I did some homework, but the tutor didn't look it. It was mainly the moles/concentration/volume bit I wasn't sure on, so I thought I'd ask here to see if I got it right or not. Also, may as well throw in my balanced equation. Did I get the state symbols right too?
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Write a balanced chemical equation for the reaction between sodium carbonate and hydrochloric acids. Show the state symbols.
Na2CO3(aq) + 2HCl(aq) -> 2NaCl(aq) + H2O(l) + CO2(g)
What threw me off was whether to include water with the reactants, since sodium carbonate is mixed with distilled water first.
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The moles bit, at first I think I overcomplicated it by trying to work out a concentration within a concentration, so then I redid it in a simpler, more exam-y method with the old belief that if the working out is complicated, I'm doing it wrong. So:
Calculate the moles of 23.8cm^3 sodium carbonate at concentration 0.15mol/dm^3
moles (n) = concentration (c) x volume (v) = 0.15 x (23.8/1000) = 0.850mol (to 3 S.F.)
Using this calculation and your balanced equation, calculate the number of moles of hydrochloric acid that were required to neutralize the sodium carbonate solution.
Ratio of Na2CO3 to HCL is 1:2, so moles of hydrochloric acid = 0.850 x 2 = 1.7mol
Based on this, calculate the concentration of the 25cm^3 of hydrochloric acid solution in mol/dm^3.
c = n/v = 1.7/(25/1000) = 68mol/dm^3
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Did I do good?