Hello Smogon, I'm not sure of how to work out a problem for my chemistry course and since there's plenty of smart people here, I thought I'd ask you.
One of the "active" ingediants in Alka-Seltzer is sodium bicarbonate, NaHC(O3). A student analyzes an Aka-Seltzer tablet to determine the % by mass of NaHC(O3) present in the sample. A 0.500 gram tablet was powdered and mixed with 50.00 ml of .200 M HCL (aq). This reaction mixture was allowed to proceed until all the available sodium bicarbonate had reacted.
Reaction 1) NaHCO3(aq) + HCL(aq) --> NaCl(aq) + H2O(l) + CO2(g)
Not all of the hydrochloric acid reacted and the amount of excess HCL(aq) was determined by titration with sodium hydroxide solution to a phenolphthalein end point. This "back-titration" required 47.5 mls of .125 M NaOH (aq)
Titration reaction: HCL(aq) + NaOH(aq) --> NaCl(aq) + H2O(l)
Based on this data, determine the mass percent of sodium Bicarbonate in the original Alka-Seltzer sample.
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This is what I did, but i'm not sure if i'm right since i've never seen a titration problem like this.
Thanks for your time/help.
One of the "active" ingediants in Alka-Seltzer is sodium bicarbonate, NaHC(O3). A student analyzes an Aka-Seltzer tablet to determine the % by mass of NaHC(O3) present in the sample. A 0.500 gram tablet was powdered and mixed with 50.00 ml of .200 M HCL (aq). This reaction mixture was allowed to proceed until all the available sodium bicarbonate had reacted.
Reaction 1) NaHCO3(aq) + HCL(aq) --> NaCl(aq) + H2O(l) + CO2(g)
Not all of the hydrochloric acid reacted and the amount of excess HCL(aq) was determined by titration with sodium hydroxide solution to a phenolphthalein end point. This "back-titration" required 47.5 mls of .125 M NaOH (aq)
Titration reaction: HCL(aq) + NaOH(aq) --> NaCl(aq) + H2O(l)
Based on this data, determine the mass percent of sodium Bicarbonate in the original Alka-Seltzer sample.
_________________________________________________________________
This is what I did, but i'm not sure if i'm right since i've never seen a titration problem like this.
.125M = [x/.0475 l]
x = .005937 mol NaOH
.005937 mol NaOH(1 mol/84 g. per mol.) = .49875 g NaHCO3
(The above step is where i'm pretty sure i'm wrong. My thought process was that since the mole to mole ratio of HCL to NaHCO3 is the same in both equations, that it would be right?)
.49875g/.5g = 99.75% ???
x = .005937 mol NaOH
.005937 mol NaOH(1 mol/84 g. per mol.) = .49875 g NaHCO3
(The above step is where i'm pretty sure i'm wrong. My thought process was that since the mole to mole ratio of HCL to NaHCO3 is the same in both equations, that it would be right?)
.49875g/.5g = 99.75% ???
Thanks for your time/help.