Explanation:
To calculate that you need to know the value of the Kps (constant of solubility) at 30°C of KBr in water.
<u>When the product of the concentrations of both ions (Br- and K+) equals the Kps, the solution is saturated. </u>
Given the disociation of the salt in water:
The concentration of both ions are equal (1:1 ratio) and the same as the concentration of KBr added.
The Kps:
![Kps=[K^+][Br^-]](https://tex.z-dn.net/?f=Kps%3D%5BK%5E%2B%5D%5BBr%5E-%5D)
![[KBr]=(Kps)^{1/2}](https://tex.z-dn.net/?f=%5BKBr%5D%3D%28Kps%29%5E%7B1%2F2%7D)
[KBr] are <u>moles of the salt per litre of water</u>
Assuming a density of water of 1 g/cm3, 100 g are 0.1 litre
To calculate the mass:
![m=[KBr]*M*0.1 litre](https://tex.z-dn.net/?f=m%3D%5BKBr%5D%2AM%2A0.1%20litre)
where M is the molecular weight of the salt.
I think it’s law conservation of mass.
So 200g(NH3)-47g(N2)=153g(H2)
H2+N2—->NH3
Mass per unit volume is nothing but density of an body density = Mass/Volume. hope this helps. :)
Answer:
Soluble salts can be made by reacting acids with soluble or insoluble reactants. Titration must be used if the reactants are soluble. Insoluble salts are made by precipitation reactions.
Making insoluble salts
An insoluble salt can be prepared by reacting two suitable solutions together to form a precipitate.
Determining suitable solutions
All nitrates and all sodium salts are soluble. This means a given precipitate XY can be produced by mixing together solutions of:
X nitrate
sodium Y
For example, to prepare a precipitate of calcium carbonate:
X = calcium and Y = carbonate
mix calcium nitrate solution and sodium carbonate solution together
calcium nitrate + sodium carbonate → sodium nitrate + calcium carbonate
Ca(NO3)2(aq) + Na2CO3(aq) → 2NaNO3(aq) + CaCO3(s)
It also works if potassium carbonate solution or ammonium carbonate solution is used instead of sodium carbonate solution. Remember that all common potassium and ammonium salts are soluble.
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Explanation:
