Kyleigh

Which equation represents what happens when a small amount of strong base is added to the buffer? OH- + A- A2- + H2O OH- + HA A- + H2O H3O+ + A- HA + H2O H3O+ + HA H2A+ + H2O

reuben made $135 for 9 hours of work at the same rate how much would he make for 5 hours of work

Pilgrims

First calculate the molarity (M) of each species. M H2 = moles H2 / L = 2.50 / 12.0 = 0.208 M M S2 = moles S2 / L = 1.35 x 10^-5 / 12.0 = 1.13 x 10^-6 M M H2S = moles H2S / L = 8.70 / 12.0 = 0.725 M Kc = [H2S]^2 / ([H2]^2[S2]) = (0.725^2) / ((0.208)^2(1.1...

The answer is obviously 16.

.5x.6?

you take the inverse tan. So tan-1(1.8956)= 62.2

The difference between two numbers is 34. The larger exceeds 3 times the smaller by 4. Find the numbers.

Ok, sure. I added some more info to my previous questions. Please take a look. Thank you for your help!

I think it would be the last option, as a stronger base will need less of an acid to bring the pH to a neutral 7. Is this correct?

I am not the best at working through the problems, but I came to A, 2.21, given the concentration and Ka.

I got D. Given that D is the largest reaction, I would predict it would have the largest K value.

I would choose 5.1. If one third of the base is added (in which the whole 15ml was utilized to bring to a basic state of 8.6), it must be 5.1, as the other answers are mathematically impossible.

I go there too. Looks like everyone on here does lol

For anyone that needs to know this now, it is the capture of Napoleon. You're welcome ;)