Calculate the ph of a water at 25°c that contains 0.75mg/l of carbonic acid. assume that [h+] = [hco3-] at equilibrium and neglect the dissociation of water. (note: pkafor h2co3is 6.35. assume there is no further dissociation of hco3-)

pH = 5.675

Explanation:

H2CO3 ↔ H3O+  +  HCO3-

∴ C H2CO3 = 0.75 mg/L * ( g / 1000 mg ) * ( mol / 62.03 g ) = 1.209 E-5 M

∴ Ka = ( [ HCO3- ] * [ H3O+ ] ) / [ H2CO3 ]

∴ pKa = 6.35 = - Log ka

⇒ Ka = 4.467 E-7 = ( [ HCO3- ] * [ H3O+ ] ) / [ H2CO3 ]

assuming that the dissociation of HCO3- is not signicant, we have:

mass balance:

C H2CO3 = [ H2CO3 ] + [ HCO3- ] = 1.209 E-5

charge balance:

⇒[ H3O+ ] = [ HCO3- ] assumption given for equilibrium

⇒ 1.209 E-5 - [ H3O+ ] = [ H2CO3 ]

replacing in Ka:

⇒ 4.467 E-7 * ( 1.209 E-5 - [ H3O+ ] ) = [ H3O+ ]²

⇒ 5.401 E-12 - 4.467 E-7 [ H3O+ ] = [ H3O+ ]²

⇒ [ H3O+ ]² + 4.467 E-7 [ H3O+ ] - 5.401 E-12 = 0

⇒ [ H3O+ ] = 2.111 E-6 M

⇒ pH = - Log [ H3O+]

⇒ pH = 5.675

2b2t

explanation:

2b2t