Chapter 8 part 1 : Acids Flashcards

1
Q

What is an acid?

A
  • An acid is a substance that produces hydrogen ions (H+) when dissolved in water.
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2
Q

What are the names and chemical formulae of some common acids?

A
  1. Hydrochloric acid:
    Chemical formula: HCl
  2. Nitric acid:
    Chemical formula: HNO3
  3. Sulfuric acid:
    Chemical formula: H2SO4
  4. Ethanoic acid:
    Chemical formula: CH3COOH
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3
Q

Do all acids produce hydrogen ions (H+) in an aqueous solution?

A
  • Yes, all acids produce hydrogen ions (H+) in an aqueous solution.
  • E.g. HCl (aq) โ€“> H+ (aq) + Cl (aq)
  • E.g. HNO3 (aq) โ€“> H+ (aq) + NO3- (aq)
  • E.g. H2SO4 (aq) โ€“> 2H+ (aq) + SO4 (square 2-) (aq)
  • E.g. CH3COOH (aq) โ€“>/<โ€“ H+ (aq) + CH3COO- (aq)
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4
Q

What are some properties of acids?

A

Acids:
- Have a sour taste.
- Conduct electricity due to the mobile ions produced when they dissolve in water.
- Turn blue litmus paper red.
- E.g. Lemons, oranges, hydrochloric acid, nitric acid, sulfuric acid, etcโ€ฆ

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5
Q

How are salts formed?

A
  • Acids react with some metals to form salts and hydrogen gas, and salts are also ionic compounds.
    ** Acid + metal โ€“> salt + hydrogen **
  • E.g. Hydrochloric acid + magnesium โ€“> magnesium chloride + hydrogen
    = 2 HCl (aq) + Mg (s) โ€“> MgCl2 (aq) + H2 (g)
  • E.g. Sulfuric acid + sodium โ€“> sodium chloride + hydrogen
    = H2SO4 (aq) + 2Na (s) โ€“> Na2SO4 (aq) + H2 (g)
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6
Q

How can acids react to form salts and hydrogen gas?

A
  • Acids react with some metals to form salts and hydrogen gas.
  • Salts are ionic compounds.
    ** Acid + metal โ€“> salt + hydrogen **
  • E.g. Hydrochloric acid + magnesium โ€“> magnesium chloride + hydrogen
    2 Hcl (aq) + Mg (s) โ€“> MgCl2 (aq) + H2 (g)
  • E.g. Sulfuric acid + sodium โ€“> sodium sulfate + hydrogen
    H2SO4 (aq) + 2Na (s) โ€“> MgCl2 (aq) + H2 (g)
  • E.g. Sulfuric acid + sodium โ€“> sodium sulfate + hydrogen
    H2SO4 (aq) + 2Na (s) โ€“> Na2SO4 (aq) + H2 (g)
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7
Q

How can the hydrogen gas produced during an acid and metal reaction be identified?

A
  • The hydrogen gas produced during the reaction of an acid with a metal can be identified by testing it with a burning splint.
  • The burning splint will then extinguish with a โ€˜popโ€™ sound.
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8
Q

What is an Acid + base โ€“> salts + water reaction?

A
  • Acids react with bases to from salts and water.
  • E.g. of bases: Metal oxides and metal hydroxides.
    **Acid + base โ€“> salt +water **
  • E.g. Nitric acid +magnesium oxide โ€“> magnesium nitrate + water
    2HNO3 (aq) + MgO (s) โ€“> Mg (NO3)2 (aq) + H2O (l)
  • E.g, Hydrochloric acid + potassium hydroxide โ€“> potassium chloride + water
    HCL (aq) + KOH (aq) + H2O (l)
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9
Q

What is a neutralisation reaction?

A
  • A neutralisation reaction is the reaction between an acid and a base.
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10
Q

What is an Acid + carbonates
โ€“> salts + water + carbon dioxide reaction?

A
  • Acids react with carbonates to form salts, water and carbon dioxide gas.
    ** Acid + carbonate โ€“> salt + water + carbon dioxide **
  • E.g. Hydrochloric acid + sodium carbonate โ€“> sodium chloride + water + carbon dioxide
    2HCl (aq) + NaCO3 (s) โ€“> 2NaCl (aq) + H2O (l) + CO2 (g)

-E.g. Nitric acid + calcium carbonate โ€“> calcium nitrate + water + carbon dioxide
2HNO3 (aq) + CaCO3 (s) โ€“> Ca (NO3)2 (aq) + H2O (l) + CO2 (g)

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11
Q

How can the carbon dioxide gas be identified during an acid and carbonate reaction?

A
  • The carbon dioxide gas produced during the reaction of an acid with a carbonate can be identified by bubbling it through limewater.
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12
Q

What is the salt formed in the reactions of/with acids?

A

The salt formed in the reactions of acids is:
- A chloride if hydrochloric acid is the reactant.
- A nitrate if nitric acid is present.
- A sulfate if sulfuric acid is the reactant.

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13
Q

What are some basic examples of strong and weak acids?

A
  • Strong acids are hydrochloride acid (HCl), nitric acid (NHO3), and sulfuric acid (H2SO4).
  • Weak acids are ethanoic acid (CH3COOH).
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14
Q

How do strong and weak acids ionise in an aqueous solution?

A
  • Strong acids ionise completely in aqueous solutions.
  • E.g. When 1 ole of HCl is dissolved in water, HCl ionises completely to form 1 mole of H+ ions, and 1 mole of Cl- ions.
    HCl (aq) โ€“> H+ (aq) + Cl- (aq)
  • Weak acids ionise partially in aqueous solutions.
  • E.g. When 1 mole of CH3COOH is dissolved in water, only a small amount of CH3COOH ionises partially to form H+ ions, and CH3COO- ions. Thus, at anytime there will be a mixture of CH3COOH molecules, H+ ions, and CH3COO- ions.
    **CH3COOH (aq) โ€“>/<โ€“ CH3COO- (aq) + H+ (aq) **
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15
Q

What does the โ€œstrength of an acidโ€ mean?

A
  • The strength of an acid means the extent of the ionisation of the acid in the aqueous solution, the smaller the extent of ionisation, the weaker the acid.
    ** - smaller = weaker
  • larger = stronger
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16
Q

Can the concentration of an acid be changed?

A
  • Yes, the concentration of an acid can be changed.
  • E.g. The concentration of ethanoic acid can be increased from 0.01 mol/dm3 to 1 mol/dm3 but the strength of an acid remains the same regardless of whether the acid is dilute/concentrated.
17
Q

Can strong and weak acids be dilute/concentration?

A
  • Yes, both strong and weak acids can be diluted/concentrated.
    Examples:
    1. 1 mol/dm3 HCl (aq)
    Degree of concentration: Dilute
    Strength of acid: Strong
    2. 12 mol/dm3 HCl (aq)
    Degree of concentration: Concentrated
    Strength of acid: Strong
    3. 1 mol/dm3 CH3COOH (aq)
    Degree of concentration: Dilute
    Strength of acid: Weak
    4. 12 mol/dm3 CH3COOH (aq)
    Degree of concentration: Concentrated
    Strength of acid: Weak