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Questions and Answers
If a solution has a hydroxide ion concentration of $1 \times 10^{-3}$ M, what is the pH of the solution?
If a solution has a hydroxide ion concentration of $1 \times 10^{-3}$ M, what is the pH of the solution?
- 11 (correct)
- 13
- 3
- 1
A solution has a pH of 4. What is the hydrogen ion concentration, $[H^+]$, in moles per liter?
A solution has a pH of 4. What is the hydrogen ion concentration, $[H^+]$, in moles per liter?
- $1 \times 10^{-10}$
- 10
- 4
- $1 \times 10^{-4}$ (correct)
Which of the following pH values indicates the strongest acid?
Which of the following pH values indicates the strongest acid?
- 6.9
- 5
- 7.1
- 1 (correct)
For a solution at $25^{\circ}C$, if the hydrogen ion concentration, $[H^+]$, is $1.0 \times 10^{-5}$ M, what is the pOH of the solution?
For a solution at $25^{\circ}C$, if the hydrogen ion concentration, $[H^+]$, is $1.0 \times 10^{-5}$ M, what is the pOH of the solution?
A solution is found to have a pH of 8.2. Which of the following statements is true regarding this solution?
A solution is found to have a pH of 8.2. Which of the following statements is true regarding this solution?
Which of the following statements best describes the relationship between pH and pOH in aqueous solutions at $25^{\circ}C$?
Which of the following statements best describes the relationship between pH and pOH in aqueous solutions at $25^{\circ}C$?
If the $[H^+]$ concentration in a solution is increased by a factor of 100, what will be the change in pH?
If the $[H^+]$ concentration in a solution is increased by a factor of 100, what will be the change in pH?
Which of the following indicates a neutral solution at $25^{\circ}C$?
Which of the following indicates a neutral solution at $25^{\circ}C$?
What is the pOH of a solution with a pH of 4.6 at $25^{\circ}C$?
What is the pOH of a solution with a pH of 4.6 at $25^{\circ}C$?
Which of the following solutions would have the highest concentration of hydroxide ions ($OH^−$)?
Which of the following solutions would have the highest concentration of hydroxide ions ($OH^−$)?
What is the hydrogen ion concentration $[H^+]$ of a solution with a pOH of 2?
What is the hydrogen ion concentration $[H^+]$ of a solution with a pOH of 2?
If a sample of lemon juice has $[H^+] = 3.8 \times 10^{-4}$ M, what is the pH?
If a sample of lemon juice has $[H^+] = 3.8 \times 10^{-4}$ M, what is the pH?
If a commonly available window-cleaning solution has $[OH^-] = 1.9 \times 10^{-6}$ M, what is the pH?
If a commonly available window-cleaning solution has $[OH^-] = 1.9 \times 10^{-6}$ M, what is the pH?
A sample of freshly pressed apple juice has a pOH of 10.24. What is $[H^+]$?
A sample of freshly pressed apple juice has a pOH of 10.24. What is $[H^+]$?
Which of the following is true regarding indicators?
Which of the following is true regarding indicators?
Flashcards
What is pH?
What is pH?
A method of reporting hydrogen ion concentration.
pH equation
pH equation
pH = -log[H+], where [H+] is the hydrogen ion concentration.
What is neutral pH?
What is neutral pH?
A solution with a pH of 7.00
What is acidic pH?
What is acidic pH?
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What is basic pH?
What is basic pH?
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What is pOH?
What is pOH?
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What is pKw?
What is pKw?
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pH + pOH = ?
pH + pOH = ?
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Acid-Base Indicators
Acid-Base Indicators
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What do pH meters do?
What do pH meters do?
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Study Notes
- CHEM 1220 - Chapter 16: Acid-Base Equilibria 16-4
pH
- pH is a method of reporting hydrogen ion concentration.
- pH = -log[H+]
- Neutral pH is 7.00
- Acidic pH is below 7.00
- Basic pH is above 7.00
pH Scale Examples
- Stomach acid [H+] is 1x10^-1, with a pH of 1.0, and a pOH of 13.0.
- Lemon juice [H+] is 1x10^-2, with a pH of 2.0, and a pOH of 12.0.
- Cola and vinegar [H+] is 1x10^-3, with a pH of 3.0, and a pOH of 11.0.
- Wine [H+] is 1x10^-4, with a pH of 4.0, and a pOH of 10.0.
- Black coffee [H+] is 1x10^-5, with a pH of 5.0, and a pOH of 9.0.
- Rain, Saliva, and Milk [H+] is 1x10^-6, with a pH of 6.0, and a pOH of 8.0.
- Human blood [H+] is 1x10^-7, with a pH of 7.0, and a pOH of 7.0.
- Seawater [H+] is 1x10^-8, with a pH of 8.0, and a pOH of 6.0.
- Borax [H+] is 1x10^-9, with a pH of 9.0, and a pOH of 5.0.
- Lime water [H+] is 1x10^-10, with a pH of 10.0, and a pOH of 4.0.
- Household ammonia [H+] is 1x10^-11, with a pH of 11.0, and a pOH of 3.0.
- Household bleach [H+] is 1x10^-12, with a pH of 12.0, and a pOH of 2.0.
Formulas
- pH + pOH = 14
- [H+][OH-] = 1x10^-14
Relationships among (H+), (OH-), and pH at 25 °C
- For acidic solutions [H+] >1.0 x 10^-7, [OH-] <1.0 x 10^-7, with a pH <7.00
- For neutral solutions [H+] =1.0 x 10^-7, [OH-] =1.0 x 10^-7, with a pH of 7.00
- For basic solutions [H+] <1.0 x 10^-7, [OH-] >1.0 x 10^-7, with a pH >7.00
Calculating pH from [H+]
- In a sample of lemon juice, [H+] = 3.8 x 10^-4M, the pH is 3.42
- If a window-cleaning solution has [OH-] = 1.9 x 10^-6M, the pH is 8.28
pOH and Other "p" Scales,
- The "p" in pH tells us to take the -log of a quantity, in this case, hydrogen ions.
- Other "p" systems include pOH: -log[OH] , and pKw: - log Kw
- [H3O+][OH-] = Kw = 1.0 x 10^14
- -log[H3O+] + -log[OH-] = -log Kw = 14.00
- This results in pH + pOH = pKw = 14.00
Calculating [H+] from pOH
- A sample of freshly pressed apple juice has a pOH of 10.24, therefore the [H+] = 1.74 x 10^-4 M
Indicators
- Indicators, including litmus paper, are used for less accurate measurements.
- An indicator is one color in its acid form and another color in its basic form.
- pH meters are used for accurate measurements of pH.
- Electrodes indicate small changes in voltage to detect pH.
- Most indicators have a useful range of about 2 pH units.
- Common acid-base indicators include: methyl violet, thymol blue, methyl orange, methyl red, bromthymol blue, phenolphthalein, and alizarin yellow R.
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