muhali3 Posted February 27, 2005 Share Posted February 27, 2005 Is this reaction balanced and correct? NaHCO3 + HCl -------- NaCl + H2CO3 Link to comment Share on other sites More sharing options...
budullewraagh Posted February 27, 2005 Share Posted February 27, 2005 nope. NaHCO3+HCl -->NaCl+CO2+H2O Link to comment Share on other sites More sharing options...
Guest Pavel Posted February 27, 2005 Share Posted February 27, 2005 muhali3 you are correct, just know that carbonic acid (H2CO3) decomposes into water and carbon dioxide. Link to comment Share on other sites More sharing options...
budullewraagh Posted February 27, 2005 Share Posted February 27, 2005 the carbonic acid is an intermediate of the reaction, so it's not actually a product Link to comment Share on other sites More sharing options...
Silencer Posted February 28, 2005 Share Posted February 28, 2005 Also, if your teacher is a stickler for putting the state of the chemicals, don't forget that. Link to comment Share on other sites More sharing options...
muhali3 Posted February 28, 2005 Author Share Posted February 28, 2005 Thanks for your help. Btw, is carbonic acid able to exist without decomposing. Link to comment Share on other sites More sharing options...
jdurg Posted February 28, 2005 Share Posted February 28, 2005 Thanks for your help. Btw, is carbonic acid able to exist without decomposing. Yes. Link to comment Share on other sites More sharing options...
budullewraagh Posted February 28, 2005 Share Posted February 28, 2005 carbonates and bicarbonates decompose in acids Link to comment Share on other sites More sharing options...
muhali3 Posted February 28, 2005 Author Share Posted February 28, 2005 Thanks, but i still have to annoy you guys a little more. sorry. Could anyone tell me or link me to an explanation on how to find out theoretical yield, excess reactant, and limiting reactant for the reaction? i googled it but i didn't get anything good. sry for my botheration (if that is a word). Link to comment Share on other sites More sharing options...
muhali3 Posted February 28, 2005 Author Share Posted February 28, 2005 Nevermind..i already found out how to do it. Thanks for everyones help. I realized i should've posted this in the homework thread but w/e. Link to comment Share on other sites More sharing options...
budullewraagh Posted February 28, 2005 Share Posted February 28, 2005 no worries. glad to be of service Link to comment Share on other sites More sharing options...
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