3. The laboratory technician accidentally mixed NaHCO3 with BaCl22H2O instead of KCl when preparing unknown mixtures for this experiment. A. How would this mistake affect the calculated percentage of NaHCO3 in the mixture? Justify your answer with an explanation. B. Is it still possible to determine the percentage of NaHCO3 in the mixture given the error made by the lab technician? Justify your answer with an explanation.

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g

colorless gas, exhibiting a blue glow when placed in an electric field

b) solid

its a type of rock