Compare the solubility of mn(oh)2 (ksp = 1.6x10-13)in the following solutions: pure water, a solution buffered to be ph = 6.5 a solution buffered to be ph = 3.5 compare the solubility of mn(oh)2 (ksp = 1.6x10-13)in the following solutions: pure water, a solution buffered to be ph = 6.5 a solution buffered to be ph = 3.5 pure water > ph 3.5 > ph 6.5 (least soluble) ph 3.5 > ph 6.5 > pure water (least soluble) ph 3.5 > pure water > ph 6.5 (least soluble) pure water > ph 6.5 > ph 3.5 (least soluble) ph 6.5 > ph 3.5 > pure water (least soluble)

The order will be:

pH 3.5 > pH 6.5 > pH 7

Explanation:

The solubility equation for Mn(OH)₂ is:

As per the reaction, Mn(OH)₂ is giving hydroxide ions

The given conditions are

a) Pure water = here the pH of water is 7.

[OH⁻] = 10⁻⁷ M

b) pH = 6.5

pOH = 7.5

[OH⁻] = 3.16 X 10⁻⁸ M

c) pH = 3.5

pOH = 10.5

[OH⁻] =3.16 X  10⁻¹¹ M

Thus from the three solutions and water the maximum concentration of hdyroxide ion is in pure water, hence the Mn(OH)₂ will be least soluble in it.

More the concentration of hydroxide, lesser the solubility of Mn(OH)₂

Order will be

pH 3.5 > pH 6.5 > pH 7

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.