What volume of water is needed to dissolve 0.010 moles of AgCl entirely? The K for AgCl is 1.7x10-10

The volume of water = 766.87 L

Given

The K for AgCl is 1.7x10⁻¹⁰

Required

the volume of water

Solution

AgCl dissolves in water to form ions(s=solubility)

AgCl    ⇒    Ag⁺  +    Cl⁻

  s               s            s

K AgCl = [Ag⁺] [Cl⁻]

K AgCl = (s) (s) = s²

1.7x10⁻¹⁰ = s²

s=1.304 x 10⁻⁵ mol/L

The solubility of AgCl in water = 1.304 x 10⁻⁵ mol/L

So for 0.01 moles of AgCl, water needed :

it can be observed without changing the identity of the object.

it depends on what substance you're talking about as well as many other factors. in quantum mechanics, the observation of particles affects the observers ability to measure certain properties. for example: you can know the velocity of a particle, but you can't know it's position; or you can know it's position, but not it's velocity. it's like trying to find out where a grain of sand is by throwing other grains of sand at it. once you find out where it is, it's been moved. it's also like trying to find an answer to the question of whether or not a tree falling in a forest makes a sound if nobody is there to hear it. paradoxically, the only way to find out is to be there and hear it.