After doing the lab these are the givens:
Total mass of empty beaker= 85.000g
After 2g Sodium Carbonate (Na2CO3) added total mass = 87.000g
After adding HCl in 1mL increments from graduated cylinder until bubbling stopped:
Ending volume of HCl in graduated cylider=12.00mL +1=13.00mL (added 1 since the last 1mL caused no effervesence)
Mass of beaker after heating solution and only sodium chloride (NaCl) left = 87.206g
From the above information I have answered the following: (I'm pretty sure A,B,C,D,& E are correct if not please correct)
A. Mass of empty beaker (g) = 85.000g
B. Mass of beaker plus Na2CO3 (g) = 87.000g
C. Mass of Na2CO3 (g) = 2g
D. Mass of beaker plus NaCl (after boiling off the water) (g) = 87.206g
E. Mass of NaCl (d - a) = 87.206g-85.000g=2.206g
From the above information I also need the following answered:
1. Convert the mass of Na2CO3 to moles, given its molecular weight (MW) of 105.989 g/mole.
2. Convert the mass of NaCl to moles, given its molecular weight (MW) of 58.443 g/mole.
3.Calculate the experimentally determined ratio of moles of NaCl produced to moles of Na2CO3 reacted, according to:
mole-ratio = (moles NaCl)/(moles Na2CO3)
4. Use the mole ratio to write a balanced chemical equation for the reaction.
5. What is the theoretical mole ratio according to this balanced equation?
6. Use the theoretical mole ratio to calculate the theoretical yield of NaCl in grams from 2 g of Na2CO3?
7. The "percent yield" is the ratio of the actual amount of a product to the theoretical amount. Calculate the percent yield of NaCl as: % yield = (experimental grams NaCl) / (theoretical grams NaCl) * 100%
8. What was the acid in the reaction?
9. What was the base in the reaction?
This solution offers detailed step-wise calculation to a acid-base titration lab.