what volume of 0.15 M sodium hydrogen oxalate must be added to 20.00 ml of 0.25 M sodium oxalate to produce a solution with a ph of 4.80?
Sodium hydrogen oxalate = 0.15M
let be the volume of Sodium hydrogen oxalate = V L
number of moles of Sodium hydrogen oxalate = 0.15M x V L = 0.15V mole
Sodium oxalate = 20.00 mL of 0.25M
number of moles of Sodium oxalate = 0.25M x 0.0200L = 0.005 moles
PH = 4.80
Ka2 of hydrogen oxalate = 6.4x10^-5
Ka= 6.4x10^-5
-log(Ka) = -log(6.4x10^-5)
Pka = 4.19
PH = Pka + log[salt/acid]
4.80 = 4.19 + log(0.005 / 0.15V)
0.61 = log( 0.005 /0.15V)
0.005/ 0.15V= 10^0.61
0.005/ 0 15V = 4.074
0.005 = 0.6111V
V= 0.0082
Volume of Sodium hydrogen oxalate = 0.0082L = 8.2 mL
volume of Sodium hydrogen oxalate = 8.2 mL
what volume of 0.15 M sodium hydrogen oxalate must be added to 20.00 ml of 0.25 M sodium oxalate to produce a solution with a ph of 4.80?
what volume of 0.15 M sodium hydrogen oxalate must be added to 20.00 ml of 0.25 M sodium oxalate to produce a solution with a ph of 4.80?
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