Water superheated under pressure to 200 °C and 750 atm has Kw = 1.5 * 10-11. What is 3H3O+ 4 and 3OH-4 at 200 °C? Is the water acidic, basic, or neutral?

Video transcript

well everyone's in this problem, we're given the kw of water which is equal to 1.89 times 10 to the negative nine. When the water is being super heated to 450 degrees Celsius and an 810 80 m under pressure. So at this temperature where the concentrations of H 30 plus and O H minus is the water neutral, acidic or basic. So the chemical equation that we're dealing with here is that we have two moles of H 20. And it's an equilibrium with H 30 plus as well as O. H minus. So if you recall the kw occasion here is equal to the concentration of H 30 plus, multiplied by the concentration of L. H minus. So again we're at degrees Celsius, R. K. W. Here which is given to us in the problem is equal to 1.89 times 10 to the negative nine. So in pure water the concentration of O. H minus is equal to the concentration of H 30 plus. So that also means then that my K. W. Is just equal to the concentration of O. H minus, raised to the power of two. So then the concentration again of O. H. - is equal to the concentration of H. Plus. Which then just equal to the square root of R. K. W. Value. Of course we already are given the kw value. So we just need to plug this in. So we're basically taking the square root of 1. times 10 to the negative nine. So once you put that into a calculator, we get the value that's equal to 4. times 10 to the negative five molars. So since The concentration of O. H. - is equal to the concentration of H. 30. Plus, we get that this value of the polarity here, they're equal to each other. So we have an overall neutral solution. So again, this problem being asked where the concentrations of HDL plus and a. O. H minus recent that they're both equal to each other and they're both equal to this value here and that we have a neutral solution. So this is going to be my final answer for this problem.