaCl

First we<u> calculate how many moles of each reactant were added</u>, using the <em>given volumes and concentrations</em>:

  • FeCl₃ ⇒ 100 mL * 0.240 M = 24 mmol FeCl₃
  • NaOH ⇒ 100 mL * 0.182 M = 18.2 mmol NaOH

24 mmol of FeCl₃ would react completely with (24 * 3) 72 mmol of NaOH. There are not as many NaOH mmoles, so NaOH is the limiting reactant.

Now we <u>calculate how many moles of Fe(OH)₃ are formed</u>, using the <em>moles of the limiting reactant</em>:

  • 18.2 mmol NaOH * \frac{1mmolFe(OH)_3}{3mmolNaOH} = 6.07 mmol Fe(OH)₃

Finally we <u>convert 6.07 mmol Fe(OH)₃ to grams</u>, using its<em> molar mass</em>:

  • 6.07 mmol Fe(OH)₃ * 106.867 mg/mmol = 648.68 mg
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Given :

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