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Lena772
 one year ago
Calculate the following values for a 1.25 L solution that is 0.002915 M NaOH.
Lena772
 one year ago
Calculate the following values for a 1.25 L solution that is 0.002915 M NaOH.

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Lena772
 one year ago
Best ResponseYou've already chosen the best response.0Is it NaOH+H2O> OH + Na+ + H2O? or NaOH + H2O> H3O+ + NaO

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0First identify whether or not NaOH is a strong electrolyte. If it is, then we can assume that it completely dissociates, that is, any ion produced is equal to the concentration of the whole compound. If it's a weak electrolyte, then you have use an equilibrium expression. Next write the dissociation equation for NaOH

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0it's \(\sf NaOH\rightarrow Na^++OH^\)

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0Its strong, but I tried 0 for H3O+ and that was wrong.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0it can't be 0 for \([H_3O^+]\), it will just be very small

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0When I calculate X, that's what I get

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0Use the relations: \(\sf pOH=log[OH^]\) \(\sf pH=log[H_3O^+]\) \(\sf pH+pOH=14\) \(\sf [OH^][H_3O^+]=K_w=1.0*10^{14}\)

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0Yes but my Ka chart says the Kb of OH is 1*10^14

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0Based on that, H3O+ and pH should be 0, but it isn't. :/

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0the Kb of NaOH is very very large, so that's not right

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0no the Kb is like in the billions, which means it's a strong (electrolyte) base, it dissociates to essentially 100% therefore \(\sf [OH^]=[NaOH]\)

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0So log(0.002915) = OH? I can do the rest from there.

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0So is H3O+ 3.47e12? Is that small enough?

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0I got pH and pOH right but when I take 10^(pOH) and 10^(pH), and those are wrong so idk...

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0It's asking for the concentrations at equilibrium but idk if that makes a difference @aaronq

aaronq
 one year ago
Best ResponseYou've already chosen the best response.0what did you get wrong?
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