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What Is the Concentration of [OH-] in a Solution of 0.5 M HCl?
When discussing the concentration of hydroxide ions ([OH-]) in a solution, it is important to understand the concept of pH and the relationship between hydrogen ions ([H+]) and hydroxide ions ([OH-]). In a neutral solution, the concentration of [H+] is equal to the concentration of [OH-], resulting in a pH of 7. However, in an acidic solution, the concentration of [H+] is higher than that of [OH-], leading to a pH below 7. Conversely, in a basic (alkaline) solution, the concentration of [OH-] is higher than that of [H+], resulting in a pH above 7.
In this case, we are given a solution of hydrochloric acid (HCl) with a concentration of 0.5 M. HCl is a strong acid that dissociates completely in water, resulting in the formation of H+ and Cl- ions. Since HCl is a strong acid, it does not contribute to the concentration of hydroxide ions directly.
To determine the concentration of [OH-] in this solution, we need to calculate the concentration of [H+] first. This can be done using the equation for the dissociation of HCl:
HCl → H+ + Cl-
Since HCl dissociates completely, the concentration of H+ is equal to the concentration of HCl. Therefore, the concentration of [H+] in the solution is 0.5 M.
Now, since we know that in a neutral solution the concentration of [H+] is equal to the concentration of [OH-], we can conclude that the concentration of [OH-] in the solution of 0.5 M HCl is also 0.5 M.
FAQs:
Q: Can the concentration of [OH-] be greater than 0.5 M in this solution?
A: No, in this case, the concentration of [OH-] cannot be greater than 0.5 M. Since HCl is a strong acid that completely dissociates, it does not contribute to the concentration of [OH-]. Therefore, the concentration of [OH-] in this solution is solely determined by the concentration of water, which is typically around 55.6 M. Thus, the concentration of [OH-] cannot exceed 55.6 M.
Q: What is the pH of a 0.5 M HCl solution?
A: The pH of a 0.5 M HCl solution is determined by the concentration of [H+]. Since the concentration of H+ is 0.5 M, the pH can be calculated using the formula pH = -log[H+]. In this case, the pH would be equal to -log(0.5), which is approximately 0.3. Therefore, the pH of a 0.5 M HCl solution is approximately 0.3, indicating a highly acidic solution.
Q: Is it possible to have a solution with a high concentration of [OH-] and a low concentration of [H+]?
A: Yes, it is possible to have a solution with a high concentration of [OH-] and a low concentration of [H+]. Such a solution would be basic or alkaline, with a pH greater than 7. In this case, the concentration of hydroxide ions ([OH-]) would be higher than the concentration of hydrogen ions ([H+]). This can be achieved by adding a base, such as sodium hydroxide (NaOH), to the solution.
Q: How does the concentration of [OH-] affect the acidity or basicity of a solution?
A: The concentration of [OH-] directly affects the basicity of a solution. A higher concentration of [OH-] indicates a more basic (alkaline) solution, while a lower concentration of [OH-] indicates a more acidic solution. The concentration of [OH-] and [H+] are inversely proportional, meaning that an increase in [OH-] corresponds to a decrease in [H+], and vice versa.
In conclusion, the concentration of [OH-] in a solution of 0.5 M HCl is 0.5 M. This is because HCl is a strong acid that dissociates completely, resulting in a solution with a high concentration of [H+] and a low concentration of [OH-]. Understanding the relationship between [H+] and [OH-] is crucial in determining the acidity or basicity of a solution.
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