Question #71391

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Question #71391

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Answer 1 · 2017-03-27T23:20:16

No, the solution is not saturated.

Explanation:

Your tool of choice here will be the solubility graph of potassium nitrate, ${KNO}_{3}$ $"KNO"_3$ , which looks like this

![www.nakka-rocketry.net]()

The curve shows you the amount of potassium nitrate than can be dissolved per $100 mL$ $"100 mL"$ of water at various temperatures in order to create a saturated solution of potassium nitrate.

For the sake of simplicity, let's assume that the graph shows the solubility of the salt per $100 g$ $"100 g"$ of water.

Now, if you draw a vertical line starting from $90^{\circ} C$ $90^@"C"$ , you will notice that it intersects the curve at approximately $200 g$ $"200 g"$ of potassium nitrate per $100 g$ $"100 g"$ of water.

This represents the solubility of the salt at this temperature. In other words, you can only hope to dissolve $200 g$ $"200 g"$ of potassium nitrate for every $100 g$ $"100 g"$ of water at $90^{\circ} C$ $90^@"C"$ .

Your solution contains $30 g$ $"30 g"$ of potassium nitrate per $100 g$ $"100 g"$ of water at this temperature, so it will not be saturated because you can dissolve an additional

$200 g . - . 30 g = {170 g KNO}_{3}$ $"200 g"color(white)(.) - color(white)(.)"30 g" = "170 g KNO"_3$

for every $100 g$ $"100 g"$ of water at this temperature. You can thus say that the solution is unsaturated.

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Question #71391

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