1. A 427- mL sample of unknown HCl solution reacts completely with Na2CO3 to form 10.1 g CO2 . What was the concentration of the HCl solution?

Question

1a) What mass of silver chloride can be produced from 1.07 LL of a 0.194 MM solution of silver nitrate?

1b) The reaction described in Part A required 3.12 LL of sodium chloride. What is the concentration of this sodium chloride solution?

Express the molar concentration numerically.

Answer 1

The balanced equation: 2HCl + Na₂CO₃ --------> 2NaCl + CO₂ + H₂O

The following conversion factor can be used to calculate the number of moles of HCl reacted.

2 moles HCl / Molecular mass of CO₂ = 2 moles HCL / 44 g CO₂ = 0.0455 moles HCl / gm CO₂.

To determine the number of moles of HCl used, multiply 0.0455 moles HCl / gm CO₂ x 10.1 g CO₂ = 0.46 moles HCl used.

Since 0.46 moles HCl was in 427 mL of solution, the molar concentration of HCl is

0.46 moles / 427 mLx 1000 mL/L = 1.08 molar.

Try the other parts of the question using the same approach. Check my math.