Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M

Video transcript

Hello, everyone. Today, we have the following problem. Calculate the concentration of hydroxide ions for a solution with hydrogen ion concentration of 1.6 times 10 to the negative eight moller and determine if the solution is neutral, acidic or basic. So the first thing we need to do is we need to recall our equation for does her main P H and O H or hydrogen and hydroxide. We're going to have the concentration of hydrogen ions times the concentration of hydroxide ions equaling our dissociation constant or KW. And so if we rearrange this equation, we're going to get the concentration of hydroxide equally our dissociation constant divided by the concentration of hydrogen ions Furthering this equation, our constant or KW is going to be a constant that you can find in a reference text and it's going to be equal to one times 10 to the -14. And we have our concentration of hydrogen ions from the question stem which was 1. times 10 to the -8. We'll put those in brackets, someone find this, we will get 6.25 times 10 to the negative seven moller. So we'll keep track of that number. A general principle is that if the concentration of hydroxide ions is greater than one Times 10 to the -7, we will have a basic solution. If the concentration of hydroxide island is less than 1.0 times 10 to the negative seventh, we will have an acidic solution. And of course, if the concentration of hydroxide units or ions is equal to 1.8 times 10 to negative seventh, we will have a neutral species or a neutral solution. Because 6.25 times 10 to negative seventh is actually greater Than 1.0 times 10 to the -7. We're going to have a basic solution. And so with that, we have answered the question overall, I hope this helped until next time.