For the reaction at 20 degree C, NH_3(aq) + H^+ (aq) NH_4 (aq) the equilibrium c

Question

For the reaction at 20 degree C, NH_3(aq) + H^+ (aq) NH_4 (aq) the equilibrium constant is calculated to be K = 4.5 times 10 a. Write the equilibrium expression for this reaction. b. From the size of the number for K, does the equilibrium lie to the left or to the right? c. If a base (NaOH) was added to the mixture, in which direction would the reaction shift, to the left or to the right? Explain your answer. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30 M for each of these ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex? In the reaction below, NH_3(g) + H_2O(I) NH^-_2 + H_3O^+ the equilibrium constant is 10^-34. Is this reaction likely to take place? Explain your answer

Explanation / Answer

Ans 1 a. The equilibrium equation is given as

[product] / [reactant]

So for the given reaction it will be

Kc = [NH4+] / [NH3] [H+]

Ans 1 b. As the value of kc is 4.5 × 105 it means the equillibrium is shifted towards product side that is right.

For any value of kc more than 103 , the products dominate in the reaction.

Ans 1 c. NaOH will give Na+ and OH- ions in the reaction which is not a common species neither in reactant nor in product. So the addition of sodium hydroxide will have no significant effect on the equilibrium rather the hydroxide ions will neutralise protons on the left side and form ammonium hydroxide on the right side.

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.