Seawater contains 34 g of salts for every liter of solution. Assuming that the solute consists entirely of NaCl (in fact, over 90% of the salt is indeed NaCl), calculate the osmotic pressure of seawater at 20 °C

Video transcript

Hi everyone here we have a question telling us Motrin autism is an antibiotic used to treat a number of bacterial and parasitic infections. A 100.0 millimeter injectable solution of Motrin iso. 171.2 g per mole contains 500.0 mg of the drug. And our question is, what is the osmotic pressure of the solution at 25°C. So we will start by calculating the polarity of the solution. Polarity equals 0.0 mg divided by 100 middle leaders of solution times 10 To the negative three g per one mg Times one Middle Eater over 10 to the negative. three leaders times one mole over the molar mass Which is 171.2 g. So our milligrams are canceling out, our grams are canceling out. Our middle leaders are canceling out which is gonna give us moles per liter which is polarity and that equals 0.02 9 - one Molar Itty. Next we're going to calculate for the osmotic pressure. So the osmotic pressure is going to equal 0.0-9-1 more clarity Times are constant which is 0. leaders times atmospheres divided by moles times, kelvin Times 298. Kelvin which is 25°C and our osmotic pressure Equals 0.7147 Atmospheres. And that is our final answer. Thank you for watching. Bye