Method
1. Measure ≈25mL of HCl in a 50mL measuring cylinder, and ≈2g of NaHCO 3 in a
250mL beaker.
2. Weigh the HCl and NaHCO3 on the scientific balance to find the mass of the beakers.
3. Conduct the reaction between HCl and NaHCO3 in the 250mL beaker (so the products
don’t overspill during the reaction).
4. Wait for the reaction to finish, and record the mass of the NaCl and H2O by subtracting
the mass of the beakers.
5. Calculate the concentration of HCl.
n(CO2) = m/M = 1..01 ≈ 0.024 mol
n(HCl) = n(CO2) due to 1:1 ratio in the balanced equation
n(HCl) = 0.024 mol
n = cv
n(HCl) = [HCl] x V(HCl) → [HCl] = n(HCl) / V(HCl)
[HCl] = 0.024 / () because it has to be in litres
Therefore, [HCl] = 0.96 mol/L
Discussion
- It is assumed that the density of HCl was 1g/mL, which lowers the validity of the
experiment.
- We had 96% accuracy to the results because the expected result was 1 mol/L (reliability).
- Our measurements were conducted to the most accurate extent excluding human error.
millimetres of mercury mmHg 760 mmHg = 1 atm = 1.013 x 105 Nm-2
torr torr 1 torr = 1 mmHg
- Volume is inversely proportional to pressure, with constant temperature and molar mass
- Volume is proportional to temperature (K = Kelvin), with constant pressure and molar
mass
- Volume is proportional to molar mass, with constant temperature and pressure (see
below “Calculating Gas Volumes”)
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