Nelson Science Perspectives 10
1st Edition
ISBN: 9780176355289
Textbook solutions
All Solutions
Page 296: Self-Quiz
Exercise 11
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Acids and bases are electrolytes because when dissolved in water, their ions become free to move can travel to their oppositely charged terminals in presence of a potential difference. This negative ions move to the positive electrode and lose their extra electron(s) there, which travels via the battery and gained by the positive ions at the negative electrode. This movement of electron(s) constitute a current and therefore acids and bases are called electrolytes.
Exercise 12
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Acid 1: Hydrochloric acid – HCl
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Acid 2: Sulfuric acid – H$_2$SO$_4$
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Acid 3: Phosphoric acid – H$_3$PO$_4$
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Base 1: Sodium hydroxide – NaOH
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Base 2: Magnesium hydroxide – Mg(OH)$_2$
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Base 3: Potassium hydroxide – KOH
Result
7 of 7
Click to see answers.
Exercise 13
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a.
Balanced chemical equation:
$$
mathrm{HNO_{3(aq)} + KOH_{(aq)} longrightarrow KNO_{3(aq)} + H_2O_{(l)}}
$$
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b.
Balanced chemical equation:
$$
mathrm{Ca(OH)_{2(aq)} + H_2SO_{4(aq)} longrightarrow CaSO_{4(aq)} + 2H_2O_{(l)}}
$$
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c.
Balanced chemical equation:
$$
mathrm{H_2SO_{4(aq)} + 2NaOH_{(aq)} longrightarrow Na_2SO_{4(aq)} + 2H_2O_{(l)}}
$$
Result
4 of 4
Click to see answers.
Exercise 14
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1. Strong acids are used as the solvent in wet batteries.
2. They are also used to remove corrosion (specially rust from iron) from metals during the recycling process. This process is known as pickling of metals.
3. Acids are used to make paints.
4. Acids are also used by food manufacturing companies as a preservative.
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1. Sodium hydroxide is used by manufacturing industries to make soap.
2. Borax is used to maintain the pH of pools.
3. Calcium hydroxide is used to manufacture cement.
4. Ammonia based solvents are used as cleaning agents in domestic cleaning products.
Result
3 of 3
Click to see answers.
Exercise 15
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a. and b.
In an acid base reaction, the hydrogen H$^+$ ion of the acid combine with the hydroxide OH$^-$ ion of the base to form a neutral product water.
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c. This reaction is called the neutralization reaction as the acidity of the acids caused by hydrogen ions is neutralized by the basic hydroxide ions of the base to yield a neutral product water.
Result
3 of 3
Click to see answers.
Exercise 16
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a. The pH of the pool is 8.2. This is greater than 7 and therefore this implies that pool water is basic in nature.
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b. Addition of chlorine to disinfect pool water often increases the pH of pool water.
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c. Sodium bisulfate also known as dry acid is used to decrease the high pH of pool water and bring it in the optimum required pH range.
Exercise 17
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For testing the pH of a household product, first wear gloves and lab glasses. Then take a sample of the household product in a clean, small bowl and test it using universal indicator (Any indicator can be used). If the color of the indicator is in shades of red and yellow then this implies that the product is acidic in nature, if the color of the indicator is in shades of blue then this implies that the product is basic in nature and if the color of the indicator is in shades of green then this implies that the product is neutral in nature.
Exercise 18
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Corrosion is directly affected by acidity. This means that the more the acidic a solvent is, the more corrosive it is. We know that the more the acidic a solvent is, the lower its pH is, therefore, in terms of pH, it can be concluded that the more the lower the pH of a solvent is, the more corrosive it is.
Result
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The more the lower the pH of a solvent is, the more corrosive it is.
Exercise 19
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In an acid base reaction, the hydrogen H$^+$ ion of the acid combine with the hydroxide OH$^-$ ion of the base to form a neutral product water. This reaction is called the neutralization reaction as the acidity of the acids caused by hydrogen ions is neutralized by the basic hydroxide ions of the base to yield a neutral product water of pH 7.
Exercise 20
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a. Electricity is generated in thermal power plants which are powered by the combustion of fossil fuels. This combustion of fossil fuels releases sulfur dioxide in the atmosphere and this is the main constituent of acid precipitation. Saving electrical energy by turning off the light on leaving an empty room can reduce the combustion of fossil fuel and there by reducing the amount of sulfur dioxide emission in the atmosphere.
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b. Using public transport to travel instead of personal cars can also reduce fossil fuel combustion and hence decrease sulfur dioxide emission in the atmosphere.
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b. Closing the refrigerator door immediately after use also conserves energy and there by reducing the amount of fossil fuel combustion in thermal power plants.
Result
4 of 4
Click to see answers.
Exercise 21
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a. pH of $5<7$ implies that these drinks are acidic in nature and can erode teeth enamel. Therefore, dentists discourage the use of these drinks because they are detrimental to teeth health.
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b. Water of pH 7 and fresh fruit juices are good substitutes to drinks. (Note that some fresh fruit juices are slightly acidic but not as acidic as commercially manufactured juices and drinks).
Result
3 of 3
Click to see answers.
Exercise 22
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In this question, we will give two environmental applications and two consumer applications on neutralizing reactions.
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Two environmental applications on neutralizing reactions are:\
begin{enumerate}
item Wasterwater treatment: used to reduce the damage created by the effluents.
item Antiacids tablets: used to balance the pH of the soil.
end{enumerate}
begin{enumerate}
item Wasterwater treatment: used to reduce the damage created by the effluents.
item Antiacids tablets: used to balance the pH of the soil.
end{enumerate}
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Two consumer applications on neutralizing reactions are:\
begin{enumerate}
item Vinegar: to treat wasp stings.
item Toothpaste: it helps to maintain healthy teeth from the decays formed from the acids.
end{enumerate}
Exercise 23
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Vinegar is a weak acid which corresponds to acid precipitation in this experiment. Chalk corresponds to stone monument in this experiment. When vinegar is gently poured over the chalk, it reacts with the chalk to erode it away, to represent how acid precipitation erodes away stone monuments and by extension, building and even metal structures.
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