A buffer is prepared by dissolving 0.0250 mol sodium nitrite in 250 mL of 0.0410 M

Question

A buffer is prepared by dissolving 0.0250 mol sodium nitrite in 250 mL of 0.0410 M

nitrous acid. Assuming no volume change from dissolving, what is the pH of this buffer?

Answer 1

Its oops, not the way you spelled it bob. Jeez do the teachers know about this

Answer 2

Use the Henderson-Hasselbalch equation.

pH = pKa + log [(base)/(acid)
(acid) = 0.410 M nitrous acid
(base) = 0.0250 mols NaNO3/0.250 L = ?
pKa HNO2 = -log Ka HNO2
Post your work if you get stuck.

Answer 3

00ps. typo. That should be NaNO2 instead of NaNO3.

(acid) = 0.0410 M HNO2 and not 0.410.

Answer 4

Jeez. I said it was a typo. What more do you want? And for your Jeez that's spelled cheese. Do your friends know about this. We could start a club.

Answer 5

A buffer is prepared by dissolving 0.0250 mol sodium nitrite in 250 mL of 0.0410 M

Its oops, not the way you spelled it bob. Jeez do the teachers know about this

*you're

Use the Henderson-Hasselbalch equation.

00ps. typo. That should be NaNO2 instead of NaNO3.

oop-

Jeez. I said it was a typo. What more do you want? And for your Jeez that's spelled cheese. Do your friends know about this. We could start a club.

Your weird be quiet. that was a few days ago. you just don't know how to keep your mouth shut huh?