Question

the crc handbook of chemistry and physics gives the solubility of carbon dioxide (coming from NaHCO3) in water at 25 degrees celsius as 0.145g in 100ml. assuming that the solubility of carbon dioxide is the same in the acetic acid solution as in water, how much carbon dioxide (in ml of gas at 25 degrees celsius and 1atm) might be dissolved in the 4ml used for each reaction

Answer 1

Solution :-

Solubility of the CO2 is 0.145 g / 100 ml

Therefore in 4 ml solution amount of the CO2 that can be soluble is calculated as

4 ml * 0.145 g / 100 ml = 0.0058 g

Now lets calculate the moles of the CO2

Moles of CO2 = 0.0058 g / 44.01 g per mol = 0.000132 mol

Now lets calculate the volume of the CO2 gas at the given conditions

T = 25 C +273 = 298 K

PV= nRT

V= nRT/P

= 0.000132 mol * 0.08206 L atm per mol K * 298 K / 1 atm

= 0.00322 L

0.00322 L * 1000 ml / 1 L = 3.22 ml

So in the 4 ml solution volume of the CO2 3.22 ml CO2

For per ml of the solution amount of the CO2 that can be soluble = 3.22 / 4 ml = 0.805 ml CO2