Acid rain is caused by sulfur dioxide dissolving in water to form sulfuric acid. If the pH of an acid rain sample is 2.2, what is the hydrogen ion concentration in moles per liters? 6.31Ă—10-3 M 3.31 x 10-3 M 7.2 X 10-3 M 1.2 X 10-3 M
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2. We need to find the hydrogen ion concentration in moles per liters. The relationship between pH and hydrogen ion concentration is given by the formula: $$pH = -log_{10}[H^+]$$ where $[H^+]$ is the hydrogen ion concentration. Show more…
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Refer to Problem 19. Many lakes in Canada and the United States will no longer sustain some forms of wildlife because of the increase in acidity of the water from acid rain and snow caused by sulfur dioxide emissions from industry. If the pH of a sample of rainwater is $5.2,$ what is its hydrogen ion concentration in moles per liter? Compute the answer to two significant digits.
Danielle F.
Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which dissolve to form acids such as $\mathrm{H}_{2} \mathrm{SO}_{3}, \mathrm{H}_{2} \mathrm{SO}_{4}$, and $\mathrm{HNO}_{3}$. Trees and plants are affected if the acid rain has a $\mathrm{pH}$ of $3.5$ or lower. What is the hydrogen ion concentration in acid rain that has a $\mathrm{pH}$ of $3.16$ ? What is the $\mathrm{pH}$ of a solution having twice your calculated hydrogen ion concentration?
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