The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.
a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?

Question

The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.

a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?

Accepted Answer

Welcome back everyone at a carbon dioxide partial pressure of 1 a.m. and 25 Celsius. The solubility of carbon dioxide in water is 3.42 times 10 to the negative second power moles per liter, calculate the solubility of carbon dioxide in grams per milliliter at 25 Celsius. If the partial pressure of CO two is 850 millimeters of mercury, we're going to begin by thinking of Henry's law where we should recall. Henry's law is defined by the solubility of our gas in a liquid, which is set equal to Henry's law constant represented by K sub H and that is then multiplied by the partial pressure of our gas above the liquid. So we're going to begin by first determining the solubility of our gas which we are being asked about in this prompt being carbon dioxide. So finding the solubility of carbon dioxide, we are going to take our Henry's law constant for carbon dioxide, which is given in our prompt as 3.42 times 10 to the negative second power moles per liter. And we will incorporate units of ATM S in the denominator as well. So we would have times ATM. This is then going to be multiplied by the partial pressure of carbon dioxide which at 25 Celsius is given in our pump at as being 850 millimeters of mercury. Now, for the solubility of carbon dioxide, we want our final units to be in moles per liter. So we're going to need to multiply our partial pressure of carbon dioxide to go from millimeters of mercury in the denominator to then ATM in the numerator. And so we would recall from our textbooks that we have 760 millimeters of mercury equivalent to one ATM in the numerator. So canceling out units of ATM as well as millimeters of mercury. We are left with moles per liter as our final units for the solubility of carbon dioxide. And so we would calculate a solubility equal to the value of 0.03825 moles per liter for carbon dioxide. Now, we're going to need to figure out the solubility in grams per milliliter as the prompt asks. So, recalculating, we've got the solubility of CO2 and grams per milliliter. We would find this by taking our solubility expressed in moles per liter, which we just calculated above as 0.03825 moles of carbon dioxide per liter. And we will multiply to go from moles in the denominator to then grams in the numerator. So we specifically will recall our molar mass of carbon dioxide from the periodic table where we would find we have 44.01 g of carbon dioxide per mole of carbon dioxide. So canceling out then moles of carbon dioxide, we have grams per liter and we need grams per milliliter. And so our third conversion factor that we would multiply by is to go from leaders in the numerator, actually two male leaders in the denominator. So we would recall that our prefix Milly tells us that we have an equivalent of 10 to the negative third of our base unit liter. So then canceling out liters, we are left with grams per milliliter as our final units of solubility. And this will simplify so that we have a solubility of carbon dioxide equal to a value of 1.68338 times 10 to the negative third power gram per milliliter of carbon dioxide. Now we're going to need to round our answer to a total of three significant figures so that we can finish off with a value of 1.68 times 10 to the negative third grams per milliliter of carbon dioxide as its solubility. And so that would be our final answer to complete this example of the solubility of carbon dioxide in grams per liter at 25 Celsius. I hope that this made sense and let us know if you have any questions

The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.
a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?

Verified video answer for a similar problem:

Key Concepts

Henry's Law

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Temperature Effects on Solubility

The solubility of NH3 gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.a.What is the solubility of NH3 if its partial pressure is reduced to 225.0 mmHg?

Verified video answer for a similar problem:

Key Concepts

Henry's Law

Solubility

Temperature Effects on Solubility

The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.
a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?