Question
The pH of a solution of a strong acid was determined to be 3. If water is then added to dilute this solution, would the pH change? Why or why not? Could enough water ever be added to raise the pH of an acid solution above 7 ?
Step 1
A pH of 3 indicates that the concentration of hydrogen ions \([H^+]\) in the solution is \(10^{-3}\) M, since pH is defined as the negative logarithm of the hydrogen ion concentration. Show more…
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Adding a few drops of a strong acid to water will lower the pH appreciably. However, adding the same number of drops to a buffer does not appreciably alter the pH. Explain. (10.7) (FIGURE A,AND B CANT COPY)
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You make a solution by dissolving $0.0010$ mol of $\mathrm{HCl}$ in enough water to make $1.0 \mathrm{~L}$ of solution. a. Write the chemical equation for the reaction of $\mathrm{HCl}(a q)$ and water. b. Without performing calculations, give a rough estimate of the $\mathrm{pH}$ of the $\mathrm{HCl}$ solution. Justify your answer. c. Calculate the $\mathrm{H}_{3} \mathrm{O}^{+}$ concentration and the $\mathrm{pH}$ of the solution. d. Is there any concentration of the base $\mathrm{OH}^{-}$ present in this solution of $\mathrm{HCl}(a q) ?$ If so, where did it come from? e. If you increase the OH $^{-}$ concentration of the solution by adding $\mathrm{NaOH}$, does the $\mathrm{H}_{3} \mathrm{O}^{+}$ concentration change? If you think it does, explain why this change occurs and whether the $\mathrm{H}_{3} \mathrm{O}^{+}$ concentration increases or decreases. f. If you were to measure the $\mathrm{pH}$ of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g. Explain how two different volumes of your original $\mathrm{HCl}$ solution can have the same $\mathrm{pH}$ yet contain different moles of $\mathrm{H}_{3} \mathrm{O}^{+}$ h. If $1.0 \mathrm{~L}$ of pure water were added to the $\mathrm{HCl}$ solution, would this have any impact on the $\mathrm{pH}$ ? Explain.
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