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Effectus [21]
3 years ago
7

A bottle of wine contains 9.81 grams of C2H5OH, dissolved in 87.5 grams of water. The final volume of the solution is 100.0 mL.

Calculate the concentration of ethanol in wine in terms of molarity and mass percent.
Chemistry
1 answer:
dimulka [17.4K]3 years ago
3 0

Answer:

[EtOH] = 2.2M and Wt% EtOH = 10.1% (w/w)

Explanation:

1. Molarity = moles solute / Volume solution in Liters

=> moles solute = mass solute / formula weight of solute = 9.8g/46g·mol⁻¹ = 0.213mol EtOH

=> volume of solution (assuming density of final solution is 1.0g/ml) ...

volume solution =  9.81gEtOH + 87.5gH₂O = 97.31g solution x 1g/ml = 97.31ml = 0.09731 Liter solution

Concentration (Molarity) = moles/Liters = 0.213mol/0.09731L = 2.2M in EtOH

2. Weight Percent EtOH in solution (assuming density of final solution is 1.0g/ml)

From part 1 => [EtOH] = 2.2M in EtOH = 2.2moles EtOH/1.0L soln

= {(2.2mol)(46g/mol)]/1000g soln] x 100% = 10.1% (w/w) in EtOH.

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3 years ago
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bearhunter [10]

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4 0
3 years ago
Purchasing the correctly sized BMX bike is based on the height of the rider. In order to fit a customer, the salesman can use th
Phantasy [73]
Answer: Your best answer is A.

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“b = (0.29 x h)+ 1.35”
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“b = (0.29 x 60)+ 1.35”
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5 0
2 years ago
Paul determines that the hydrogen ion concentration of his unknown solution is 3.60×10^-5 M. what is the pH of this solution?​
vivado [14]

Answer:

<h2>pH = 4.44 </h2>

Explanation:

The pH of a substance can be found by using the formula

p H  =  -   log[ H^{ + }  ]

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From the question

[ H + ] = 3.60 × 10^-5 M

So the pH is

pH =  -  log(3.60 \times  {10}^{ - 5} )  \\  =4.44369749923

We have the final answer as

<h3>pH = 4.44 </h3>

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3 years ago
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Explanation:

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              P_{i} = \frac{k_{i}}{V_{i}}

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