The solubility of silver oxalate, Ag_2C_2O_4, in pure water is 2.06 times 10^-4

Question

The solubility of silver oxalate, Ag_2C_2O_4, in pure water is 2.06 times 10^-4 M (mol/L). Calculate the value of K_sp for silver oxalate from this data. a) 4.24 times 10^-8 b) 8.49 times 10^-8 c) 1.75 times 10^-11 d) 3.50 times 10^-11 A buffer solution is prepared by taking 0.250 moles of CH_3COOH, acetic acid, (pKa = 4.74) and 0.400 moles of Na(CH_3COO), sodium acetate, in sufficient water to make 1.800 liters of solution. Calculate the pH. a) 0.204 b) 4.94 c 4.54 d) 0.37 e) 5.11 Given the following system: 2Cro^2-_4(aq) + 2H^+(aq) CrO^2-_7 (aq) + H_2O(I) Which of the following chemicals, when added to the above system at equilibrium, would result a decrease in [Cr_2O^1-_)7]? a) NaOH b) HNO_3 c) Na_2CrO_4 d) Na_2Cr_2O_7

Explanation / Answer

Q15

Ag2C2O4 <--> 2Ag+ + C2O4-2

Ksp = [Ag+]^2 [C2O4-2]

find [Ag+] and [C2O4-2]

[Ag+] = 2*Ag2C2O4 = 2*2.06*10^-4 = 0.000412 M

[C2O4-2] = 1*Ag2C2O4 = 2.06*10^-4 = 0.000206 M

Ksp =(0.000412 ^2)(0.000206 )

Ksp = 3.496726*10^-11

choose D

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