Multiple Choice
If you decrease the pH of a solution from pH = 2 to pH = 1, which of the following statements is TRUE? Assume the temperature is held constant.
17. Acid and Base Equilibrium
The pH Scale
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What would be the molar concentration of hydroxide ions, [OH^-], in a pH 9.5 aqueous solution?
A
1.00 x 10^-4 M
B
3.16 x 10^-10 M
C
3.16 x 10^-5 M
D
1.00 x 10^-9 M
Verified step by step guidance1
Start by understanding the relationship between pH and pOH. The pH and pOH of a solution are related by the equation: \( \text{pH} + \text{pOH} = 14 \). Since the pH is given as 9.5, you can calculate the pOH using this equation.
Calculate the pOH: \( \text{pOH} = 14 - \text{pH} = 14 - 9.5 \). This will give you the pOH value needed to find the hydroxide ion concentration.
Use the pOH to find the concentration of hydroxide ions, \([\text{OH}^-]\). The relationship between pOH and \([\text{OH}^-]\) is given by the equation: \( \text{pOH} = -\log[\text{OH}^-] \). Rearrange this equation to solve for \([\text{OH}^-]\): \([\text{OH}^-] = 10^{-\text{pOH}} \).
Substitute the calculated pOH value into the equation \([\text{OH}^-] = 10^{-\text{pOH}} \) to find the molar concentration of hydroxide ions.
Verify your calculation by checking if the calculated \([\text{OH}^-]\) value matches one of the given options. Ensure that the value is consistent with the expected concentration for a solution with pH 9.5.
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