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Questions and Answers
Which statement best describes the relationship between pH, $[H^+]$ concentration, and acidity?
Which statement best describes the relationship between pH, $[H^+]$ concentration, and acidity?
- Lower pH indicates higher $[H^+]$ concentration and increased acidity. (correct)
- Higher pH indicates lower $[H^+]$ concentration and increased acidity.
- Higher pH indicates higher $[H^+]$ concentration and increased acidity.
- Lower pH indicates lower $[H^+]$ concentration and increased acidity.
A solution has a pH of 3.0. If water is added to dilute the solution, which of the following is most likely to occur?
A solution has a pH of 3.0. If water is added to dilute the solution, which of the following is most likely to occur?
- The pH will approach 7.0. (correct)
- The pH will become more acidic.
- The pH will remain constant.
- The pH will decrease.
Which of the following is the best example of an amphoteric substance?
Which of the following is the best example of an amphoteric substance?
- Sodium hydroxide (NaOH)
- Water ($H_2O$) (correct)
- Ammonia ($NH_3$)
- Hydrochloric acid (HCl)
In a titration experiment, 20.0 mL of 0.1 M HCl is required to neutralize 10.0 mL of a NaOH solution. What is the molarity of the NaOH solution?
In a titration experiment, 20.0 mL of 0.1 M HCl is required to neutralize 10.0 mL of a NaOH solution. What is the molarity of the NaOH solution?
A buffer solution is prepared using a weak acid HA and its conjugate base $A^-$. If the $pK_a$ of HA is 4.5, at what pH will the concentrations of HA and $A^-$ be equal?
A buffer solution is prepared using a weak acid HA and its conjugate base $A^-$. If the $pK_a$ of HA is 4.5, at what pH will the concentrations of HA and $A^-$ be equal?
Which of the following statements accurately describes the role of buffers in biological systems?
Which of the following statements accurately describes the role of buffers in biological systems?
What is the pH of a neutral solution at standard conditions?
What is the pH of a neutral solution at standard conditions?
Which of the following statements correctly distinguishes between strong and weak acids?
Which of the following statements correctly distinguishes between strong and weak acids?
Which of the following is a correct application of the Bronsted-Lowry acid-base theory?
Which of the following is a correct application of the Bronsted-Lowry acid-base theory?
A solution with a pH of 9 is considered:
A solution with a pH of 9 is considered:
Flashcards
Acids
Acids
Substances that donate protons (H+) or accept electrons.
Bases
Bases
Substances that accept protons (H+) or donate electrons.
Acid-base reactions
Acid-base reactions
Reactions involving the transfer of protons from an acid to a base.
Arrhenius acids
Arrhenius acids
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Arrhenius bases
Arrhenius bases
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Bronsted-Lowry acids
Bronsted-Lowry acids
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Bronsted-Lowry bases
Bronsted-Lowry bases
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pH
pH
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Buffers
Buffers
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Amphoteric substances
Amphoteric substances
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Study Notes
- Chemical reactions involve the rearrangement of atoms and molecules to form new substances
- Reactants are the initial substances that participate in a chemical reaction
- Products are the substances formed as a result of a chemical reaction
- Chemical equations represent chemical reactions using symbols and formulas
- Balancing chemical equations ensures that the number of atoms of each element is the same on both sides of the equation, obeying the law of conservation of mass.
- Stoichiometry is the quantitative study of reactants and products in chemical reactions
- The mole is the SI unit for the amount of a substance
- Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol)
- Limiting reactant is the reactant that is completely consumed in a reaction and determines the amount of product formed
- Excess reactant is the reactant present in a greater amount than necessary to react with the limiting reactant
- Theoretical yield is the maximum amount of product that can be formed from a given amount of reactants, assuming complete conversion
- Actual yield is the amount of product actually obtained from a reaction
- Percent yield is the ratio of actual yield to theoretical yield, expressed as a percentage
- Acids are substances that donate protons (H+) or accept electrons.
- Bases are substances that accept protons (H+) or donate electrons.
- Acid-base reactions involve the transfer of protons from an acid to a base.
- Arrhenius acids produce H+ ions in aqueous solutions.
- Arrhenius bases produce OH- ions in aqueous solutions.
- Bronsted-Lowry acids are proton donors.
- Bronsted-Lowry bases are proton acceptors.
- Lewis acids accept electron pairs.
- Lewis bases donate electron pairs.
- Conjugate acid-base pairs consist of two substances that differ by the presence of a proton.
- Amphoteric substances can act as both acids and bases.
- Water is a common amphoteric substance.
- Strong acids completely dissociate into ions in aqueous solutions.
- Weak acids only partially dissociate into ions in aqueous solutions.
- Strong bases completely dissociate into ions in aqueous solutions.
- Weak bases only partially dissociate into ions in aqueous solutions.
- pH is a measure of the acidity or basicity of a solution.
- pH is defined as the negative logarithm (base 10) of the hydrogen ion concentration ([H+]).
- pH = -log[H+]
- A pH of 7 is neutral.
- A pH less than 7 is acidic.
- A pH greater than 7 is basic or alkaline.
- The pH scale typically ranges from 0 to 14.
- Acidic solutions have a higher concentration of H+ ions than OH- ions.
- Basic solutions have a higher concentration of OH- ions than H+ ions.
- Neutral solutions have equal concentrations of H+ and OH- ions.
- Indicators are substances that change color depending on the pH of the solution.
- Litmus paper is a common pH indicator.
- pH meters are electronic devices used to measure pH accurately.
- Acid-base titrations are used to determine the concentration of an acid or a base by neutralizing it with a solution of known concentration.
- The equivalence point in a titration is the point at which the acid and base have completely reacted with each other.
- Buffers are solutions that resist changes in pH upon the addition of small amounts of acid or base.
- Buffers typically consist of a weak acid and its conjugate base, or a weak base and its conjugate acid.
- The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of the weak acid and the ratio of the concentrations of the acid and its conjugate base.
- pKa is the negative logarithm (base 10) of the acid dissociation constant (Ka).
- The Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the weak acid.
- Buffers are important in biological systems to maintain a stable pH for biochemical reactions.
- The pH of blood is tightly regulated by buffer systems.
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