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harkovskaia [24]
3 years ago
14

If you add water to a 15.00 mL solution of 3.22 M CaCl2 (MM=110.98 g/mol) in order to create a solution that is 15.00% CaCl2 by

mass, what is the final mass of the new solution. The density of water is exactly 1.00 g/mL. Assume that the density of the CaCl2 solution is also exactly 1.00 g/mL.
Chemistry
1 answer:
lesya [120]3 years ago
3 0

The mass of the new solution is 35.7 g.  

Step 1. Calculate the <em>moles of CaCl₂</em> in the first solution.  

[\text{Moles of CaCl}_{2} = \text{0.015 00 L solution} \times \frac{\text{3.22 mol CaCl}_{2}}{\text{1 L solution }} = \text{0.048 30 mol CaCl}_{2}\\  

Step 2. Calculate the <em>mass of CaCl₂</em>.  

\text{Mass of CaCl}_{2} = \text{0.048 30 mol CaCl}_{2} \times \frac{\text{110.98 g CaCl}_{2} }{\text{1 mol CaCl}_{2} } = \text{5.360 g CaCl}_{2} \\  

Step 3. Calculate the mass of the new solution.


\text{Mass of solution }= \text{5.360 g CaCl}_{2} \times \frac{\text{100 g solution }}{\text{15.00 g CaCl}_{2} } = \textbf{35.7 g solution} \\  

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1. The pH of 1.0 M trimethyl ammonium (pH = 1.01) is lower than the pH of 0.1 M phenol (5.00).

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1. The pH of a compound can be found using the following equation:

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First, we need to find [H₃O⁺] for trimethyl ammonium and for phenol.

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We can calculate [H₃O⁺] using the Ka as follows:

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2. The difference in pH values for the two acids is:

\Delta pH = pH_{C_{6}H_{5}OH} - pH_{(CH_{3})_{3}NH^{+}} = 5.00 - 1.01 = 4.95

Therefore, the difference in pH values is 4.95.

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