In which species does sulfur have the highest oxidation number? s8 (elemental form of sulfur) h2s so2 h2so3 k2so4?
1 answer:
There are rules to assigning conventional oxidation numbers to some elements. For those unspecified, you can solve them. This is how you solve it.
*S8. Since this is in elemental form, its oxidation number is assigned as 0.
*H2S. H is assigned with +1. Since the compound is neutral, the overall charge is 0. So,
2(+1) + x = 0
x = -2
The charge of S here is -2.
*SO₂. O is assigned with (-2). Using the same procedure,
x + 2(-2) = 0
x = +2
The charge of S here is +2.
*H₂SO₃.
2(+1) + x + 3(-2) = 0
x = +4.
The charge of S here is +4.
*K₂SO₄. K is assigned with +1.
2(+1) + x + 4(-2) = 0
x = +6
The charge of S here is +6.
<em>The S with the highest oxidation number is the one in K₂SO₄.</em>
*S8. Since this is in elemental form, its oxidation number is assigned as 0.
*H2S. H is assigned with +1. Since the compound is neutral, the overall charge is 0. So,
2(+1) + x = 0
x = -2
The charge of S here is -2.
*SO₂. O is assigned with (-2). Using the same procedure,
x + 2(-2) = 0
x = +2
The charge of S here is +2.
*H₂SO₃.
2(+1) + x + 3(-2) = 0
x = +4.
The charge of S here is +4.
*K₂SO₄. K is assigned with +1.
2(+1) + x + 4(-2) = 0
x = +6
The charge of S here is +6.
<em>The S with the highest oxidation number is the one in K₂SO₄.</em>
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<u>Answer:</u> The volume of concentrated solution required is 42 mL
<u>Explanation:</u>
To calculate the molarity of the diluted solution, we use the equation:
where,
are the molarity and volume of the concentrated solution
are the molarity and volume of diluted solution
We are given:
Putting values in above equation, we get:
Hence, the volume of concentrated solution required is 42 mL