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Assuming equal concentrations, rank these solutions by pH.
Highest pH to Lowest pH.
HClO4(aq)
Sr(OH)2(aq)
NH3(aq)
RbOH(aq)
HBrO(aq)
The pH scale is zero to 14, covering an array of compounds that are acidic, with low pH up to neutral at a 7 pH, and even basic at higher pH values. The pH of a highly concentrated strong base or acid can be off the scale. For example, a concentrated solution of hydrochloric acid can be negative in pH. Acids and Bases Based on the definition of Arrhenius for bases and acids, the easier is the release of the hydroxide ion of base. The stronger is the base. Thus, metal hydroxides that contain large-sized metal ions are more durable bases than those with smaller dimensions of metal ions.
The pH rises with the level of basicity, and decreases with acidity, which is why acids have lower pH while bases possess higher pH levels. Because RbOH is a base with a high strength which is more powerful as a base than the compounds mentioned and has the most highest pH. It is closely followed by Sr(OH)2 and is also a strong base. Hypobromous acid is a weak acid, so it has a low pH but is not lower than perchloric acid, which is the strongest acid. Perchloric acid therefore has the lowest possible pH.
From the highest pH to the lowest pH:
RbOH → Sr(OH)2 → NH3 → HBrO → HClO4