Question

In a 1.0× 10–6 M solution of Ba(OH)2(aq) at 25 °C, identify the relative molar amounts of these species.

Answer 1

at 25 celsius, \(\large [H^+]*[OH^-]=K_w=1.0*10^{-14}\)

To find \([OH^-]\) first write the dissociation equaiton for \(Ba(OH)_2\)

Answer 2

I am really confused. I dont even know what dissociation equation is

Answer 3

A dissociation equation is an equation that describes the process of ions of the compound separating into smaller components - for ionic compounds, this usually happens in water. Water molecules surround the ionic compounds and surround each ions, breaking it apart. The water is omitted. For example, NaCl dissociates into:

\(\large NaCl \rightarrow Na^++Cl^-\)

Answer 4

In a 1.0× 10–6 M solution of Ba(OH)2(aq) at 25 °C, identify the relative molar amounts of these species from most to least. H20, OH, Ba2+, H3O+, Ba(OH)2

Answer 5

right, so write the dissociation of \(Ba(OH)_2\) into \(Ba^{2+}\) and \(OH^-\).