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oksano4ka [1.4K]
3 years ago
6

A student finds two unlabeled flasks of clear liquids. One is believed to be 0.1 m nacl and the other to be 0.1 m naclo3. What i

s a quick way of determining what is in each flask?
Chemistry
1 answer:
KonstantinChe [14]3 years ago
6 0

Answer:

  • Add AgNO₃ solution to both unlabeled flasks: based on solubility rules, you can predict that when you add AgNO₃ to the NaCl solution, you will obtain AgCl precipitate, while no precipitate will be formed from the NaClO₃ solution.

Explanation:

<u>1. Adding AgNO₃ to NaCl solution:</u>

  • AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq)

<u>2. Adding AgNO₃ to NaClO₃ solution</u>

  • AgNO₃ (aq) + NaClO₃ (aq) → AgClO₃ (aq) + NaNO₃ (aq)

<u />

<u>3. Relevant solubility rules for the problem.</u>

  • Although most salts containing Cl⁻ are soluble, AgCl is a remarkable exception and is insoluble.

  • All chlorates are soluble, so AgClO₃ is soluble.

  • Salts containing nitrate ion (NO₃⁻) are generally soluble and NaNO₃ is not an exception to this rule. In fact, NaNO₃ is very well known to be soluble.

Hence, when you add AgNO₃ to the NaCl solution the AgCl formed will precipitate, and when you add the same salt (AgNO₃) to the AgClO₃ solution both formed salts AgClO₃ and NaNO₃ are soluble.

Then, the precipiate will permit to conclude which flask contains AgCl.

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The products obtained from the dissociation of HNO₃ in water are hydronium ion, H₃O⁺ and nitrate ion, NO₃¯

An acid is a substance which when dissolved in water produces hydronium ion, H₃O⁺ as the only positive ion.

Strong acid ionize completely in water while weak acid only ionize to a certain degree (i.e partially) in water

Trioxonitrate (v) acid, HNO₃ is a strong acid and will ionize complete in water to form hydronium ion, H₃O⁺ and nitrate ion, NO₃¯ as illustrated below:

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