Silver oxalate, Ag_2C_2O_4, is slightly soluble in water. The silver ion concent

Question

Silver oxalate, Ag_2C_2O_4, is slightly soluble in water. The silver ion concentration in a saturated solution is 2.2 times 10^-4 M. what is the K_a of Ag_2C_2O_4? 1.1 times 10^-4 2.4 times 10^-8 1.1 times 10^-11 5.3 times 106-12 1.3 times 10^-12 At the boiling point of benzene, C_6H_6, delta H_ = 30.78 kJ/mol and delta S_ = 87.15 J/(mol middot K). Determine the normal boiling temperature in degrees Kelvin for C_4H_4. 353 K 392 K 486 K 546 K 626 K For which of the following systems at equilibrium and at constant temperature will decreasing the volume cause the equilibrium to shift to the right? N_2(g) + 3H_2(g) equilibrium 2NH_3(g) 2H_2O(g) equilibrium 2H_2(g) + O_2(g) 2NO_2(g) equilibrium 2NO(g) + O_2(g) NH_4Cl(s) equilibrium NH_3(g) + HCI(g) H_2(g) + Cl_2(g) equilibrium 2HCI(g) The reaction C(s) + CO_2(g) rightarrow 2CO(g) is spontaneous only at temperatures in excess of 1100 K. We can conclude that delta H degree is positive and delta S degree is negative. delta H degree is negative and delta S degree is negative. delta H degree is positive and delta S degree is positive. delta H degree is negative and delta S degree is positive. delta G degree is negative for all temperatures. A weak base is titrated with hydrochloric acid solution. At the equivalence point, pH 7.0. pH = pK_a. the maximum buffering capacity is achieved. In the voltaic cell that is represented as Ni/Ni^2+ || (Pt) Fe^3+/Fe^2+ the electron flow will be from Pt to Ni^2+. Pt to Ni. Fe^2+ to Ni^2+. Ni^2+ to Fe^2+. Ni to Fe^3+.

Explanation / Answer

Q19

[Ag+] = 2.2*10^-4

then

[C2O4-2] = 1/2*2.2*10^-4 = 1.1*10^-4

so

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

Ksp = (2.2*10^-4)^2(1.1*10^-4) = 5.32*10^-12

choose D

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