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Questions and Answers
What is the primary purpose of a universal indicator?
What is the primary purpose of a universal indicator?
- To neutralize acids and bases
- To indicate the presence of salts
- To measure the pH of a solution (correct)
- To create a color chart for base solutions
A universal indicator is made of a single type of indicator.
A universal indicator is made of a single type of indicator.
False (B)
What is the method used to determine the pH of a solution with a universal indicator?
What is the method used to determine the pH of a solution with a universal indicator?
A drop of the indicator is added to the solution and the color is matched with a color chart.
The process of combining an acid with a base to form a salt and water is called __________.
The process of combining an acid with a base to form a salt and water is called __________.
Match the following terms with their correct descriptions:
Match the following terms with their correct descriptions:
Which of the following indicators is most commonly extracted from lichens?
Which of the following indicators is most commonly extracted from lichens?
Synthetic indicators change color sharply when an acid is neutralized by an alkali.
Synthetic indicators change color sharply when an acid is neutralized by an alkali.
What is the pH value range for strong acids?
What is the pH value range for strong acids?
The pH scale ranges from ______ to ______.
The pH scale ranges from ______ to ______.
Match each pH range to its corresponding strength:
Match each pH range to its corresponding strength:
Which indicator is not suitable for titrations due to its gradual color change?
Which indicator is not suitable for titrations due to its gradual color change?
What relationship exists between the concentration of hydrogen ions and pH?
What relationship exists between the concentration of hydrogen ions and pH?
PH 7 indicates a strong alkaline solution.
PH 7 indicates a strong alkaline solution.
What characterizes a strong acid?
What characterizes a strong acid?
Hydrochloric acid is an example of a weak acid.
Hydrochloric acid is an example of a weak acid.
What is the chemical equation for the reaction between ethanoic acid and sodium hydroxide?
What is the chemical equation for the reaction between ethanoic acid and sodium hydroxide?
An acid is a proton (H+) __________.
An acid is a proton (H+) __________.
Match the acids to their associated products when reacting with magnesium:
Match the acids to their associated products when reacting with magnesium:
Which of the following statements is true about weak acids?
Which of the following statements is true about weak acids?
The concentration of an acid determines whether it is strong or weak.
The concentration of an acid determines whether it is strong or weak.
What is a base in terms of proton transfer?
What is a base in terms of proton transfer?
A concentrated solution of an acid contains a higher number of acid molecules per __________ of solution.
A concentrated solution of an acid contains a higher number of acid molecules per __________ of solution.
What product is formed when hydrochloric acid reacts with magnesium carbonate?
What product is formed when hydrochloric acid reacts with magnesium carbonate?
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Study Notes
Proton Transfer
- Acids are proton donors, releasing H+ ions in solutions, making the solution acidic.
- Bases are proton acceptors, taking H+ ions from acids.
Strong and Weak Acids
- Strong acids fully ionize in water, creating solutions with a low pH.
- Examples of strong acids are HCl and H2SO4.
- Weak acids partially ionize in water, resulting in solutions with pH closer to 7.
- Weak acids establish an equilibrium between the molecules and ions in water.
- Examples of weak acids include propanoic acid and ethanoic acid.
Acid-Base Reactions
- Reaction with Metals: Acid + Metal → Salt + Hydrogen
- Example: Magnesium + Hydrochloric acid → Magnesium chloride + Hydrogen
- Reaction with Bases: Acid + Base → Salt + Water
- Example: Magnesium hydroxide + Hydrochloric acid → Magnesium chloride + Water
- Reaction with Carbonates: Acid + Carbonate → Salt + Carbon dioxide + Water
- Example: Magnesium carbonate + Hydrochloric acid → Magnesium chloride + Carbon dioxide + Water
Indicators
- Indicators show the pH of substances.
- Litmus is a natural indicator extracted from lichens, turning red in acid and blue in alkali.
- Synthetic indicators, like thymolphthalein and methyl orange, are organic compounds showing distinct color changes in different pH ranges.
pH Scale
- The pH scale ranges from 0-14.
- Acids have a pH below 7, alkalis above 7.
- A neutral solution has a pH of 7.
- Strong acids have a low pH (0-2), while strong alkalis have a high pH (12-14).
- Universal indicators are mixtures of indicators used to determine the pH of a solution by matching the resulting colour to a chart.
- Lower pH indicates higher H+ ion concentration, and higher pH indicates higher OH- ion concentration.
Neutralization
- Neutralization is a reaction between an acid and a base, producing salt and water.
- The pH of the resulting solution is closer to neutral (pH 7).
- The neutralization reaction is a commonly used process in chemistry.
Titration
- Titration is a technique used to determine the concentration of an unknown solution using a solution of known concentration.
- A burette is used to deliver a known volume of the solution with known concentration (the titrant) into a flask containing the unknown solution (the analyte).
- The endpoint of the titration is the point at which the reaction is complete, indicated by a clear color change in the indicator.
- Titration is used in many chemical applications, including determining the concentration of acids and bases, measuring the amount of a substance in a sample, and monitoring chemical reactions.
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