Hi,
Sorry for the barrage of questions lately....but I am confused about one thing on this acid neutralization problem. It says that a 2.50-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25-mL of 0.798 M HCl. Some acid remains after treatment of the sample. The thing I don't get is how there is some acid that remains after the treatments are placed together. Here is the equation for the reaction and the molar concentrations for the ICE chart(I left out Nacl since that really doesn't appear to contribute to anything)
Na2CO3(s) + 2HCl(aq) => 2NaCl(aq) + H2O + CO2
2.3x10^-2 mol 2x10^-2 mol 0 0 0
-1x10^-2 mol -2x10^-2 mol +2x10^-2 mol for all 3 products
1.3x10^-2 mol 0 mol 2x10^-2 mol for all 3 products
All the HCl appears to be used up, and there is no more acidic species. I don't see how this solution can still be acidic. Thanks so much. Any input would be great.
Ryan