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jeyben [28]
2 years ago
7

In an experiment, a 88.11 mL sample of unknown silver nitrate solution was treated with 9.753 g of sodium chloride, resulting in

4.576 g of precipitate. Calculate the molarity of the silver nitrate solution
Chemistry
1 answer:
zlopas [31]2 years ago
4 0

Answer:

0.362 M

Explanation:

The reaction that takes place is:

  • AgNO₃ + NaCl → NaNO₃ + AgCl(s)

First we <u>convert the mass of AgCl (the precipitate) into moles</u>, using its <em>molar mass</em>:

  • 4.576 g AgCl ÷ 143.32 g/mol = 0.0319 mol AgCl

Now we <u>convert AgCl moles into AgNO₃ moles:</u>

  • 0.0319 mol AgCl * \frac{1molAgNO_3}{1molAgCl} = 0.0319 mol AgNO₃

Finally we <u>calculate the molarity</u>, after <em>converting 88.11 mL to L</em>:

  • 88.11 mL / 1000 = 0.08811 L
  • Molarity = 0.0319 mol AgNO₃ / 0.08811 L = 0.362 M
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When nahco3 completely decomposes, it can follow this balanced chemical equation:

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percentage yield = experimental yield/theoretical yield × 100

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Therefore the percentage yield of the product is 98.456%

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