Bicarbonate Determination

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12 Terms

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K =

C + 273.15

2
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Barometric pressure units

mmHg

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mL —> L

/1000

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Vapor pressure of water (mmHg)

Found from barometric pressure

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Ex. Pressure of dry CO2

  1. barometric pressure mmHg - vapor pressure of water mmHg

  2. x (1 atm / 760 mmHg)

  3. final units = atm

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R =

0.0821 atm x L / mol x K

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Moles =

(PV)/(RT)

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Ex. Grams of NaHCO3 in ¼ tablet

Moles of CO2 —> grams of NaHCO3

  • moles of CO2 x stoichimetric relationship (1:1)

  • x molar mass of NaHCO3

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Ex. mass % of NaHCO3 in ¼ tablet

grams of NaHCO3 in ¼ tablet / mass of ¼ tablet (taken initially)

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Theoretical mass %

Given to you

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% error 

theoretical mass % - mass % / theoretical mass % x 100 

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Ideal gas law

PV = nRT