Calculate the solubility of barium carbonate, BaCO_3 in water. K_ = 2.0 times 10

Question

Calculate the solubility of barium carbonate, BaCO_3 in water. K_ = 2.0 times 10^-9 ___________________mol/L A 0.350 M aqueous solution of hydrocyanic acid, HCN, is titrated with 0.100 M NaOH (aq) to the endpoint. K_a for HCN is 4.9 times 10^-10. a) List all the species in the solution in order of decreasing concentration prior to the addition of any NaOH(aq). (No calculate should beta needed, and you need not show any work.) b) List all the species in the solution in order of decreasing concentration at the equivalence point. (No calculation should beta needed, and you need not show any work.)Write the solubility product expression, K_ for silver sulfate, Ag_2 SO_4. Write the chemical equation for that reaction that occurs solution of the weak acid HF is titrated with KOH(aq).

Explanation / Answer

1)

BaCO3 -----------------------> Ba+2 + CO3-2

                                              S             S

Ksp = S^2

2.0 x 10^-9 = S^2

S = 4.47 x 10^-5 M

solubility = 4.47 x 10^-5 M

2)

a)

H2O >   HCN > H3O+ > OH-

b) H2O < HCN < H3O+ < OH- < Na+ = CN-

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