what will happen to the chemical equilibrium of nh4cl is added to this solution
Could you lot please check that I responded correctly to the questions...
Could you please bank check that I responded correctly to the questions regarding Equilibrium and Le Chatelier'southward Principle. Thank you.
Organization I
Saturated solution of ammonium chloride:
NH4Cl(s) ↔ NH4+(aq) + Cl-(aq)
(a) Predict what will happen if HCl solution is added to the test tube.
When the full-bodied HCL solution is added to the saturated solution of ammonium chloride, information technology was observed that NH4Cl formed due to ion consequence based on Le Chatelier'south Principle.
(b) Bank check your predication . Was your predication correct ?
NH4Cl(s)<--->NH4Cl+(aq) +Cl-(aq)
HCL(aq)----> H+(aq) + Cl-(aq)
HCl disassociates which increases the Cl- ion concentration causing the equilibrium to shift backwards and NH4Cl is the precipitate.
(c) Predict what will happen if oestrus is added to the contents of the test tube in step 3.
When heat is practical to the test tube, the NH4Cl dissolves and the NH4Cl precipitate evaporates.
(d) Check your prediction.
NH4Cl(s)<--->NH+(aq)+Cl-(aq)
The chemical reaction moves forward due to the addition of rut and shifts backward due to the HCL ion effect. The forward reaction is endothermic and the astern reaction is exothermic.
System II
Methyl violet indicator solution:
HMV(aq)-yellow ↔ H+(aq) + MV-(aq)-violet
(a) Predict what will happen if HCl solution is added to the reaction system.
When the acidic HCl solution is added, the H+ ions react with the MV- anions to produce HMV which shifts the equilibrium to the left and the solution will turn yellow.
(b) Bank check your prediction.
HMV(aq)-yellow <----->H+(aq)+MV-(aq)-violet
As in that location is an backlog of HMV (aq), the equilibrium shifts back to the left and the solution turns yellow.
(c) Predict what volition happen if NaOH solution is added to the reaction arrangement.
Adding NaOH to the solution, the H+ ions will combine with the OH- ions and subtract the concentration. The equilibrium will shift to the right and decrease the reaction. To keep the equilibrium, HMV will dissociate and produce more MV- and the solution will turn violet.
(d). Bank check your prediction.
More MV-(aq)-violet is produced then the solution became darker.
(e) Now predict what will happen if NaOH solution is added to the well y'all already used to a higher place in step #10.
If the excess NaOH is added then it volition react with the HMV to form a circuitous which is colorless. The solution will become articulate.
System Iii
Cobalt(Ii) complex ion solution:
[CoCl4]-ii(aq) + 6H2O(l) ↔ [Co(H2O)six]+2(aq) + 4Cl-(aq)
blue pink
(a) Predict what will happen if HCl solution is added to the reaction system.
If HCl is added, the Cl- is reduced and the equilibrium volition shift to the right and the solution volition turn blueish co-ordinate to Le Chatelier'due south Principle.
(b) Check your prediction.
Cl- is reduced and the solution volition plough blue.
(c) Predict what will happen if water is added to the well used in step #17.
The solution volition plow pink apace upon the add-on of H2O.
(d) Check your prediction..
With the addition of H2o, the blue solution becomes less full-bodied shifting the equilibrium and changing colour of the solution to pinkish.
System Iv
Acetic acid solution with bromocresol green indicator:
CH3COOH(aq) ↔ CH3COO-(aq) + H3O+(aq)
(a) Predict what will happen if solid sodium acetate (CH3COONa) is added to the reaction system.
When solid sodium acetate is added, it will react with H3O+ ions thus moving the equilibrium to the left per Le Chatelier's Principle. The solution volition be green.
(b) Cheque your prediction.
Every bit the H3O+ ion concentration decreases equally it reacts to the sodium acetate, the pH will increase/become less acidic giving the solution a green color.
(c) Predict what will happen if NaOH solution is added to the reaction system.
The sodium acetate will react with the NaOH until all of the acetate is neutralized as the H+ ion concentration decreases. The pH will non significantly modify.
(d) Check your prediction.
Since the buffer was used, the pH did not increase significantly which will plough the solution less dark-green to blue.
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