The following data came from a titration experiment.
A student titrated 10.00 mL samples of Na2SO4 with 0.350 mol/L HBr
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Trail | 1 | 2 | 3 | 4 |
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Final Buret Reading (mL) | 15.2 | 28.9| 42.8 | 14.2 |
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Initial Buret Reading (mL) | 0.6 | 15.2| 28.9 | 0.4 |
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Volume of HBr used (mL)
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1. The average volume of HBr added is ____ mL. (Three Digit Answer)
2. What is the amount concentration of Na(2)SO(4) (aq)? Show your work.
Any help would be greatly appreciated im sorry for the chart looking messed up it was the best I could do given the parameters!
For Trail it's meant to be a column so 1 would be above 15.2 and 0.6 and then 2 above 28.9 and 15.2 etc...
The volume used in the titration is
Final reading - initial reading = volume of titration.
After you have done this for each trial then take the average. I assume you know how to do that. It's
(vol #1 + vol #2 + vol #3 + vol #4)/4 = ?
You need to tell me more about the titration for me to help calculate concn Na2SO4.
To find the average volume of HBr added, you need to calculate the sum of all the volumes used and divide it by the number of trials.
1. Calculate the sum of the volumes used:
Volume of HBr used in Trial 1 = Final Buret Reading (15.2 mL) - Initial Buret Reading (0.6 mL) = 14.6 mL
Volume of HBr used in Trial 2 = Final Buret Reading (28.9 mL) - Initial Buret Reading (15.2 mL) = 13.7 mL
Volume of HBr used in Trial 3 = Final Buret Reading (42.8 mL) - Initial Buret Reading (28.9 mL) = 13.9 mL
Volume of HBr used in Trial 4 = Final Buret Reading (14.2 mL) - Initial Buret Reading (0.4 mL) = 13.8 mL
Sum of volumes used = 14.6 mL + 13.7 mL + 13.9 mL + 13.8 mL = 56.0 mL
2. Calculate the average volume of HBr added:
Average volume of HBr added = Sum of volumes used (56.0 mL) / Number of trials (4) = 14.0 mL
So, the average volume of HBr added is 14.0 mL.
To find the amount concentration of Na2SO4 (aq), you can use the balanced chemical equation for the reaction between Na2SO4 and HBr:
Na2SO4 + 2HBr -> 2NaBr + H2SO4
In this reaction, the mole ratio between Na2SO4 and HBr is 1:2. Since HBr has a known concentration of 0.350 mol/L, you can use the volume of HBr and the mole ratio to calculate the concentration of Na2SO4.
3. Calculate the moles of HBr used:
Moles of HBr = Volume of HBr used (14.0 mL) * Concentration of HBr (0.350 mol/L) / 1000 mL/L = 0.0049 mol
4. Calculate the moles of Na2SO4:
From the balanced chemical equation, the mole ratio between Na2SO4 and HBr is 1:2. This means that for every 2 moles of HBr, 1 mole of Na2SO4 is reacted.
Moles of Na2SO4 = Moles of HBr / 2 = 0.0049 mol / 2 = 0.00245 mol
5. Calculate the amount concentration of Na2SO4:
Amount concentration of Na2SO4 = Moles of Na2SO4 / Volume of Na2SO4 (in liters)
We know that the volume of Na2SO4 is 10.00 mL = 0.01000 L
Amount concentration of Na2SO4 = 0.00245 mol / 0.01000 L = 0.245 mol/L
So, the amount concentration of Na2SO4(aq) is 0.245 mol/L.