Posted by Sarie on Sunday, September 19, 2010 at 11:32am.
1. Hmmmm. Cannot be determined. Assuming one is acid and one is base, the immediate question is that a mole does not neutralize a mole: one could be di or tri protic. You have to have a balanced equation. Frankly, I like to work with Normal solution on these.
2. Look at your solubility rules, for instance: on the first, all potassium compounds are soluble, but not all mercury: is Mercury(II)sulfate soluble?
Memorize those rules, millions before you have done the same.
Ok, great! Thank you.
Sorry about question 1, I left out the full question. This is it:
What is the molarity of a NaOH solution if 48.0 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of NaOH solution?
2NaOH + H2SO4 --> Na2SO4 + H2O
moles H2SO4 = M x L
moles NaOH = 2x moles H2SO4
Molarity NaOH = moles NaOH/L NaOH.
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