Answer:
Solubility in water Anhydrous: 74.5 g/100 mL (20 °C) Hexahydrate: 49.4 g/100 mL (−25 °C) 59.5 g/100 mL (0 °C) 65 g/100 mL (10 °C) 81.1 g/100 mL (25 °C) 102.2 g/100 mL (30.2 °C) α-Tetrahydrate: 90.8 g/100 mL (20 °C) 114.4 g/100 mL (40 °C) Dihydrate: 134.5 g/100 mL (60 °C) 152.4 g/100 mL (100 °C)
Answer:
has molar mass of 142 g.
Explanation:
Firstly we will find out the atomic weight of the elements of the compound.
Mg = 24 P = 31 Al = 27 Cl = 35 Ba = 137 O = 16
Now 1st compound is , in this compound there is 1 atom of Magnesium and 2 atom of Chlorine.
So atomic weight of =
2nd compound is , in this compound there is 2 atom of Phosphorus and 5 atom of Oxygen.
So atomic weight of =.
3rd compound is , in this compound there is 1 atom of Barium and 2 atom of Chlorine.
So atomic weight of =
4th compound is , in this compound there is 1 atom of Aluminium and 3 atom of Chlorine.
So atomic weight of =
Hence the substance having molar mass of 142 g is .
Answer is: the maximum concentration of Pb²⁺ is 6.8·10⁻³ M.
Chemical reaction 1: PbCl₂(s) → Pb²⁺(aq) + 2Cl⁻(aq).
Chemical reaction 2: NaCl(aq) → Na⁺(aq) + Cl⁻(aq).
Ksp(PbCl₂) = 1.7·10⁻⁵.
c(NaCl) = c(Cl⁻) = 0.0500 M.
Ksp(PbCl₂) = c(Pb²⁺) · c(Cl⁻)².
c(Pb²⁺) = Ksp(PbCl₂) ÷ c(Cl⁻)².
c(Pb²⁺) = 1.7·10⁻⁵ M³ ÷ (0.0500 M)².
c(Pb²⁺) = 0.000017 M³ ÷ 0.0025 M².
c(Pb²⁺) = 0.0068 M = 6.8·10⁻³ M.
One element, two atoms.
Element is Hydrogen.
Two atoms of Hydrogen.
There’s no other degenerate s orbital because the there can be only one s orbital for any value of n.