The solubility of silver oxalate, Ag_2C_2O_4, in pure water is 2.06 times 10^-4
ID: 527069 • Letter: T
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_4^2- (aq) + 2H^+ (aq) Cr_2O_7^2- (aq) + H_2O(I) Which of the following chemicals, when added to the above system at equilibrium, would result in a decrease in [Cr_2O_7^2-]? a) NaOH b) HNO_3 c) Na_2CrO_4 d) Na_2Cr_2O_7 Which of the following processes have a Delta S > 0? a) CH_3OH (1) rightarrow CH_3OH(s) b) N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) c) CH_4(g) + H_2O(g) rightarrow CO(g) + 3 H_2(g) d) Na_2CO_3 (s) + H_2O(g) + CO_2 (g) rightarrow 2 NaHCO_3(s) e) All of the above processes have a Delta S > 0.Explanation / Answer
17.The answer for this is option D.
This can be explained by using Le Chatlier's principle.
According to this when a system at equilibrium is subjected to a change in pressure or temperature or concentration then the equilibrium will shift in such a direction that it nullifies the change.
In order to reduce the amount of product that is Cr2O7-2, that is the equilibrium should shift towards left then we must add Cr2O7-2 that is N2Cr2O7 at equilibrium.
Due to the increase in concentration of Cr2O7-2 on right side equilibrium will shift towards left.