Questions and Answers
How can the concentration of hydroxide ions in a solution be expressed in terms of the pOH value?
$pOH = -log[OH^-]$
How does the net direction of an acid-base reaction depend on relative acid and base strengths?
The reaction proceeds to the greater extent in the direction where a stronger acid and stronger base form a weaker acid and weaker base.
What is one way to determine the strength of acids based on their pH values?
Acid strength increases as the pH value decreases.
What happens to the strength of an acid as its percent ionization increases?
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What does percent ionization of an acid measure?
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How is the strength of a base determined from its pOH value?
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What role does water play in reactions with acids?
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What is the term for molecules or ions that can donate or accept a proton?
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In the autoionization reaction of water, what do some water molecules do?
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How does water behave when it reacts with the base NH3?
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Which species is the most important amphiprotic species?
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What happens to a water molecule when it accepts a proton?
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What is the key variable that determines the concentration of H3O+ in the Henderson-Hasselbach equation?
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In the Henderson-Hasselbach equation, what does pKa represent?
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What is the relationship described by the Henderson-Hasselbach equation for any conjugate acid-base pair?
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In a weak base dissociation, what does pKb represent?
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Which term in the Henderson-Hasselbach equation relates to the concentration of the weak acid?
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What does the Henderson-Hasselbach equation enable the calculation of for a buffer solution?
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What is the pH of a buffer solution containing 0.1 M CH₃COOH and a 0.1 M solution of CH₃COONa?
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If 1.0 mL of 0.10 M NaOH is added to 100 mL of the buffer in the first question, what will be the new pH?
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When 1.0 mL of 0.10 M HCl is added to 100 mL of the buffer in the previous question, what is the resulting pH?
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What is the purpose of a buffer solution?
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Why is a buffer solution made using an acid-base conjugate pair?
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How can a simple buffer solution be prepared?
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Why are the equilibrium concentrations of the acid and conjugate base assumed to be the same in a buffer solution?
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What role do acetic acid and sodium acetate play in a simple buffer solution?
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Why should a buffer solution not consume the acid and base components in a neutralization reaction?
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