The formation constant* of
Warning! Long Answer. The equilibrium concentration of
The balanced equation is
#"M"^"2+" + "6CN"^"-" ⇌ "M(CN)"_6^"4+"; K_text(f) = 2.50 × 10^17#
We can set up an ICE table.
This result looks rather unpromising. We must solve a seventh-order polynomial.
However, the value of
Thus, 0.150 mol of
We can approach the equilibrium from the other end. Let's assume that the reaction goes to completion and write the equilibrium in reverse.
#"M(CN)"_6^"4+" ⇌"M"^"2+" + "6CN"^"-"#
Then,
Our new ice table becomes
Check for negligibility
Then,
Check:
It checks!
The formation constant* of [M(CN) 6 ]4− is 2.50 × 10 17 , where M is a generic metal. A 0.140 mole quantity of M(NO3)2 is added to a liter of 1.210 M NaCN solution. What is the concentration of M2+ ions at equilibrium?
The formation constant* of [M(CN)6]4– is 2.50 × 1017, where M is a generic metal. A 0.170-mole quantity of M(NO3)2 is added to a liter of 1.41 M NaCN solution. What is the concentration of M2 ions at equilibrium?
The formation constant of M(CN)614-is 2.50 x 10'7, where M is a generic metal. A 0.130 mole quantity of M(NO3)2 is added to a liter of 1.010 M NaCN solution. What is the concentration of M2+ ions at equilibrium? [M²+] = 3.513 x10-14
The formation constant* of [M(CN) 4 ]2− is 7.70×1016 , where M is a generic metal. A 0.130 mole quantity of M(NO3)2 is added to a liter of 0.870 M NaCN solution. What is the concentration of M2+ ions at equilibrium?
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A 0.170-mole quantity of M(NO3) is added to a liter of 0.540 M NaCN solution. What is the concentration of M ions at equilibrium?
The formation constant* of [M(CN)2]-is 5.30 x 1018, where M is a generic metal. A 0.170 mole quantity of M(NO3) is added to a liter of 0.650 M NaCN solution. What is the concentration of M+ ions at equilibrium? [M2+] =
The formation constant of M(CN),1'-is 2.50 x 101, where M is a generic metal A 0.130 wole quantity of M(NO3)> is alled to a liter of' 1.010 M NaCN solution. What is the concentration of Mº ions at equilibrium? M? 1- 3.513 x10-14
can someone please help me answer these, for some reason theh are both wrong and i cant get them right, will rate you good if you can help get both correct answers! thanks The formation constant of M(CN)61 is 2.50 x 10'7, where M is a generic metal. A 0.130 mole quantity of M(NO3) is added to a liter of 1.180 M NaCN solution. What is the concentration of M2+ ions at equilibrium? [M ] = 4.6 x10-19 The generic...
A 0.180 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Ni?+ ions at equilibrium? Assume the formation constant of Ni(NH)2+ is 5.5 x 10
A 0.170 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Nia + ions at equilibrium? Assume the formation constant of Ni(NH)2+ is 5.5 x 10%.