Which of the following is an example of a strong base?

Which of the following is an example of a strong base?

• A. NH3
• B. Ca(OH)2
• C. HCO3-
• D. Me(OH)2

Answer: (B)

The choice of calcium hydroxide, Ca(OH)2, as an example of a strong base is accurate due to its complete dissociation in water, which results in a high concentration of hydroxide ions (OH-) in solution. Strong bases are characterized by their ability to significantly increase the pH of a solution by providing hydroxide ions, thus making the solution strongly alkaline. Calcium hydroxide is classified as a strong base because it readily dissolves in water, although it is not as soluble as some alkali metal hydroxides. When dissolved, it dissociates completely into calcium ions (Ca2+) and hydroxide ions (OH-), which is the defining behavior of strong bases. The presence of these free hydroxide ions leads to a high pH and increases the basicity of the solution. In contrast, ammonia (NH3) is a weak base that only partially accepts protons in solution, leading to a lesser concentration of hydroxide ions. Bicarbonate (HCO3-) is actually a weak base as well, and while it can act as a buffer, it does not exhibit the properties of a strong base. The compound Me(OH)2 (where Me stands for a metal) suggests a divalent metal

The choice of calcium hydroxide, Ca(OH)2, as an example of a strong base is accurate due to its complete dissociation in water, which results in a high concentration of hydroxide ions (OH-) in solution. Strong bases are characterized by their ability to significantly increase the pH of a solution by providing hydroxide ions, thus making the solution strongly alkaline.

Calcium hydroxide is classified as a strong base because it readily dissolves in water, although it is not as soluble as some alkali metal hydroxides. When dissolved, it dissociates completely into calcium ions (Ca2+) and hydroxide ions (OH-), which is the defining behavior of strong bases. The presence of these free hydroxide ions leads to a high pH and increases the basicity of the solution.

In contrast, ammonia (NH3) is a weak base that only partially accepts protons in solution, leading to a lesser concentration of hydroxide ions. Bicarbonate (HCO3-) is actually a weak base as well, and while it can act as a buffer, it does not exhibit the properties of a strong base. The compound Me(OH)2 (where Me stands for a metal) suggests a divalent metal