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3 years ago

Suppose you wanted to know how many grams of KCl would be left if 350mL of

Chemistry

1 answer:

strojnjashka [21]3 years ago

8 0

Answer:

52.2g of KCl would be left

The mass of KCl will remain despite the solution is been heated

Explanation:

When you are heating a solution, just the solvent (In this case, water), will be evaporated and, in theory, the mass of KCl will remain despite the solution is been heated.

Now, the mass of KCl that you can obtain from 350mL of a 2.0M solution will be:

<em>Moles KCl:</em>

350mL = 0.350L * (2.0mol / L) = 0.700 moles

<em>Mass KCl -Molar mass: 74.55g/mol-:</em>

0.700mol * (74.55g/mol) = 52.2g of KCl would be left

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0.85 moles formula units of lead nitrate will produce 0.57 moles formula units of chromium (III) nitrate.

<h3>Explanation</h3>

Typically, the oxidation state of Pb in lead nitrate tend to be +2. In other words, Pb in lead nitrate tends to exist as $\text{Pb}^{2+}$ ions. The formula for a nitrate ion is ${\text{NO}_3}^{-}$ . The charge on each of the nitrate ion is -1. The charge on the two ions should balance. As a result, each $\text{Pb}^{2+}$ ion in lead nitrate would pair up with two ${\text{NO}_3}^{-}$ ions. The formula for lead nitrate will be $\text{Pb}({\text{NO}_3})_2$ . Each formula unit of lead nitrate will contain one $\text{Pb}^{2+}$ ion and two ${\text{NO}_3}^{-}$ ions.

The "III" in the name "chromium (III) nitrate" is a Roman Numeral. It indicates that the oxidation state of Cr in chromium (III) nitrate is +3. The Cr in that compound will exist as $\text{Cr}^{3+}$ . Similarly, each $\text{Cr}^{3+}$ will pair up with three ${\text{NO}_3}^{-}$ ions. The formula for chromium (III) nitrate will be $\text{Cr}(\text{NO}_3})_3$ . Each formula unit of chromium (III) nitrate will contain one ${\text{NO}_3}^{-}$ ion and three ${\text{NO}_3}^{-}$ ions.

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