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Questions and Answers
What is the pH of a solution that is neither acidic nor basic?
What type of reaction involves the transfer of H+ ions?
What is a characteristic of strong acids?
What is the result of a neutralization reaction?
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What happens to the concentration of H+ ions when the pH of a solution decreases by one unit?
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What type of acid is HCl?
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Study Notes
pH Scale
- pH is a measure of the concentration of hydrogen ions (H+) in a solution
- pH scale ranges from 0 to 14
- pH 7 is neutral (neither acidic nor basic)
- pH below 7 is acidic (high concentration of H+ ions)
- pH above 7 is basic (low concentration of H+ ions)
- Each step down the pH scale represents a 10-fold increase in H+ ion concentration
- Each step up the pH scale represents a 10-fold decrease in H+ ion concentration
Acid-Base Reactions
- Acid-base reactions involve the transfer of H+ ions
- Acids donate H+ ions (proton donors)
- Bases accept H+ ions (proton acceptors)
- Types of acid-base reactions:
- Neutralization: acid + base → salt + water
- Acid-carbonate reaction: acid + carbonate → salt + water + CO2
- Acid-metal reaction: acid + metal → salt + hydrogen gas
Strong and Weak Acids
- Strong acids:
- Completely dissociate in water to produce H+ ions
- Examples: HCl, HNO3, H2SO4
- Strong acids are strong electrolytes
- Weak acids:
- Partially dissociate in water to produce H+ ions
- Examples: CH3COOH, HF, H2CO3
- Weak acids are weak electrolytes
Neutralization
- Neutralization is a reaction between an acid and a base to form a salt and water
- General equation: acid + base → salt + water
- Examples:
- HCl (acid) + NaOH (base) → NaCl (salt) + H2O
- H2SO4 (acid) + Ca(OH)2 (base) → CaSO4 (salt) + H2O
- Neutralization reactions are exothermic, meaning they release heat
pH Scale
- pH measures the concentration of hydrogen ions (H+) in a solution, ranging from 0 to 14
- pH 7 is neutral, pH below 7 is acidic (high H+ ion concentration), and pH above 7 is basic (low H+ ion concentration)
- Each step down the pH scale represents a 10-fold increase in H+ ion concentration, and each step up represents a 10-fold decrease
Acid-Base Reactions
- Acid-base reactions involve the transfer of H+ ions, with acids donating H+ ions and bases accepting them
- Types of acid-base reactions include:
- Neutralization: acid + base → salt + water
- Acid-carbonate reaction: acid + carbonate → salt + water + CO2
- Acid-metal reaction: acid + metal → salt + hydrogen gas
Strong and Weak Acids
- Strong acids:
- Completely dissociate in water to produce H+ ions
- Examples: HCl, HNO3, H2SO4
- Strong acids are strong electrolytes
- Weak acids:
- Partially dissociate in water to produce H+ ions
- Examples: CH3COOH, HF, H2CO3
- Weak acids are weak electrolytes
Neutralization
- Neutralization is a reaction between an acid and a base to form a salt and water
- General equation: acid + base → salt + water
- Examples:
- HCl (acid) + NaOH (base) → NaCl (salt) + H2O
- H2SO4 (acid) + Ca(OH)2 (base) → CaSO4 (salt) + H2O
- Neutralization reactions are exothermic, releasing heat
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Description
Test your knowledge of pH scale and acid-base reactions, including concentration of hydrogen ions and acidic/basic solutions.
