Question

A student plans to neutralize a 10.00 mL sample of 2.00 M HCl with sodium carbonate. Consider sig. figs. for all answers.

A. Balance the following equation that signifies the above reaction:

Na₂CO₃ + HCl -> NaCl +  H₂O + CO₂

B. Calculate the number of moles of HCl involved in the reaction

C. Calculate the number of moles of Na₂CO₃ required to neutralize the moles of HCl found in (b)

D. Calculate the mass (in grams) of Na₂CO₃ required to react completely with 10.00mL of 2.00M HCl.

Answer 1

A)
balanced equation :

Na₂CO₃ + 2 HCl --------------------------> 2 NaCl +  H₂O + CO₂

B)

moles of HCl = 10 x 2 / 1000 = 0.02

C)

1 mol Na2CO3 ------------------------> 2 mol HCl

x mol Na2CO3 -----------------------> 0.02 mol HCl

moles of Na2CO2 = 1 x 0.02 / 2 = 0.01

moles of Na2CO3 = 0.01

C)

mass of Na2CO3 = moles x molar mass

                          = 0.01 x 106

                         = 1.06 g