In which compound does chlorine have the highest oxidation number? (1) naclo (3) naclo3(2) naclo2 (4) naclo4

              NaClO₄

Solution:

Let us calculate the oxidation state of Chlorine in each compound one by one;

1) NaClO

               O.N of Na = +1

               O.N of O = -2

So,

               (+1) + (Cl) + (-2) = 0

               1 + Cl - 2 = 0

               Cl = -1 + 2

               Cl = +1

2) NaClO₃

               (+1) + (Cl) + (-2)3 = 0

               (+1) + (Cl) - 6 = 0

               1 + Cl - 6 = 0

               Cl = -1 + 6

               Cl = +5

3) NaClO₂

               (+1) + (Cl) + (-2)2 = 0

               (+1) + (Cl) + (-4) = 0

               1 + Cl - 4 = 0

               Cl = -1 + 4

               Cl = +3

4) NaClO₄

               (+1) + (Cl) + (-2)4 = 0

               (+1) + (Cl) + (-8) = 0

               1 + Cl - 8 = 0

               Cl = -1 + 8

               Cl = +7

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

it's 3.2 on edge, i just took the test.