(Will give medal!!)
1. Calculate the hydrogen ion concentration (H+) for an aqueous solution in which [OH^-] is 1 x 10^-4 mol/L. Is the solution basic, acidic, or neutral?
2. What reaction is spontaneous for the following cell?
Ag+ + e- >>> Ag (E* = 0.80V)
Ba^2+ + 2e- >>> Ba (E+ = -2.90V)
Stacey Warren - Expert brainly.com
Hey! We 've verified this expert answer for you, click below to unlock the details :)
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga.
Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus.
Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
For qn. 1, have you ever heard of the the equation [H+][OH-] = 1 * 10^(-14)?
The value at the end is K, the equilibrium dissociating constant of pure water (since it is neutral yo u will have equal concentrations of both ion in solution 1*10^-7, and this value is very small since water is really weak at dissociating).
By rearranging the formula and plugging in OH- concentration and rearranging, you will find the answer for H+ concentration. If you are not familiar with pH it is figuring out how acidic or basic a solution is, but using a logarithim scale. The general formula is pH= log [H+]. Use the concentration you got from the last step.
For qn. 2 reactions that have a do not have a positive reduction potential do not occur at standardized conditions because they require larger amounts of energy. Hope this leads you to your answer.