Question

Нужно очень срочно решить задачу Вычислите концентрацию ионов серебра в 0,1М [Ag(NH3)2]Cl, если константа неустойчивости комплексного иона равна 5,89*10-8. Раствор соли содержит 5 г/л аммиака.

Answer 1

Ответ:

[Ag(NH3)2]Cl=[Ag(NH3)2]+ + Cl- диссоциация протекает практически полностью, поэтому С [Ag(NH3)2]+=С (Сl-) = 0,1 моль/л

диссоциация компл. иона [Ag(NH3)2]+=Ag+ + 2NH3

Кнест=[Ag+][NH3]^2 / [Ag(NH3)2]+

n(NH3)=m/M=5/17=0,2941 моль

C(NH3)=n/V=0,2941 моль/л- большой избыток, поэтому NH3, обр. в рез диссоциации компл. иона, можно пренебречь и считать [NH3]=0,2941

тогда 5,89*10^–8 = [Ag+]*(0,2941)^2 / 0,1

[Ag+]=6,81*10-8 моль/л

Объяснение:

Как то так, вроде правильно

Answer 2

Calculation of Silver Ion Concentration in 0.1M [Ag(NH3)2]Cl Solution

To calculate the concentration of silver ions in the given solution, we need to consider the equilibrium reaction of the complex ion [Ag(NH3)2]+ with water:

[Ag(NH3)2]+ ⇌ Ag+ + 2NH3

The equilibrium constant for this reaction is given as 5.89 * 10^-8.

We are also given that the solution contains 5 g/L of ammonia (NH3).

To solve this problem, we can use the concept of the solubility product constant (Ksp) and the concentration of the complex ion.

The solubility product constant (Ksp) is defined as the product of the concentrations of the ions in a saturated solution at equilibrium. In this case, the Ksp can be expressed as:

Ksp = [Ag+][NH3]^2

Since the concentration of Ag+ is what we need to find, let's express it in terms of the concentration of the complex ion [Ag(NH3)2]+:

[Ag(NH3)2]Cl ⇌ [Ag(NH3)2]+ + Cl-

The concentration of [Ag(NH3)2]+ can be expressed as:

[Ag(NH3)2]+ = [Ag(NH3)2]Cl

Now, let's substitute this expression into the Ksp equation:

Ksp = [Ag(NH3)2]Cl * [NH3]^2

We are given that the concentration of [Ag(NH3)2]Cl is 0.1 M. However, we need to convert the concentration of ammonia from grams per liter (g/L) to moles per liter (M). The molar mass of ammonia (NH3) is approximately 17 g/mol.

Concentration of NH3 = (5 g/L) / (17 g/mol) = 0.294 M

Now, let's substitute the values into the Ksp equation:

5.89 * 10^-8 = (0.1 M) * (0.294 M)^2

Simplifying the equation, we can solve for the concentration of Ag+:

[Ag+] = (5.89 * 10^-8) / (0.1 M * (0.294 M)^2)

Calculating this expression gives us the concentration of silver ions in the solution.

Please note that the search results provided by You.com did not yield any relevant information for this specific question. Therefore, the calculation was performed based on the given information and the principles of equilibrium chemistry.