Balance the following ionic equation for a redox reaction, using whole number coefficients. mno−4(aq)+so2−3(aq)+h3o+(aq)⟶mn2+(a q)+so2−4(aq)+h2o(l)

Answer : The balance ionic equation for a redox reaction will be,

Explanation :

The half balanced redox reactions in acidic medium will be:

(1)

(2)

In order of balance the electrons, we multiply the equation 1 by 2 and equation 2 by 5, we get:

(1)

(2)

Now adding both the equation, we get:

The overall reaction will be,

c most likely

hop this let me know if it is wrong

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%