Which of the following solutions is the most basic? (a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.

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Identify the nature of each compound: NaCl is a neutral salt, CsOH is a strong base, and Sr(OH)2 is a strong base.

Recognize that the basicity of a solution is determined by the concentration of hydroxide ions (OH⁻) it produces.

Calculate the concentration of OH⁻ ions for each solution: NaCl does not produce OH⁻ ions, CsOH produces OH⁻ ions equal to its concentration, and Sr(OH)2 produces twice the concentration of OH⁻ ions because it dissociates into two OH⁻ ions per formula unit.

Compare the OH⁻ ion concentrations: 0 M for NaCl, 0.150 M for CsOH, and 0.200 M for Sr(OH)2.

Determine which solution has the highest OH⁻ concentration, indicating it is the most basic.

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pH and Basicity

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. A pH value above 7 signifies a basic solution, while a value below 7 indicates acidity. Basic solutions contain higher concentrations of hydroxide ions (OH-) compared to hydrogen ions (H+), which is crucial for determining the most basic solution among the options provided.

Strong Bases

Strong bases are substances that completely dissociate in water to produce hydroxide ions. Examples include alkali metal hydroxides like CsOH and alkaline earth metal hydroxides like Sr(OH)2. The strength of a base is determined by its ability to increase the concentration of OH- ions in solution, which directly affects the pH and basicity of the solution.

Concentration and Dilution

Concentration refers to the amount of solute present in a given volume of solution, typically expressed in molarity (M). In this context, higher concentrations of strong bases will lead to a greater production of hydroxide ions, thus increasing the basicity of the solution. Understanding how concentration affects pH is essential for comparing the basicity of the given solutions.