Question

In: Chemistry

2. A 1.00 liter solution contains 0.42 M ammonia and 0.32 M ammonium iodide. If 0.16...

2. A 1.00 liter solution contains 0.42 M ammonia and 0.32 M ammonium iodide. If 0.16 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydroiodic acid.)

A. The number of moles of NH3 will decrease.

B. The number of moles of NH4+ will increase.

C. The equilibrium concentration of H3O+ will increase.

D. The pH will increase.

E. The ratio of [NH3] / [NH4+] will increase.

2A. A 1.00 liter solution contains 0.35 M ammonia and 0.45 M ammonium perchlorate.

If 0.110 moles of calcium hydroxide are added to this system, indicate whether the following statements are true or false.

(Assume that the volume does not change upon the addition of calcium hydroxide.)

_______TrueFalse A. The number of moles of NH₃ will decrease.

_______TrueFalse B. The number of moles of NH₄⁺ will increase.

_______TrueFalse C. The equilibrium concentration of H₃O⁺ will decrease.

_______TrueFalse D. The pH will decrease.

_______TrueFalse E. The ratio of [NH₃] / [NH₄⁺] will increase.

Expert Solution

after addition of HCl,

poH of basic buffer = pkb+ log((NH4+ + HCl)/(NH3-HCl))

pH = 14-pOH

pH = - log[H3O+]

2)

A. The number of moles of NH3 will decrease = True

B. The number of moles of NH4+ will increase = True

C. The equilibrium concentration of H3O+ will increase = true

D. The pH will increase = false

E. The ratio of [NH3] / [NH4+] will increase = false

2A)

after addition of ca(OH)2,

poH of basic buffer = pkb+ log((NH4+ -(2*ca(OH)2))/(NH3+(2*ca(OH)2)))

pH = 14-pOH

pH = - log[H3O+]

A. The number of moles of NH3 will decrease = false

B. The number of moles of NH4+ will increase = false

C. The equilibrium concentration of H3O+ will decrease = true

D. The pH will decrease = false

E. The ratio of [NH3] / [NH4+] will increase = true

queen_honey_blossom answered 2 years ago

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