Scott prepares a solution which contains a large excess of iron and a small amount of thiocyanate. He notices a faint orange color appear in the solution once mixed. He repeats this process with a higher concentration of thiocyanate and notices a deepening of the orange color in the solution once mixed. Explain what has happened to the equilibrium in this case. Has the value of Keq changed? Explain.

To 200 ml of a solution containing 0.002 mol of aluminium chloride and 0.001 mol of calcium chloride is slowly added solid sodium phosphate (assuming no change in volume). How many grams of sodium phosphate must be added to precipitate as much of one ion as possible, while the other ion just doesn't precipitate? What percentage of the ion that will precipitate first is left in the solution at that moment?

Consider a pale blue solution of CuSO4. Include phases in the balanced chemical equations. When a strong base is added to the pale blue solution of CuSO4, a precipitate forms and the solution above the precipitate is colorless(1) What is the net ionic equation that describes this irreversbile reaction?    Ammonia is then added to the above heterogenous mixture. The precipitate dissolves, and then the entire solution turns a deep navy blue. However adding OH- to the deep navy blue solution results in the precipiate reforming.(2) What is the net ionic equation that describes this reversible event?

Explain why the solubility of a sparingly soluble salt represents an equilibrium system.

(a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in mg/L., on the basis of the solubility product principle, when the chloride concentration has been reduced to 0.2 mg/L? (b) If the concentration of chromate indicator used is 5 x 10 M, how much excess silver ion in mg/L. must be present before the formation of a red precipitate will begin?

An equilibrium reaction between chromate ions, CrO4 2- (yellow), and H+ ions is established to produce dichromate, Cr₂072- (orange). Note the colours. A student adds NaOH to a test tube containing an orange mixture of the above reagents. What is observed? 01. The solution turns from orange to yellow O 2.A precipitate forms 3. The solution tuimns from orange to colourless O4. The solution remains orange

A mixture of 5.000×10−3mol H2 and 1.000×10−2 mol I2 is placed in a 5.000 L flask at 448°C and allowed to come to equilibrium. Analysis of the equilibrium mixture shows that the concentration of HI is 1.87×10−3 M. Calculate the equilibrium constant (Kc).

A sample can contain any ion from groups I to IV. Adding 6M HCl does not produce precipitates.The H + concentrations are adjusted to 0.3M and the solution is saturated with H2S, no precipitate forms.However, when [ H+] is reduced to 10-9M and saturated again with H2S, precipitate appears. Subsequently, it is found that this precipitate is a group III hydroxide.In group IV analysis, a precipitate is formed by adding (NH4) 2CO3. What ions must be present from groups a) I, b) II, c) III d) IV ?

7. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant of ammonia, NH3, is 1.815x10-5 A student worker is asked to prepare a buffer solution with NH3 and ammonium salt. However, after the student did a thorough search, no ammonium salt is found. After the student reported the result to the professor, the professor told the student the buffer can be prepared with ammonia and a strong acid. Can you help this student out? The pH of the buffer to be prepared is 10.08. The molarity of the ammonia in the buffer is 0.4717 M. The molarity of the ammonia solution found in the laboratory is 1.201 M, the strong acid solution is 0.9948 M HNO3. The volume of the buffer solution to be prepared is 500.0 mL. Please answer the following questions. A. B. What is the molarity of the ammonium ion in the buffer? Please provider your answer below. Check answer How many mL of 0.9948 M HNO3 solution is needed? Please provider your answer below. 0² 0₂ $…