We can solve this problem by employing the ideal gas law.

PV = nRT

where

P = pressure (atm) = 1.000 atm

V = volume (L) = (86.44mL/1000mL)L

n = number of moles = ?

R = gas constant, 0.08206 atm-L/mol/K

T = temperature (in Kelvin) = 25.00 + 273.15 = 298.15K

n = PV/RT = (1.00*0.08644)/(0.08206*298.15)

= 0.003522 moles CO2

Ca(HCO3)2 ---> Ca(OH)2 + 2CO2

There are 2 moles of CO2 per one mole of Ca(HCO3)2 so,

0.003522 moles CO2 x ( 1 mole Ca(HCO3)2 / 2 moles CO2)

= 0.0017665moles Ca(HCO3)2

remember that n = mass/ molar mass

so, mass Ca(HCO3)2= n* molar mass

mass Ca(HCO3)2 = 0.0017665 * 162.11464 g/mol

= 0.28638 g Ca(HCO3)2

percent active ingredient = 0.28638/0.406 x100

=** 70.5% active ingredient**

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