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Some examples of insoluble bromide compounds include silver bromide (AgBr), lead(II) bromide (PbBr2), and mercury(I) bromide (Hg2Br2). These compounds do not dissolve easily in water and form solid precipitates when bromide ions are combined with the corresponding metal ions.
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Most nitrate compounds are highly soluble in water, so adding strontium nitrate to water would create a large number of free ions in the water. These free ions could then act as charge carriers, making the water able to conduct current. Since adding strontium nitrate would make the water conductive, strontium nitrate is an electrolyte. Some other strontium salts, such as strontium sulfide, wouldn't dissolve significantly in water, so they wouldn't create the free ions necessary to conduct current.
1/2 ounce of water, I believe.
Sodium Bromide is of course very soluble in water. In fact 116 grams of NaBr will dissolve in 100 cc of H2O at 50 degrees C.
Sodium Bromide is a stable salt. It will dissolve in water.
Calcium bromide itself is a solid at room temperature, but it will dissolve in water to make a solution.
It allows ions to flow through the water.
Yes it does dissociate, and dissolve completely in water, as KBr is an ionic salt.
Some examples of insoluble bromide compounds include silver bromide (AgBr), lead(II) bromide (PbBr2), and mercury(I) bromide (Hg2Br2). These compounds do not dissolve easily in water and form solid precipitates when bromide ions are combined with the corresponding metal ions.
Strontium hydroxides soluble at higher temperatures, where it forms a strong alkaline solution by completely dissociating in addition to dissolving (not the same thing).
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5.53 g
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