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Chapter 15: Problem 53

What is the \(\mathrm{pH}\) of a solution prepared by dissolving 0.15 \(\mathrm{mol}\) of the strong base \(\mathrm{Ba}(\mathrm{OH})_{2}\) in one liter of water? (Hint: How much hydroxide ion does barium hydroxide generate per mole in solution?)

Short Answer

Expert verified
After performing the steps, you will find out that the pH of the solution is greater than 7 which indicates that the solution is basic.

Step by step solution

01

Determine the Concentration of Hydroxide ions (\([OH^{-}]\)

Barium hydroxide \([Ba(OH)_{2}]\) is a strong base and it completely dissociates in the solution to give barium ions \([Ba^{2+}]\) and hydroxide ions \([OH^{-}]\). As each mole of barium hydroxide will produce two moles of \([OH^{-}]\), the concentration of hydroxide ions in the solution becomes twice the amount of \([Ba(OH)_{2}]\) dissolved. Given that, 0.15 mol of \([Ba(OH)_{2}]\) is dissolved in 1 L of water, therefore, \([OH^{-}]= 2 \times 0.15 Mol/L = 0.3 Mol/L.
02

Calculate pOH

After finding the \([OH^{-}]\) concentration, calculate the pOH of the solution. pOH is calculated using the formula: pOH = \(-\log[OH^{-}]\). Therefore, pOH = \(-\log(0.3)\).
03

Calculate pH

Once the pOH is known, use the relationship between pH and pOH to find the pH of the solution. This relationship is expressed by the equation: \[pH + pOH = 14 \]. So, we can rewrite this equation to solve for pH: \[ pH = 14 - pOH \].

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Most popular questions from this chapter

Explain what a titration curve is, and sketch its shape.

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