Answer:
AC₄ will precipitate out first.
Explanation:
A solid will precipitate out if the ionic product of the solution exceeds the solubility product.
Let us check the ionic product
a) A₂B₃
Ionic product = [A]²[B]³
[A] = say "s"
[B] = 0.05 , [B]³ = (0.05)³ = 0.000125
2.3 X 10⁻⁸ = [A]²(0.000125)
[A] = 0.0136
b) AC₄
Ionic product = [A] [C]⁴
[A] = "s"
[A][0.05]⁴ = 4.10 X 10⁻⁸
[A]=0.00656 M
So for ionic product to exceed solubility product, we need less concentration of A in case of AC₄.
Answer: 770 g water are needed to dissolve 27.8 g of ammonium nitrate 
in order to prepare a 0.452 m solution
Explanation:
Molality : It is defined as the number of moles of solute present per kg of solvent
Formula used :
where,
n= moles of solute
Moles of 
= weight of the solvent in g = ?
Thus 770 g water are needed to dissolve 27.8 g of ammonium nitrate in order to prepare a 0.452 m solution
Answer:
178 grams
Explanation:
<em>It is known that 1.0 mole of a compound contains Avogadro's number of molecules (6.022 x 10²³).</em>
<em><u>Using cross multiplication:</u></em>
1.0 mol contains → 6.022 x 10²³ molecules.
??? mol contains → 6.3 x 10²⁴ molecules.
∴ The no. of moles of (6.3 x 10²⁴ molecules) of NH₃ = (1.0 mol)(6.3 x 10²⁴ molecules)/(6.022 x 10²³ molecules) = 10.46 mol.
<em>∴ The no. of grams of NH₃ present = no. of moles x molar mass</em> = (10.46 mol)(17.0 g/mol) = <em>177.8 g ≅ 178 g.</em>
Lets assume the gas is acting Ideally, then According to Ideal Gas Equation the density is given as,
d = P M / R T ------- (1)
Where;
P = Pressure = 1.03 atm
M = Molar Mass = 146.06 g/mol
R = Gas Constant = 0.08206 atm.L.mol⁻¹.K⁻¹
T = Temperature = 297 K
Putting Values in eq. 1,
d = (1.03 atm × 146.06 g/mol) ÷ (0.08206 atm.L.mol⁻¹.K⁻¹ × 297 K)
density = 6.17 g/L
Answer:
The Earth is divided into two halves by the prime meridian, forming two half spheres divided vertically. The Earth is also divided into two halves by the equator, creating two half spheres divided horizontally.
Explanation:
I took it on edge ( :
