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18 Nov 2019
Suppose 1 mL of 0.010 M AgNO_3 is mixed with 1 mL of 6 M HCI. Show that precipitation should occur. Answer question la substituting a 0.010 M solution of Pb(NO_3)_2 in place of the AgNO_3. K_sp (PbCI_2) = 1.6 times 10^-5. 6 M NH_3 is added to a Ni(OH)_2 precipitate so that some of the precipitate dissolves according to the equation: Ni(OH_2)(s) + 6 NH_3(aq) Ni(NH_3)_6^2+(aq) + 2OH^-(aq) What does the NH_3 concentration need to be at equilibrium in order to dissolve enough nickel(II) hydroxide such that there is 0.10 M Ni(NH_3)_6^2+ in solution? K_sp (Ni(OH)_2) = 5.5 times 10^-16: K_f(Ni(NH_3)_6^2+) = 5.6 times 10^8.
Suppose 1 mL of 0.010 M AgNO_3 is mixed with 1 mL of 6 M HCI. Show that precipitation should occur. Answer question la substituting a 0.010 M solution of Pb(NO_3)_2 in place of the AgNO_3. K_sp (PbCI_2) = 1.6 times 10^-5. 6 M NH_3 is added to a Ni(OH)_2 precipitate so that some of the precipitate dissolves according to the equation: Ni(OH_2)(s) + 6 NH_3(aq) Ni(NH_3)_6^2+(aq) + 2OH^-(aq) What does the NH_3 concentration need to be at equilibrium in order to dissolve enough nickel(II) hydroxide such that there is 0.10 M Ni(NH_3)_6^2+ in solution? K_sp (Ni(OH)_2) = 5.5 times 10^-16: K_f(Ni(NH_3)_6^2+) = 5.6 times 10^8.
Deanna HettingerLv2
4 Jun 2019