Calculate the ph of a solution prepared by mixing 40.0 ml of a 0.02 m hcl solution with 200.0 ml of 0.20 m hcn solution. assume volumes to be additive ka for hcn=1.0x10^-10

Question

Kenna

Chemistry

24 November, 02:31

Calculate the ph of a solution prepared by mixing 40.0 ml of a 0.02 m hcl solution with 200.0 ml of 0.20 m hcn solution. assume volumes to be additive ka for hcn=1.0x10^-10

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Cheeky · Answer 1

First, we have to get moles of each HCl & HCN

moles of HCl = volume * molarity

= 0.04 L * 0.02 M = 0.0008 moles

moles of HCN = volume * molarity

= 0.2 L * 0.2 M = 0.04moles

∴Total moles = 0.04 + 0.0008 = 0.0408 moles

and the total volume = 0.04 L + 0.2 L = 0.24 L

∴the total concentration = total moles / total volume

= 0.0408 moles / 0.24 L

= 0.17 M

when we assume [H+] = X

∴ Ka = X^2 / (0.17-X)

by substitution

∴ 1 x 10^-10 = X^2 / (0.17 - X)

∴X = 4.12 x 10^-6

∴[H+] = 4.12 x 10^-6

∴PH = - ㏒ (4.12 x 10^-6)

= 5.4