Basic facts about sex and reproduction, as told to a child
The screen will not be useful in separating the mixture of saw dust, salt and pebbles.
Answer: Option C
<u>Explanation:
</u>
The separation of individual elements from the mixture can be done easily if the size of the elements in the mixture is varying significantly. Just like in the present case, the size of sawdust and salt is very small compared to that of pebbles.
So by using sieves having pores of smaller sizes, pebbles can be separated from the mixture as pebbles will not pass through the minute pores. Even depending upon the size of pores, the saw dust can also be separated using it.
Similarly, we can use water also to separate this mixture as sawdust have least density it will float in water surface and pebbles being the highest density will sink and settle in the bottom of the container.
Remaining salt will get dissolved in water which can be obtained by heating the water in order to precipitate the salt. Even filter paper with different mess size will also help in separating this mixture. But as this mixture is not permeable through screen, the screen cannot be used to separate this mixture.
Answer:
1) The equilibrium constant for the required reaction is 
.
2) 1.2474 M the concentration of ammonia needed to form 0.060 M of complex.Explanation:
Solubility product of silver chloride:
![K_{sp}=1.77\times 10^{-10}=[Ag^+][Cl^-]](https://tex.z-dn.net/?f=K_%7Bsp%7D%3D1.77%5Ctimes%2010%5E%7B-10%7D%3D%5BAg%5E%2B%5D%5BCl%5E-%5D)
..(1)
Formation constant of 
:
![K_f=1.6\times 10^7=\frac{[Ag(NH_3)_2^{+}]}{[Ag^+][NH_3]^2}](https://tex.z-dn.net/?f=K_f%3D1.6%5Ctimes%2010%5E7%3D%5Cfrac%7B%5BAg%28NH_3%29_2%5E%7B%2B%7D%5D%7D%7B%5BAg%5E%2B%5D%5BNH_3%5D%5E2%7D)
..(2)
Reactions solid silver chloride and liquid ammonia:
Expression of an equilibrium constant of the above reaction can be written as:
![K=\frac{[Ag(NH_3)_2^{+}][Cl^-]}{[AgCl][NH_3]^2}](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BAg%28NH_3%29_2%5E%7B%2B%7D%5D%5BCl%5E-%5D%7D%7B%5BAgCl%5D%5BNH_3%5D%5E2%7D)
[AgCl] = solid = 1
![K=\frac{[Ag(NH_3)_2^{+}][Cl^-]}{[1][NH_3]^2}\times \frac{[Ag^+]}{[Ag^+]}](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BAg%28NH_3%29_2%5E%7B%2B%7D%5D%5BCl%5E-%5D%7D%7B%5B1%5D%5BNH_3%5D%5E2%7D%5Ctimes%20%5Cfrac%7B%5BAg%5E%2B%5D%7D%7B%5BAg%5E%2B%5D%7D)
(from 1 and 2)
The equilibrium constant for the required reaction is .
2)
Concentration of complex at equilibrium : ![[Ag(NH_3)_2^{+}]](https://tex.z-dn.net/?f=%5BAg%28NH_3%29_2%5E%7B%2B%7D%5D)
= 0.060 M
Initaly
x 0 0
At equilibrium
x- 2(0.060) 0.060 0.060
![K=\frac{[Ag(NH_3)_2^{+}][Cl^-]}{[1][NH_3]^2}](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BAg%28NH_3%29_2%5E%7B%2B%7D%5D%5BCl%5E-%5D%7D%7B%5B1%5D%5BNH_3%5D%5E2%7D)
x = 1.2474 M
1.2474 M the concentration of ammonia needed to form 0.060 M of complex.
Answer: Volume is 0.466 ml. Maybe in this case it is safer to round downward.
Explanation: V = 14.0 mg / 30 mg/mL = 0.466.. ml
