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Ch.16 - Acid-Base Equilibria
All textbooksBrown 14th EditionCh.16 - Acid-Base EquilibriaProblem 38
Chapter 16, Problem 38

Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid (H2CO3), causing the pH of clean, unpolluted rain to range from about 5.2 to 5.6. What are the ranges of [H+] and [OH-] in the raindrops?

Verified step by step guidance
1
Step 1: Understand the relationship between pH and [H+]. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration: \( \text{pH} = -\log[H^+] \).
Step 2: Calculate the range of [H+] using the given pH range. For pH 5.2, use the formula \( [H^+] = 10^{-\text{pH}} \) to find the concentration of hydrogen ions. Repeat this calculation for pH 5.6.
Step 3: Understand the relationship between [H+] and [OH-] using the water dissociation constant. At 25°C, the product of the concentrations of hydrogen ions and hydroxide ions in water is constant: \( [H^+][OH^-] = 1.0 \times 10^{-14} \).
Step 4: Calculate the range of [OH-] using the [H+] values obtained in Step 2. Rearrange the equation from Step 3 to solve for [OH-]: \( [OH^-] = \frac{1.0 \times 10^{-14}}{[H^+]} \).
Step 5: Verify the consistency of your results. Ensure that the calculated [H+] and [OH-] values are consistent with the pH range and the water dissociation constant.
Related Practice
Open Question
Complete the following table by calculating the missing entries and indicating whether the solution is acidic or basic.
Open Question
Complete the following table by calculating the missing entries. In each case, indicate whether the solution is acidic or basic.
Textbook Question

The average pH of normal arterial blood is 7.40. At normal body temperature 137 °C2, Kw = 2.4 * 10-14. Calculate 3H+4, 3OH-4, and pOH for blood at this temperature.

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Textbook Question

Addition of the indicator methyl orange to an unknown solution leads to a yellow color. The addition of bromthymol blue to the same solution also leads to a yellow color. (b) What is the range (in whole numbers) of possible pH values for the solution?

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Textbook Question

Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromthymol blue to the same solution leads to a yellow color. (b) Which of the following can you establish about the solution: (i) A minimum pH, (ii) A maximum pH, or (iii) A specific range of pH values?

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Textbook Question

Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromthymol blue to the same solution leads to a yellow color. (c) What other indicator or indicators would you want to use to determine the pH of the solution more precisely?

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