(Please-urgent) what is the molar concentration of solution having dissolved .1moles of (potassium nitrate) in enough water to prepare 400ml of the solution? i got .25molar = supposedly wrong...

Question

anonymous · Answer

i used the equation Molarity of solution=moles of solute/ liters of solution.. right?

espex · Answer

That is the right formula, just looking over units.

anonymous · Answer

another question (on my exam review) stated acid-base neutralizations were reactions of "h+ ions with o2gas"... that cant be right.. its gotta be a typeo cause i know acid base neutralizations are "h+ with oh- to form h2o.. right?

espex · Answer

Well, acid base reactions give up h or strip off h depending on the direction.

anonymous · Answer

so (h with o2) would be right, whereas (h with oh) would be wrong?

espex · Answer

Well if you were producing a base of hcl for example, the Hydrogen would come off as a H+ ion and mix with the Oxygen in the air, which is a diatomic molecule.

espex · Answer

Looking at your original question, unless I am missing something, I cannot see why .25 was incorrect.

anonymous · Answer

but were talking about aquious reactions, so there is no o2 involved, at least thats what i think. would the first or the second answer be correct? it was a multiple choice

rogue · Answer

O2 gas? Where does that from from? Acid-base neutralization involves the reaction of H+ and OH- not H+ and O2. For example, lets look at the net ionic reaction for the neutralization of hydrochloric acid by sodium hydroxide.
$$HCl + NaOH \rightarrow NaCl + H_2O$$$$H^+ + Cl^- + Na^+ + OH^- \rightarrow Na^+ + Cl^- + H_2O$$$$H^+ + OH^- \rightarrow H_2O$$A general acid-base neutralization reaction goes by$$Acid + Base \rightarrow Ionic Salt + water$$

anonymous · Answer

^thank you. i knew i wasnt crazy

rogue · Answer

;D Trust your instincts.