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What are the 4 basic types of chemical reactions?
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What occurs during a Synthesis Reaction?
Two or more substances react to form a more complex product.
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What is the chemical equation for cellular respiration?
2H₂ + O₂ → 2H₂O
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What is the reaction for synthesis of oxy-haemoglobin?
Hb + O₂ → HbO₂
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Which type of reaction involves two or more substances reacting to form a more complex product?
Decomposition Reaction
Synthesis Reaction
Single Replacement Reaction
Double Replacement Reaction
Which type of reaction involves two or more substances reacting to form a more complex product?
Decomposition Reaction
Synthesis Reaction
Single Replacement Reaction
Double Replacement Reaction
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The basic types of chemical reactions are: - _______ - _______ - _______ - _______
The basic types of chemical reactions are: - Synthesis Reaction - Decomposition Reaction - Single Replacement Reaction - Double Replacement Reaction
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What are the products of the synthesis reaction in cellular respiration?
Water (H₂O)
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What is a decomposition reaction?
One reactant breaks down into two or more products.
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Provide an example of carbonic acid breakdown.
H₂CO₃(aq) → H₂O(l) + CO₂(g)
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Why is decomposition important for breathing?
CO₂ from cells forms carbonic acid in blood, then decomposes in lungs.
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What is the breakdown formula for hydrogen peroxide?
2H₂O₂ → 2H₂O + O₂
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What characterizes a single replacement reaction?
One element replaces another element in a compound.
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Provide an example of a single replacement reaction.
K + NaCl → KCl + Na
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What happens in a double replacement reaction?
The anions and cations of two compounds switch places.
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What are A and C in ion classification?
A and C are cations (positive ions).
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What are B and D in ion classification?
B and D are anions (negative ions).
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What is produced in the antacid reaction: NaHCO₃ + HCl?
Produces NaCl, H₂O, and CO₂.
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According to the Arrhenius Theory, an acid is any substance which releases _______ ions in water solution.
According to the Arrhenius Theory, an acid is any substance which releases H⁺ ions in water solution.
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According to Brønsted-Lowry Theory, an acid is any substance that donates a _______.
According to Brønsted-Lowry Theory, an acid is any substance that donates a proton.
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An example of an acid dissociating in water: HCl(aq) → _______ + Cl⁻(aq).
An example of an acid dissociating in water: HCl(aq) → H⁺(aq) + Cl⁻(aq).
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An example of a base dissociating in water: NaOH(aq) → _______ + _______.
An example of a base dissociating in water: NaOH(aq) → Na⁺(aq) + OH⁻(aq).
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In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), NH₃ acts as a _______ by accepting H⁺.
In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), NH₃ acts as a Brønsted-Lowry base by accepting H⁺.
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In the same reaction, H₂O acts as a _______ by donating H⁺.
In the same reaction, H₂O acts as a Brønsted-Lowry acid by donating H⁺.
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What defines conjugate acid-base pairs?
Acid donates H⁺, resulting in a conjugate base; base accepts H⁺, resulting in a conjugate acid.
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What is the Arrhenius definition of an acid?
Any substance which releases H⁺ ions in water solution.
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What is the Brønsted-Lowry definition of an acid?
Any substance which donates a proton.
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What is the Lewis definition of an acid?
Any substance which can accept an electron pair.
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What is the Arrhenius definition of a base?
Any substance which releases OH⁻ ions in water solution.
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What is the Brønsted-Lowry definition of a base?
Any substance which accepts a proton.
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What is the Lewis definition of a base?
Any substance which can donate an electron pair.
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For HCl in water: Arrhenius states HCl(aq) → H⁺(aq) + Cl⁻(aq). As a Brønsted-Lowry acid, it donates H⁺ to form H₃O⁺: HCl(aq) + H₂O(l) → _______(aq) + Cl⁻(aq). The Lewis definition involves H⁺ accepting an electron pair from H₂O.
For HCl in water: Arrhenius states HCl(aq) → H⁺(aq) + Cl⁻(aq). As a Brønsted-Lowry acid, it donates H⁺ to form H₃O⁺: HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq). The Lewis definition involves H⁺ accepting an electron pair from H₂O.
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When NH₃ is in water, the Brønsted-Lowry equation is: NH₃(aq) + H₂O(l) ⇌ _______(aq) + OH⁻(aq). As a Lewis acid, NH₃ acts similarly by forming NH₄⁺ and OH⁻.
When NH₃ is in water, the Brønsted-Lowry equation is: NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq). As a Lewis acid, NH₃ acts similarly by forming NH₄⁺ and OH⁻.
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What does NH₃ act as in Lewis theory?
A Lewis base by donating one electron pair.
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What role does H⁺ of H₂O play?
Acts as a Lewis acid by accepting one electron pair.
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What happens in the reaction BF₃ + :F⁻?
BF₃ accepts one electron pair, acting as a Lewis acid.
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What defines an amphoteric species?
A species that can act as both acid and base.
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What is the autoionisation reaction of water?
2 H₂O(l) ⇌ H₃O⁺(aq) + OH⁻(aq)
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What is the equilibrium expression for the autoionisation of water?
K = [H₃O⁺][OH⁻]/[H₂O]² ≈ [H₃O⁺][OH⁻] = 1.0×10⁻¹⁴.
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What are the properties of aqueous solutions based on [H₃O⁺] and [OH⁻]?
[H₃O⁺] > [OH⁻] indicates acidity; [H₃O⁺] = [OH⁻] indicates neutrality.
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In the reaction HCl(aq) + H₂O(l), H₂O acts as a _______.
In the reaction HCl(aq) + H₂O(l), H₂O acts as a base.
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In the reaction NH₃(aq) + H₂O(l), H₂O acts as an _______.
In the reaction NH₃(aq) + H₂O(l), H₂O acts as an acid.
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The reaction of HCO₃⁻ + H₂O results in _______ and _______.
The reaction of HCO₃⁻ + H₂O results in H₃O⁺ and CO₃²⁻.
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The reaction of HSO₄⁻ + H₂O results in _______ and _______.
The reaction of HSO₄⁻ + H₂O results in H₃O⁺ and SO₄²⁻.
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What is an alkaline solution characterized by?
[H₃O⁺] < [OH⁻]
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What happens to strong acids or bases in water?
Ionisation is essentially complete.
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What is the ionisation reaction for a strong acid?
HA(aq) + H₂O(l) → H₃O⁺(aq) + A⁻(aq)
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What happens with weak acids and bases in water?
Ionisation is incomplete (equilibrium).
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What is the expression for the ionisation constant of a weak acid (Kₐ)?
Kₐ = [H₃O⁺][A⁻] / [HA]
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What indicates a stronger acid regarding Kₐ?
The larger the Kₐ, the less weak the acid.
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What is the reaction for the ionisation of a weak base?
B(aq) + H₂O(l) ⇌ HB⁺(aq) + OH⁻(aq)
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What is the expression for the ionisation constant of a weak base (K<0xE1><0xB5><0xA7>)?
K<0xE1><0xB5><0xA7> = [HB⁺][OH⁻] / [B]
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What signifies a stronger base in terms of K<0xE1><0xB5><0xA7>?
The larger the K<0xE1><0xB5><0xA7>, the less weak the base.
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What is the equilibrium constant expression for the dissociation of HA in water?
Kₐ = \frac{[H₃O⁺][A⁻]}{[HA]}
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What is the equilibrium constant expression for the reaction of A⁻ with water?
Kₑ = \frac{[HA][OH⁻]}{[A⁻]}
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How is the equilibrium constant Kₕ for water defined?
Kₕ = \frac{[H₃O⁺][OH⁻]}{[H₂O]²}
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What relationship holds for the equilibrium constants of summed reactions?
Kₐ × Kₑ = Kₕ = 1.0×10⁻¹⁴
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The relationship between Ka and Kb shows that the stronger the acid or base, the weaker its conjugate partner, which can be expressed as: Kₕ = Kₐ × Kb = _______.
The relationship between Ka and Kb shows that the stronger the acid or base, the weaker its conjugate partner, which can be expressed as: Kₕ = Kₐ × Kb = 1.0×10⁻¹⁴.
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The acids and their corresponding bases that undergo complete ionization in water include perchloric acid, sulfuric acid, and hydrogen iodide, among others. For example, the conjugate base of sulfuric acid is _______.
The acids and their corresponding bases that undergo complete ionization in water include perchloric acid, sulfuric acid, and hydrogen iodide, among others. For example, the conjugate base of sulfuric acid is hydrogen sulfate ion.
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_______ and _______ can also be seen as conjugate acid-base pairs.
Hydronium ion and water can also be seen as conjugate acid-base pairs.
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Strong acids like Kₐ ≈ ∞ lead to their conjugate bases having Kₑ ≈ 0. For instance, the strong acid _______ results in a conjugate base with Kₑ ≈ 0.
Strong acids like Kₐ ≈ ∞ lead to their conjugate bases having Kₑ ≈ 0. For instance, the strong acid sulfuric acid results in a conjugate base with Kₑ ≈ 0.
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What is the mathematical operation that is the inverse of exponentiation?
Logarithm
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What is the formula for the logarithm?
logₐ(x) = y ⇒ x = aʸ
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What is the natural logarithm base?
e (approximately 2.718)
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If \(10^x = 100\), what is log₁₀ 100?
2
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What is log 1000?
3
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What is the formula for the Product Rule of logarithms?
logₐ(xy) = logₐ x + logₐ y
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What is the formula for the Quotient Rule of logarithms?
logₐ(x/y) = logₐ x - logₐ y
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What is the formula for the Power Rule of logarithms?
logₐ xᵖ = p logₐ x
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What is pKa in acid-base theory?
pKa = -log Kₐ
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What is the pKa value for Hydrogen Sulfate ion (HSO₄⁻)?
1.99
8.64
3.15
4.74
What is the pKa value for Hydrogen Sulfate ion (HSO₄⁻)?
1.99
8.64
3.15
4.74
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Which acid has the smallest Ka value?
Acetic acid (CH₃COOH)
Nitrous acid (HNO₃)
Phenol (C₆H₅OH)
Hydrogen Sulfate ion (HSO₄⁻)
Which acid has the smallest Ka value?
Acetic acid (CH₃COOH)
Nitrous acid (HNO₃)
Phenol (C₆H₅OH)
Hydrogen Sulfate ion (HSO₄⁻)
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What is the relationship between Ka and pKa?
When Ka is small, pKa is large and the acid does not dissociate significantly.
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What is a monoprotic acid?
An acid that donates one H⁺ per molecule in water, e.g., HCl, HNO₃.
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What is the reaction for HCl as a monoprotic acid?
HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq)
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What is a diprotic acid?
An acid that donates two H⁺ per molecule in water, e.g., H₂CO₃.
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What is the first ionization step for H₂CO₃?
H₂CO₃(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HCO₃⁻(aq) (Kₐ₁ = 4.5×10⁻⁷)
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What is the second ionization step for H₂CO₃?
HCO₃⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CO₃²⁻(aq) (Kₐ₂ = 1.0×10⁻²)
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What is a triprotic acid?
An acid that donates three H⁺ per molecule in water, e.g., H₃PO₄.
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What is the first ionization step for H₃PO₄?
H₃PO₄(aq) + H₂O(l) ⇌ H₃O⁺(aq) + H₂PO₄⁻(aq) (Kₐ₁ = 7.1×10⁻³)
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What is the second ionization step for H₃PO₄?
H₂PO₄⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HPO₄²⁻(aq) (Kₐ₂ = 6.3×10⁻⁸)
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What is the third ionization step for H₃PO₄?
HPO₄²⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + PO₄³⁻(aq) (Kₐ₃ = 4.2×10⁻¹³)
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What is a monoprotic base?
A base that accepts one H⁺, e.g., NaOH.
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What is the reaction for NaOH as a monoprotic base?
NaOH(aq) + H₂O(l) → Na⁺(aq) + H₂O(l) + OH⁻(aq)
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A diprotic acid donates _______ per molecule in water.
A diprotic acid donates two H⁺ per molecule in water.
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The first step for H₂SO₄ ionization is: H₂SO₄(aq) + H₂O(l) → H₃O⁺(aq) + _______(aq).
The first step for H₂SO₄ ionization is: H₂SO₄(aq) + H₂O(l) → H₃O⁺(aq) + HSO₄⁻(aq).
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The dissociation of calcium hydroxide in water can be represented as: \(\text{Ca(OH)}_2(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{Ca(OH)}^+(aq) + \text{H}_2\text{O}(aq) + \text{OH}^-(aq)\) with \(K_1 = _______}\).
The dissociation of calcium hydroxide in water can be represented as: \(\text{Ca(OH)}_2(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{Ca(OH)}^+(aq) + \text{H}_2\text{O}(aq) + \text{OH}^-(aq)\) with \(K_1 = 3.7 \times 10^{-6}\).
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In the second step of calcium hydroxide dissociation, \(\text{Ca(OH)}^+(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{Ca}^{2+}(aq) + \text{H}_2\text{O}(aq) + \text{OH}^-(aq)\), we have \(K_2 = _______}\).
In the second step of calcium hydroxide dissociation, \(\text{Ca(OH)}^+(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{Ca}^{2+}(aq) + \text{H}_2\text{O}(aq) + \text{OH}^-(aq)\), we have \(K_2 = 4.0 \times 10^{-2}\).
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What is stomach acid commonly represented by?
HCl
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Which substance acts as an antacid?
NaHCO₃
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What does lactic acid indicate?
Anaerobic metabolism
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In the blood buffer system, which acid is involved?
H₂CO₃
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What is the chemical structure of Vitamin C known as?
Ascorbic Acid
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What potential risk does too much Vitamin C pose?
Kidney-stone risk due to urine acidification.
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Amino acids are the building blocks of proteins and can act as both acids and bases, making them _______.
Amino acids are the building blocks of proteins and can act as both acids and bases, making them amphoteric.
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The structure of glycine, an amino acid, can act as a base in acidic solutions and as an acid in basic solutions, forming zwitterions: \(H_3N^+-CH(R)-COO^-\) which contains both _______ and _______.
The structure of glycine, an amino acid, can act as a base in acidic solutions and as an acid in basic solutions, forming zwitterions: \(H_3N^+-CH(R)-COO^-\) which contains both -COOH and -NH₂.
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What is the structure of glycine under acidic conditions?
Acts as a base, accepting H⁺.
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How does glycine behave in basic solutions?
Acts as an acid, donating H⁺.
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What is the chemical name of Aspirin?
Acetylsalicylic acid
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Is Aspirin acidic or basic?
Aspirin is acidic.
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How can Aspirin affect the stomach?
It can irritate the stomach lining.
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When is Aspirin often taken?
Often taken with food.
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In an acidic stomach, Aspirin remains _______ and is easily absorbed.
In an acidic stomach, Aspirin remains non-ionized and is easily absorbed.
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In a basic intestine, Aspirin becomes _______ and is _______.
In a basic intestine, Aspirin becomes ionized and is less absorbed.
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What is the chemical name of Paracetamol?
Acetaminophen
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Is Paracetamol acidic?
Not significantly acidic.
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How does Paracetamol affect the stomach compared to Aspirin?
It is gentler on the stomach.
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What are the 4 basic types of chemical reactions?
What occurs during a Synthesis Reaction?
Two or more substances react to form a more complex product.
What is the chemical equation for cellular respiration?
2H₂ + O₂ → 2H₂O
What is the reaction for synthesis of oxy-haemoglobin?
Hb + O₂ → HbO₂
Which type of reaction involves two or more substances reacting to form a more complex product?
Decomposition Reaction
Synthesis Reaction
Single Replacement Reaction
Double Replacement Reaction
The basic types of chemical reactions are: - Synthesis Reaction - Decomposition Reaction - Single Replacement Reaction - Double Replacement Reaction
What are the products of the synthesis reaction in cellular respiration?
Water (H₂O)
What is a decomposition reaction?
One reactant breaks down into two or more products.
Provide an example of carbonic acid breakdown.
H₂CO₃(aq) → H₂O(l) + CO₂(g)
Why is decomposition important for breathing?
CO₂ from cells forms carbonic acid in blood, then decomposes in lungs.
What is the breakdown formula for hydrogen peroxide?
2H₂O₂ → 2H₂O + O₂
What characterizes a single replacement reaction?
One element replaces another element in a compound.
Provide an example of a single replacement reaction.
K + NaCl → KCl + Na
What happens in a double replacement reaction?
The anions and cations of two compounds switch places.
What are A and C in ion classification?
A and C are cations (positive ions).
What are B and D in ion classification?
B and D are anions (negative ions).
What is produced in the antacid reaction: NaHCO₃ + HCl?
Produces NaCl, H₂O, and CO₂.
According to the Arrhenius Theory, an acid is any substance which releases H⁺ ions in water solution.
According to Brønsted-Lowry Theory, an acid is any substance that donates a proton.
An example of an acid dissociating in water: HCl(aq) → H⁺(aq) + Cl⁻(aq).
An example of a base dissociating in water: NaOH(aq) → Na⁺(aq) + OH⁻(aq).
In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), NH₃ acts as a Brønsted-Lowry base by accepting H⁺.
In the same reaction, H₂O acts as a Brønsted-Lowry acid by donating H⁺.
What defines conjugate acid-base pairs?
Acid donates H⁺, resulting in a conjugate base; base accepts H⁺, resulting in a conjugate acid.
What is the Arrhenius definition of an acid?
Any substance which releases H⁺ ions in water solution.
What is the Brønsted-Lowry definition of an acid?
Any substance which donates a proton.
What is the Lewis definition of an acid?
Any substance which can accept an electron pair.
What is the Arrhenius definition of a base?
Any substance which releases OH⁻ ions in water solution.
What is the Brønsted-Lowry definition of a base?
Any substance which accepts a proton.
What is the Lewis definition of a base?
Any substance which can donate an electron pair.
For HCl in water: Arrhenius states HCl(aq) → H⁺(aq) + Cl⁻(aq). As a Brønsted-Lowry acid, it donates H⁺ to form H₃O⁺: HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq). The Lewis definition involves H⁺ accepting an electron pair from H₂O.
When NH₃ is in water, the Brønsted-Lowry equation is: NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq). As a Lewis acid, NH₃ acts similarly by forming NH₄⁺ and OH⁻.
What does NH₃ act as in Lewis theory?
A Lewis base by donating one electron pair.
What role does H⁺ of H₂O play?
Acts as a Lewis acid by accepting one electron pair.
What happens in the reaction BF₃ + :F⁻?
BF₃ accepts one electron pair, acting as a Lewis acid.
What defines an amphoteric species?
A species that can act as both acid and base.
What is the autoionisation reaction of water?
2 H₂O(l) ⇌ H₃O⁺(aq) + OH⁻(aq)
What is the equilibrium expression for the autoionisation of water?
K = [H₃O⁺][OH⁻]/[H₂O]² ≈ [H₃O⁺][OH⁻] = 1.0×10⁻¹⁴.
What are the properties of aqueous solutions based on [H₃O⁺] and [OH⁻]?
[H₃O⁺] > [OH⁻] indicates acidity; [H₃O⁺] = [OH⁻] indicates neutrality.
In the reaction HCl(aq) + H₂O(l), H₂O acts as a base.
In the reaction NH₃(aq) + H₂O(l), H₂O acts as an acid.
The reaction of HCO₃⁻ + H₂O results in H₃O⁺ and CO₃²⁻.
The reaction of HSO₄⁻ + H₂O results in H₃O⁺ and SO₄²⁻.
What is an alkaline solution characterized by?
[H₃O⁺] < [OH⁻]
What happens to strong acids or bases in water?
Ionisation is essentially complete.
What is the ionisation reaction for a strong acid?
HA(aq) + H₂O(l) → H₃O⁺(aq) + A⁻(aq)
What happens with weak acids and bases in water?
Ionisation is incomplete (equilibrium).
What is the expression for the ionisation constant of a weak acid (Kₐ)?
Kₐ = [H₃O⁺][A⁻] / [HA]
What indicates a stronger acid regarding Kₐ?
The larger the Kₐ, the less weak the acid.
What is the reaction for the ionisation of a weak base?
B(aq) + H₂O(l) ⇌ HB⁺(aq) + OH⁻(aq)
What is the expression for the ionisation constant of a weak base (K<0xE1><0xB5><0xA7>)?
K<0xE1><0xB5><0xA7> = [HB⁺][OH⁻] / [B]
What signifies a stronger base in terms of K<0xE1><0xB5><0xA7>?
The larger the K<0xE1><0xB5><0xA7>, the less weak the base.
What is the equilibrium constant expression for the dissociation of HA in water?
Kₐ = \frac{[H₃O⁺][A⁻]}{[HA]}
What is the equilibrium constant expression for the reaction of A⁻ with water?
Kₑ = \frac{[HA][OH⁻]}{[A⁻]}
How is the equilibrium constant Kₕ for water defined?
Kₕ = \frac{[H₃O⁺][OH⁻]}{[H₂O]²}
What relationship holds for the equilibrium constants of summed reactions?
Kₐ × Kₑ = Kₕ = 1.0×10⁻¹⁴
The relationship between Ka and Kb shows that the stronger the acid or base, the weaker its conjugate partner, which can be expressed as: Kₕ = Kₐ × Kb = 1.0×10⁻¹⁴.
The acids and their corresponding bases that undergo complete ionization in water include perchloric acid, sulfuric acid, and hydrogen iodide, among others. For example, the conjugate base of sulfuric acid is hydrogen sulfate ion.
Hydronium ion and water can also be seen as conjugate acid-base pairs.
Strong acids like Kₐ ≈ ∞ lead to their conjugate bases having Kₑ ≈ 0. For instance, the strong acid sulfuric acid results in a conjugate base with Kₑ ≈ 0.
What is the mathematical operation that is the inverse of exponentiation?
Logarithm
What is the formula for the logarithm?
logₐ(x) = y ⇒ x = aʸ
What is the natural logarithm base?
e (approximately 2.718)
If \(10^x = 100\), what is log₁₀ 100?
2
What is log 1000?
3
What is the formula for the Product Rule of logarithms?
logₐ(xy) = logₐ x + logₐ y
What is the formula for the Quotient Rule of logarithms?
logₐ(x/y) = logₐ x - logₐ y
What is the formula for the Power Rule of logarithms?
logₐ xᵖ = p logₐ x
What is pKa in acid-base theory?
pKa = -log Kₐ
What is the pKa value for Hydrogen Sulfate ion (HSO₄⁻)?
1.99
8.64
3.15
4.74
Which acid has the smallest Ka value?
Acetic acid (CH₃COOH)
Nitrous acid (HNO₃)
Phenol (C₆H₅OH)
Hydrogen Sulfate ion (HSO₄⁻)
What is the relationship between Ka and pKa?
When Ka is small, pKa is large and the acid does not dissociate significantly.
What is a monoprotic acid?
An acid that donates one H⁺ per molecule in water, e.g., HCl, HNO₃.
What is the reaction for HCl as a monoprotic acid?
HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq)
What is a diprotic acid?
An acid that donates two H⁺ per molecule in water, e.g., H₂CO₃.
What is the first ionization step for H₂CO₃?
H₂CO₃(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HCO₃⁻(aq) (Kₐ₁ = 4.5×10⁻⁷)
What is the second ionization step for H₂CO₃?
HCO₃⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CO₃²⁻(aq) (Kₐ₂ = 1.0×10⁻²)
What is a triprotic acid?
An acid that donates three H⁺ per molecule in water, e.g., H₃PO₄.
What is the first ionization step for H₃PO₄?
H₃PO₄(aq) + H₂O(l) ⇌ H₃O⁺(aq) + H₂PO₄⁻(aq) (Kₐ₁ = 7.1×10⁻³)
What is the second ionization step for H₃PO₄?
H₂PO₄⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HPO₄²⁻(aq) (Kₐ₂ = 6.3×10⁻⁸)
What is the third ionization step for H₃PO₄?
HPO₄²⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + PO₄³⁻(aq) (Kₐ₃ = 4.2×10⁻¹³)
What is a monoprotic base?
A base that accepts one H⁺, e.g., NaOH.
What is the reaction for NaOH as a monoprotic base?
NaOH(aq) + H₂O(l) → Na⁺(aq) + H₂O(l) + OH⁻(aq)
A diprotic acid donates two H⁺ per molecule in water.
The first step for H₂SO₄ ionization is: H₂SO₄(aq) + H₂O(l) → H₃O⁺(aq) + HSO₄⁻(aq).
The dissociation of calcium hydroxide in water can be represented as: \(\text{Ca(OH)}_2(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{Ca(OH)}^+(aq) + \text{H}_2\text{O}(aq) + \text{OH}^-(aq)\) with \(K_1 = 3.7 \times 10^{-6}\).
In the second step of calcium hydroxide dissociation, \(\text{Ca(OH)}^+(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{Ca}^{2+}(aq) + \text{H}_2\text{O}(aq) + \text{OH}^-(aq)\), we have \(K_2 = 4.0 \times 10^{-2}\).
What is stomach acid commonly represented by?
HCl
Which substance acts as an antacid?
NaHCO₃
What does lactic acid indicate?
Anaerobic metabolism
In the blood buffer system, which acid is involved?
H₂CO₃
What is the chemical structure of Vitamin C known as?
Ascorbic Acid
What potential risk does too much Vitamin C pose?
Kidney-stone risk due to urine acidification.
Amino acids are the building blocks of proteins and can act as both acids and bases, making them amphoteric.
The structure of glycine, an amino acid, can act as a base in acidic solutions and as an acid in basic solutions, forming zwitterions: \(H_3N^+-CH(R)-COO^-\) which contains both -COOH and -NH₂.
What is the structure of glycine under acidic conditions?
Acts as a base, accepting H⁺.
How does glycine behave in basic solutions?
Acts as an acid, donating H⁺.
What is the chemical name of Aspirin?
Acetylsalicylic acid
Is Aspirin acidic or basic?
Aspirin is acidic.
How can Aspirin affect the stomach?
It can irritate the stomach lining.
When is Aspirin often taken?
Often taken with food.
In an acidic stomach, Aspirin remains non-ionized and is easily absorbed.
In a basic intestine, Aspirin becomes ionized and is less absorbed.
What is the chemical name of Paracetamol?
Acetaminophen
Is Paracetamol acidic?
Not significantly acidic.
How does Paracetamol affect the stomach compared to Aspirin?
It is gentler on the stomach.
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