Podcast
Questions and Answers
Which of the following is not considered one of the seven common strong acids?
Which of the following is not considered one of the seven common strong acids?
- Nitric acid (HNO3)
- Sulfuric acid (H2SO4)
- Hydrochloric acid (HCl)
- Acetic acid (CH3COOH) (correct)
Why is H2SO4 categorized differently from HCl, HNO3, HBr, HI, HClO3, and HClO4?
Why is H2SO4 categorized differently from HCl, HNO3, HBr, HI, HClO3, and HClO4?
- It contains sulfur, giving it unique properties.
- It is a weak acid, unlike the others.
- It does not fully ionize in solution.
- It is a diprotic acid, while the others are monoprotic. (correct)
In a solution of a strong monoprotic acid, what is the relationship between the concentration of the acid and the concentration of $H^+$ ions?
In a solution of a strong monoprotic acid, what is the relationship between the concentration of the acid and the concentration of $H^+$ ions?
- The $H^+$ concentration is equal to the square root of the original acid concentration.
- The $H^+$ concentration is the same as the original acid concentration. (correct)
- The $H^+$ concentration is half of the original acid concentration.
- The $H^+$ concentration is negligible compared to the original acid concentration.
What is the pH of a 0.001 M solution of hydrobromic acid (HBr)?
What is the pH of a 0.001 M solution of hydrobromic acid (HBr)?
An aqueous solution of $HClO_4$ has a pH of 2. What is the concentration of the acid?
An aqueous solution of $HClO_4$ has a pH of 2. What is the concentration of the acid?
Which of the following is a characteristic of strong bases in aqueous solution?
Which of the following is a characteristic of strong bases in aqueous solution?
Identify which of the following compounds is not a strong base?
Identify which of the following compounds is not a strong base?
A solution is labeled as 0.50 M KOH. What does this indicate about the composition of the solution?
A solution is labeled as 0.50 M KOH. What does this indicate about the composition of the solution?
The pH of a solution of NaOH is 12. What is the concentration of $H^+$ ions in this solution?
The pH of a solution of NaOH is 12. What is the concentration of $H^+$ ions in this solution?
The pH of a solution of Ca(OH)2 is 11. What is the pOH of this solution?
The pH of a solution of Ca(OH)2 is 11. What is the pOH of this solution?
A solution of KOH has a pH of 11.89. What is the concentration of the solution?
A solution of KOH has a pH of 11.89. What is the concentration of the solution?
For a solution of $Ca(OH)_2$ to have a pH of 11.68, what must be the concentration of the $Ca(OH)_2$?
For a solution of $Ca(OH)_2$ to have a pH of 11.68, what must be the concentration of the $Ca(OH)_2$?
Calculate the pH of a 0.050 M solution of nitric acid ($HNO_3$).
Calculate the pH of a 0.050 M solution of nitric acid ($HNO_3$).
Determine the concentration of $H^+$ in a solution of hydroiodic acid (HI) with a pH of 1.7.
Determine the concentration of $H^+$ in a solution of hydroiodic acid (HI) with a pH of 1.7.
What is the $OH^-$ concentration in a solution of 0.005 M NaOH?
What is the $OH^-$ concentration in a solution of 0.005 M NaOH?
Flashcards
Strong Acids
Strong Acids
Acids that completely ionize in solution, donating all their protons (H⁺).
Examples of Common Strong Acids
Examples of Common Strong Acids
HCl, HNO3, H2SO4, HBr, HI, HClO3, HClO4
[H+] in Strong Monoprotic Acids
[H+] in Strong Monoprotic Acids
For strong monoprotic acids, the concentration of H+ ions is equal to the initial concentration of the acid.
Common Strong Bases
Common Strong Bases
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pH Calculation Formula
pH Calculation Formula
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Complete Dissociation (Acids/Bases)
Complete Dissociation (Acids/Bases)
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Ca(OH)₂ Dissociation
Ca(OH)₂ Dissociation
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Monoprotic Acid
Monoprotic Acid
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Study Notes
Strong Acids
- Seven common strong acids exist, including six monoprotic acids and one diprotic acid.
- Common strong acids are:
- HCl - hydrochloric acid
- HNO₃ – nitric acid
- H₂SO₄ – sulfuric acid
- HBr - hydrobromic acid
- HClO₃ – chloric acid
- HI - hydroiodic acid
- HClO₄ – perchloric acid
- For a strong monoprotic acid, [H+] equals the original concentration of the acid.
- Nitric acid (HNO₃) is a strong, monoprotic acid, so the original acid concentration equals the concentration of hydrogen ions.
- pH of a 0.040 M solution of HClO₄ is 1.40.
- [H+] = 0.040 M
- pH = -log[H+]
- pH = -log(0.040)= 1.40
- An aqueous solution of HNO3 has a pH of 2.34, and the concentration of the acid is 4.57 × 10-3 M.
- pH = -log[H+]
- 2.34 = -log[H+]
- 10^-2.34 = [H+]= 0.00457 M
Strong Bases
- Most common strong bases are the ionic hydroxides of alkali metals (NaOH, KOH, etc.)
- Ionic hydroxides of the heavier alkaline metals, such as Sr(OH)₂, are also strong bases.
- Strong bases completely dissociate into ions in aqueous solution.
- A solution labeled 0.30 M NaOH consists of 0.30 M Na⁺(aq) and 0.30 M OH⁻(aq).
Calculating the pH of a Strong Base
- The pH of a 0.028 M solution of NaOH is 12.45.
- (H+)(0.028 M OH) = 1.0 × 10⁻¹⁴
- [H+] = 3.57 × 10⁻¹³ M
- -log (3.57 × 10⁻¹³) = pH
- Ca(OH)₂ dissociates to produce two OH- ions.
- The pH of a 0.0011 M solution of Ca(OH)2 is 11.34.
- (H+)(2 × 0.0011 M OH-) = 1.0×10⁻¹⁴
- [H+] = 4.55 × 10⁻¹² M
- -log (4.55 × 10⁻¹²) = pH
- The concentration of a solution of KOH is 7.8 x 10^-3 if the pH is 11.89.
- KOH is a strong base that dissociates to produce one OH-
- The concentration of a solution of Ca(OH)₂ is 2.38 × 10⁻³ M if the pH is 11.68
- Ca(OH)₂ is a strong base that dissociates to produce two OH-
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