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

Question

aaronq · Answer

at 25 celsius, $\large [H^+]*[OH^-]=K_w=1.0*10^{-14}$

To find $[OH^-]$ first write the dissociation equaiton for $Ba(OH)_2$

anonymous · Answer

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

aaronq · Answer

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:

$\large NaCl \rightarrow Na^++Cl^-$

anonymous · Answer

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

aaronq · Answer

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