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# dissociation of ammonium chloride in water

Question:A solution is prepared by dissolving 0.16 mol of acetic acid and 0.16 mol of ammonium chloride in enough water to make 1 L of solution. calculate ph.

Answers:Impossible to calculate. Acetic acid is a weak acid, and ammonium chloride is a weak base. They do not fully dissociate in water, so we cannot determine the amount of hydrogen ions and hydroxide ions present in solution. Thus, neither pH nor pOH can be calculated. It can either be determined experimentally, or by means of literature sources.

Question:Why did I get these wrong?!?! Please correct it. Write equations for the dissociation of the following in water. Include physical states for all species. 1)CaCl2 CaCl2(s) --> Ca2+(aq) + Cl-(aq) 2) (NH4)2SO4 (NH4)2SO4(aq) ---> 2NH4+(aq)+SO4-(aq) 3) NaC2H3O2 NaC2H3O2(aq) ---> Na+(aq) + C2H3O2-(aq) >_< Help

Answers:I can see why you got all these wrong. The correct expressions would be 1) CaCl2 Ca2+ + 2Cl- Since there are 2 Cl atoms in CaCl2, therefore, dissociation of CaCl2 in water will produce 2 Cl- (chloride ions) in solution, which you haven't considered. 2) NH4)2SO4 2NH4+ + SO4 2- The valency of sullphate (SO4 2-) anion is 2 and not 1. 3) N2C2H3O2 is sodium acetate, and can be written as CH3COONa. CH3COONa Na+ + CH3COO- This one was correct.

Question:What is the balanced equation for calcium chloride + acetic acid + ammonium oxalate [with (aq) and (s) and (ppt)]?

Answers:Calcium Chloride(s)+ acetic acid(aq) gives us Calcium Acetate(aq) and Water(l) Further Calcium Acetate(aq) + ammonium oxalate(aq) gives us Calcium Oxalate(s or ppt) and 2*Ammonium Acetate(aq) It is a test for Identifying the presence of Calcium Ion in a given salt

Question:

Answers:Neither acid nor base reacts *directly* with ammonium chloride in water. When NH4Cl is dissolved in water, it dissociates into ions: NH4Cl (s) NH4+(aq) + Cl-(aq) The ammonium ion is a weak acid, meaning it partially and reversibly reacts with water to form a hydronium ion and ammonia, to a stable equilibrium state: NH4+(aq) + H2O H3O+(aq) + NH3 Left to its own, the ammonium chloride will settle on a pH which can be calculated. If acid is added to this NH4Cl solution, all that will be done is that the equilibrium will be forced to the left as it is written here, to form more NH4+. If base is added, the H3O+ will be consumed, and the equilibrium will shift to the right, making more H3O+ and NH3. This equilibrium is the basis for understanding buffer solutions, and how they control pH.