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Chemistry chemistry concerning moles?
I got this question wrong on an exam and I need clarification as to why I got it wrong.
A student spilled 100.0 ml of 6.00M HCL (aq) on the work bench and tried to neutralize it with 0.125 L of 4.00M NaHCO3 (aq).
Will that be enough to get rid of all the acid? Why or why not?
As for my calculations, I did (6M HCL/100 mL) * (1000 mL/1 L) to find the molarity of HCL.
I did (4M NaHCO3/.125 L) * 1 L to find the molarity of NaHCO3.
In the end, my explanation was that even though the student is using more volume to clean up the HCL spill, it contains a smaller molarity than the 100 mL of 6.00 M HCL, so it would not be enough to get rid of the acid.
Any answer is appreciated.
1 Answer
- Simonizer1218Lv 78 years agoFavorite Answer
moles of HCl = 0.1 L x 6 mol/L = 0.6 moles HCl
moles NaHCO3 = 0.125 L x 4 mol/L = 0.5 moles NaHCO3
According to the balanced equation of HCl + NaHCO3 --> NaCl + CO2 + H2O it takes 1 moles NaHCO3 to neutralize 1 moles HCl. You don't have enough NaHCO3 (0.5 moles) to neutralize all HCl (0.6 moles).
NOTE: It is the number of MOLES and not the MOLARITY that matters. In your answer, you use the term molarity, which is incorrect.
