Chemical Solutions and Salts Quiz

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Questions and Answers

Which type of salt is represented by the formula NaHCO₃?

  • Mixed salt
  • Basic salt
  • Normal salt
  • Acid salt (correct)

What is the pH of a solution formed by mixing 75 mL of 0.1 M CH₃COOH and 25 mL of 0.1 M NaOH?

  • 12.70
  • 4.70
  • 7.00
  • 8.85 (correct)

What happens to the solubility of a salt when a common ion is added?

  • Solubility decreases (correct)
  • Solubility increases
  • No change in solubility
  • Solubility remains constant

If the Ksp of AgCl is 10⁻¹⁰ (mol²/L²), what is the solubility of AgCl in 0.1 M AgNO₃?

<p>10⁻⁹ mol/L (C)</p> Signup and view all the answers

In the isohydric sol concept, how is the relative strength of two acids related?

<p>[H]₁/√Ka₁C₁ = [H]₂/√Ka₂C₂ (A)</p> Signup and view all the answers

When a mixture shows that Kjp > Ksp, what occurs?

<p>Precipitate forms (C)</p> Signup and view all the answers

How is the solubility of AgCl affected in a solution of 0.1 M CaCl₂ compared to pure water?

<p>It decreases (B)</p> Signup and view all the answers

What type of buffer is created by mixing acetic acid and sodium acetate?

<p>Acidic buffer (A)</p> Signup and view all the answers

What type of salt is represented by the formula K₂SO₄.Al₂(SO₄)₃.24H₂O?

<p>Double salt (B)</p> Signup and view all the answers

Which method is NOT a way to prepare an acidic buffer?

<p>Using a weak acid and strong acid (A)</p> Signup and view all the answers

What is the calculated pH when 50 mL of 2M acetic acid is mixed with 10 mL of 1M sodium acetate?

<p>4 (D)</p> Signup and view all the answers

In the reaction C(s) + CO₂(g) ⇌ 2CO(g), if the equilibrium pressure is 12 atm, what is the value of Kp?

<p>16 atm (A)</p> Signup and view all the answers

For the reaction NH₄HS(s) ⇌ NH₃(g) + H₂S(g) with an observed pressure of 1.12 atm, what is the value of Kp?

<p>0.3136 atm² (A)</p> Signup and view all the answers

Which of the following conjugate base pairs is correctly matched?

<p>H₂PO₄⁻ and HPO₄²⁻ (A)</p> Signup and view all the answers

What happens to the concentration of reactants when their concentration decreases according to Le Chatelier's principle?

<p>The reaction shifts towards the products (A)</p> Signup and view all the answers

In the equilibrium expression for $2NH₃ ightleftharpoons N₂ + 3H₂$, how are the moles of products calculated?

<p>By adding moles of N₂ and H₂ (C)</p> Signup and view all the answers

What is the resulting pH when mixing equal volumes of 0.02 M HOCI and 0.2 M CH₃COOH?

<p>2.7 (C)</p> Signup and view all the answers

When calculating the pH of a mixture of 0.01 M NaH₂PO₄ and 0.1 M Na₂HPO₄, what is the resulting pH?

<p>10.5 (A), 5.5 (B)</p> Signup and view all the answers

In a mixture of 10⁻¹ M HCl and 10⁻² M CH₃COOH, what is the calculated pH?

<p>3.4 (A)</p> Signup and view all the answers

What does the hydrolysis of CH₃COO⁻ in water produce?

<p>CH₃COOH and OH⁻ (B)</p> Signup and view all the answers

Which factor primarily determines whether the solution of a weak acid and strong base is acidic or basic after hydrolysis?

<p>The strength of the weak acid. (D)</p> Signup and view all the answers

What is the effect of increasing pressure on the equilibrium of the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?

<p>The reaction shifts to the right (A)</p> Signup and view all the answers

For an endothermic reaction, how does increasing the temperature affect the equilibrium?

<p>The equilibrium shifts to the right (A)</p> Signup and view all the answers

What happens to the equilibrium when an inert gas is added at constant pressure?

<p>The reaction shifts in the direction with more moles (B)</p> Signup and view all the answers

In the reaction H₂(g) + I₂(g) ⇌ 2HI(g), what is the value of Δn?

<p>0 (C)</p> Signup and view all the answers

In a reaction quotient Q, when is it equal to the equilibrium constant K?

<p>When Q = K (D)</p> Signup and view all the answers

What describes the degree of dissociation for the reaction A ⇌ 2B?

<p>x / 2 (C)</p> Signup and view all the answers

What role do Lewis acids perform in chemical reactions?

<p>Lone pair acceptors (A)</p> Signup and view all the answers

In the equilibrium constant expression Kc = [C]ʸ[D]ˢ / [A]ᵃ[B]ᵇ, what does the symbol Qc refer to when not at equilibrium?

<p>It reflects the concentrations of reactants and products at any point (A)</p> Signup and view all the answers

What is the pH of a 10⁻³ M HCl solution?

<p>3 (B)</p> Signup and view all the answers

What is the resulting pH when mixing 50 mL of HCl with 50 mL of H₂SO₄?

<p>0.7 (D)</p> Signup and view all the answers

Which of the following is a correct relationship in acid-base theory?

<p>Weak Base + H⁺ = Conjugate Acid (A)</p> Signup and view all the answers

Which equation correctly describes the relationship between pH and pOH at 25°C?

<p>pH + pOH = 14 (C)</p> Signup and view all the answers

For a weak polybasic acid such as phosphoric acid, what is true about its dissociation constants?

<p>Ka₁ &gt; Ka₂ &gt; Ka₃ (D)</p> Signup and view all the answers

What is the calculated pH for a solution with a hydrogen ion concentration of 10⁻⁸ M from HCl?

<p>6.9 (C)</p> Signup and view all the answers

In the context of acid-base theory, what is formed when a strong base reacts with a weak acid?

<p>A conjugate base and water (B)</p> Signup and view all the answers

When calculating the pH of a mixture of two weak acids, which formula would you use?

<p>[H⁺] = √(K₁C₁ + K₂C₂) (A)</p> Signup and view all the answers

Flashcards

Isohydric Solution

A solution containing two or more acids with the same hydrogen ion concentration. This means their [H+] is equal, even if the acids have different strengths or concentrations.

Normal Salt

A salt formed when a base neutralizes all the acidic hydrogen atoms of a polyprotic acid.

Acid Salt

A salt formed when a base neutralizes only part of the acidic hydrogen atoms of a polyprotic acid. This leaves some acidic hydrogen atoms remaining in the salt.

Basic Salt

A salt formed when a base is partially neutralized by an acid. This results in a salt containing OH⁻ ions.

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Double Salt

A salt formed by the combination of two or more salts. It's a single compound containing multiple cations and anions.

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Complex Salt

A salt containing a complex ion, a central metal ion surrounded by ligands (typically neutral molecules or anions) bonded to it.

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Solubility

The maximum concentration of a solute that can dissolve in a given solvent at a specific temperature.

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Solubility Product (Ksp)

The product of the ion concentrations raised to their stoichiometric coefficients in a saturated solution of a sparingly soluble salt. This is a constant value at a given temperature.

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Buffer Solution

A solution's ability to resist pH changes when small amounts of strong acid or base are added. It typically consists of a weak acid and its conjugate base or a weak base and its conjugate acid.

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Solubility Product Constant (Ksp)

The equilibrium constant that governs the solubility of a sparingly soluble ionic compound. It is the product of the ion concentrations raised to their stoichiometric coefficients. For example, for CaF2(s), Ksp = [Ca2+][F-]^2.

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Degree of Dissociation (α)

A measure of the extent to which a reaction proceeds to completion. A higher degree of dissociation indicates that more reactants have converted into products which is usually the case with stronger acids.

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Le Chatelier's Principle

The law states that if a change of condition (concentration, temperature, pressure) is applied to a system at equilibrium, the system will shift in a direction that relieves the stress.

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Kp (Equilibrium Constant in Terms of Partial Pressure)

An equilibrium constant expressed in terms of partial pressures of gaseous reactants and products. It specifically applies to reactions involving gases in equilibrium.

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Conjugate Acid-Base Pair

A pair of chemical species that differ by a single proton. The acid donates a proton and the base accepts a proton to form conjugate pairs.

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Degree of Dissociation (D.O.D)

The ratio of the equilibrium concentration (partial pressure) of a particular reactant or product to its initial concentration (partial pressure). It indicates the extent to which that species has reacted.

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Henderson-Hasselbalch Equation

The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log(base/acid). The pKa is the negative logarithm of the acid dissociation constant (Ka).

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Δn (Change in moles)

The change in the number of moles of gaseous reactants and products during a reaction. It determines the effect of pressure changes on equilibrium.

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Effect of Pressure on Equilibrium (Δn < 0)

The reaction will shift to the side with fewer moles of gas to relieve pressure.

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Effect of Pressure on Equilibrium (Δn > 0)

The reaction will shift to the side with more moles of gas to relieve pressure.

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Effect of Pressure on Equilibrium (Δn = 0)

The reaction will not shift, regardless of pressure changes.

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Reaction Quotient (Qc)

The ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients, at any point during a reaction, but not at equilibrium.

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Equilibrium (Qc = Kc)

Qc = Kc. The reaction is at equilibrium.

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Shift Backward (Qc > Kc)

Qc > Kc. The reaction will shift backward (to the left) to reach equilibrium.

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Shift Forward (Qc < Kc)

Qc < Kc. The reaction will shift forward (to the right) to reach equilibrium.

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pH

The negative logarithm of the hydrogen ion concentration ([H+]) in a solution. It measures the acidity of a solution.

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pOH

The negative logarithm of the hydroxide ion concentration ([OH-]) in a solution. It measures the basicity of a solution.

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Kw

The product of the hydrogen ion concentration ([H+]) and the hydroxide ion concentration ([OH-]) in a solution. It is a constant value at a given temperature. The higher the temperature the higher the value.

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pH of a strong acid

The pH of a solution containing only a strong acid, where the [H+] is solely determined by the acid's concentration.

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pH of a weak monobasic acid

The pH of a solution containing a weak monobasic acid. This involves calculating the [H+] based on the acid's ionization constant (Ka) and concentration.

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pH of a weak polybasic acid

The pH of a solution containing a weak polybasic acid. This involves considering the multiple ionization steps and their respective Ka values.

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pH of a mix of strong acids

The pH of a solution containing a mix of two strong acids or one strong acid and one strong base.

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pH of WA + SA Mix

The pH of a solution containing a weak acid (WA) and a strong acid (SA) is determined by the stronger acid, but the weak acid also contributes slightly to the [H+].

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pH of WB + SB Mix

Calculating the pH of a solution containing a weak base (WB) and a strong base (SB) is similar to determining the pH of a WA and SA mix. The stronger base dominates the [OH-] while the weaker base impacts it minimally.

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pH of Amphiprotic Species

Amphiprotic species can act as both an acid and a base, depending on the conditions. When determining the pH of an amphiprotic salt solution, consider the relative values of K1 and K2 to find the predominant acidic/basic form.

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Salt Hydrolysis

The pH of a salt solution is determined by the hydrolysis of the ions it contains. Anionic hydrolysis occurs when an anion reacts with water, resulting in a basic solution. Cationic hydrolysis involves a cation reacting with water, producing an acidic solution.

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Basic and Acidic Salt

Salts formed from weak acid and strong base reactions are basic due to anionic hydrolysis, while those from strong acid and weak base reactions are acidic due to cationic hydrolysis.

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Study Notes

Types of Salts

  • Normal salts: Examples include NaCl, Na₂SO₄, and Na₃PO₄.
  • Acid salts: Examples include NaHCO₃ and NaHSO₄.
  • Basic salts: Examples include Zn(OH)Cl and Mg(OH)Cl.
  • Double salts: Example is K₂SO₄·Al₂(SO₄)₃·24H₂O (Potash alum).
  • Complex salts: Examples include [Ag(NH₃)₂]Cl and [Cu(NH₃)₄]SO₄.
  • Mixed salts: Examples include NaKS and NaKRbPO₄.

Isohydric Solutions

  • Solutions having the same [H⁺] concentration.
  • [Ka₁][C₁] = [Ka₂][C₂]

Relative Strengths of Acids

  • The relative strength of acids is related to their H⁺ ion concentrations
  • R.S = [H⁺]√Ka₁/Ka₂

Buffer Solutions

  • Mixtures of a weak acid and its salt, or a weak base and its salt, resist changes in pH.
  • These solutions are important in many chemical and biological systems, as they maintain a relatively constant pH.

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