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deck_19268925 Flashcards

(48 cards)

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1
Q

Name common acids found in homes, foods, and personal products.

A
  • Vinegar
  • Lemon
  • Body lotions
  • Hair conditioners
  • Toilet cleaner
  • Aspirin
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2
Q

List acids used in school laboratories.

A
  • Hydrochloric acid
  • Sulphuric acid
  • Nitric acid
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3
Q

Describe the properties of acids.

A
  • Sour taste
  • Can conduct electricity
  • React with alkalis
  • React with metals to form hydrogen gas
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4
Q

Explain the uses of acids.

A
  • Preserving food by preventing microorganism growth
  • Removing stains as cleaning agents (e.g. hydrochloric acid)
  • Making industrial chemicals like fertilizers, dyes, and paints (e.g. sulphuric acid)
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5
Q

Identify common household alkalis.

A
  • Glass cleaners
  • Kitchen cleaners
  • Drain cleaners
  • Baking soda
  • Toothpaste
  • Soap
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6
Q

List alkalis used in school laboratories.

A
  • Sodium hydroxide
  • Ammonia solution
  • Calcium hydroxide (limewater)
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7
Q

Describe the properties of alkalis.

A
  • Bitter taste
  • Slippery feel
  • Can conduct electricity
  • React with acids
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8
Q

Explain the uses of alkalis.

A
  • Removing grease (e.g., ammonia in kitchen and glass cleaners)
  • Making industrial chemicals like batteries (potassium hydroxide)
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9
Q

What safety precautions should be taken when handling acids and alkalis in the laboratory?

A
  • Read hazard warning labels on reagent bottles
  • Wear safety goggles and gloves
  • Pour waste into appropriate bottles
  • Wash hands thoroughly after experiments
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10
Q

Describe the steps to take if acids or alkalis come into contact with skin or eyes.

A
  • Wash affected area under slow running water for at least 10 minutes
  • Remove contaminated clothing
  • Wash eyes with eye wash bottle for at least 10 minutes
  • Call an ambulance for serious injuries
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11
Q

How does litmus indicator work?

A

Litmus solution and paper turn blue in alkaline conditions and red in acidic conditions.

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12
Q

What is a universal indicator?

A

A mixture of several indicators that shows a range of colors depending on the pH of the solution, available as a solution or pH paper.

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13
Q

Explain the pH scale.

A

A scale from 0 to 14 that measures acidity or alkalinity; lower pH indicates acidity, higher pH indicates alkalinity, pH 7 is neutral.

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14
Q

What does a pH value of 7 signify?

A

The solution is neutral.

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15
Q

Describe a pH meter.

A

A device with a probe connected to a digital display used to measure the pH value of a solution

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16
Q

What is the purpose of an er system in monitoring solutions?

A

It helps monitor the change in pH value of a solution.

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17
Q

Describe the process of neutralization.

A

Neutralization is the chemical reaction of mixing acids and alkalis together, which can change the acidity or alkalinity of a solution, resulting in a change in pH value.

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18
Q

Identify the reactants involved in a neutralization reaction.

A

The reactants are substances that take part in the reaction, such as acid and alkali.

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19
Q

Identify the products formed during neutralization.

A

The products are substances formed from the reaction, such as salt and water.

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20
Q

Write the general chemical equation for neutralization.

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A

Acid + alkali → salt + water.

21
Q

What is released during the process of neutralization?

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A

Heat is given out during neutralization.

22
Q

Does mass change during neutralization?

Study These Flashcards
A

No, mass is conserved in neutralization.

23
Q

Give an example of a neutralization reaction.

Study These Flashcards
A

Hydrochloric acid + sodium hydroxide → sodium chloride + water.

24
Q

Explain how neutralization is used to prevent tooth decay.

Study These Flashcards
A

Brushing teeth with slightly alkaline toothpaste neutralizes acids produced by bacteria in the mouth, which can cause tooth decay. Chewing sugar-free gum stimulates saliva, which is alkaline and neutralizes mouth acids.

25
Describe how neutralization helps relieve stomach upset.
Antacids containing alkalis neutralize excess hydrochloric acid in the stomach, reducing burning sensations caused by too much acid.
26
How are acids and alkalis used to treat insect stings or bites?
The treatment involves neutralizing the acids or alkalis present in the sting or bite area.
27
Explain the importance of neutralization in industrial waste management.
Industrial waste containing acids or alkalis can cause water pollution if discharged untreated. Neutralization with alkalis or acids helps to treat the waste before disposal.
28
Describe how pH regulation is achieved in soil.
If soil is too acidic, farmers add slaked lime (calcium hydroxide) to neutralize it. If too alkaline, sulfur is added to convert to sulfuric acid, balancing the pH for better plant growth.
29
What is the corrosive nature of acids?
Acids react with metals, often releasing hydrogen gas, which can be tested by using a burning splint.
30
How can you test for the presence of hydrogen gas?
Use a burning splint; if hydrogen is present, it will produce a popping sound.
31
Describe what happens when a burning splint is placed over a test tube containing hydrogen.
It burns with a 'pop' sound.
32
Explain the reaction between acids and metals.
Acids react with metals to produce salt and hydrogen gas, causing the metal to decrease slightly in size.
33
Provide an example of a reaction between hydrochloric acid and a metal.
Hydrochloric acid reacts with magnesium to produce magnesium chloride and hydrogen.
34
Identify which metal reacts strongly with acids and which does not.
Magnesium reacts strongly, while copper does not react.
35
Describe the reaction between acids and calcium carbonate in building materials.
Acids react with calcium carbonate to produce salt, carbon dioxide, and water.
36
Give an example of an acid reacting with calcium carbonate.
Sulphuric acid reacts with calcium carbonate to produce calcium sulphate, carbon dioxide, and water.
37
Define acid rain.
Rainwater that is slightly acidic with a pH less than 5.6, caused by pollutants like sulphur dioxide and nitrogen oxides from burning fossil fuels.
38
Explain how acid rain forms.
Pollutants like sulphur dioxide and nitrogen oxides dissolve in water droplets in the atmosphere, forming sulphuric acid and nitric acid, which then fall as acid rain.
39
Describe the environmental effects of acid rain.
It causes corrosion of metal objects and buildings, damages plants by destroying leaves and washing away nutrients, and harms aquatic life by increasing water acidity and dissolving harmful minerals.
40
Explain how acid rain affects aquatic life.
It increases water acidity, making it difficult for most aquatic organisms to survive, and dissolves harmful minerals that can slow their growth and reproduction.
41
Classify acids and alkalis based on their strength.
Strong acids include hydrochloric, sulphuric, and nitric acids; weak acids include citric, ethanoic, and carbonic acids. Strong alkalis include sodium hydroxide and potassium hydroxide; weak alkalis include ammonia solution.
42
Compare the corrosiveness of strong and weak acids and alkalis.
Strong acids and alkalis are more corrosive than weak ones; strong acids can corrode metal, skin, and flesh, especially when concentrated.
43
Describe proper handling precautions for household cleaners containing acids and alkalis.
Read precautions on containers, use in well-ventilated areas, never mix cleaners, and handle with care.
44
Explain how to safely dilute concentrated acids or alkalis.
Mix them slowly with water in a well-ventilated area, add acid or alkali to water (not water to acid/alkali), stir continuously, and wear safety gear.
45
List the safety precautions when diluting acids or alkalis.
Dilute in a well-ventilated area, wear safety goggles and gloves, add acid or alkali slowly to water, and stir continuously.
46
Identify actions to avoid when handling concentrated acids or alkalis.
Never add water directly to concentrated acids or alkalis, never dilute with bare hands, and never inhale vapors.
47
advantages of using a pH sensor
more accurate measurement, can be reused, can measure dark coloured liquids
48
disadvantages of using a pH sensor
more expensive, larger size, probe needs to be calibrated and need to be cleaned after use

Intergrated science (10 decks)

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