Solutions and their properties
this part of a solution is present in the greater amount and does the dissolving.
What is the solvent?
This factor increases the rate of a chemical reaction by lowering the activation energy.
What is a catalyst?
This type of substance donates a proton (H⁺) in a chemical reaction.
What is a Brønsted–Lowry acid?
What is the molarity of a solution that contains 2.0 moles of NaCl in 1.0 L of solution?
What is 2.0 M?
A red blood cell placed in this type of solution will swell and may burst, a process called hemolysis.
What is a hypotonic solution?
When dissolved in water, this type of solute produces ions and conducts electricity.
What is an electrolyte?
In a reversible reaction at equilibrium, the rates of the forward and reverse reactions are...?
What are equal?
Identify the conjugate base in this reaction:
NH₄⁺ + H₂O ⇌ NH₃ + H₃O⁺
What is NH₃?
How many mL of 6.0 M HCl are needed to make 500 mL of a 1.5 M solution?
What is 125 mL?
(Use M₁V₁ = M₂V₂ → (6.0)(V₁) = (1.5)(500))
Given K = 10 for the reaction A ⇌ B, and [A] = 0.2 M at equilibrium, what is [B]? (Assume only A was initially present).
What is [B] = 0.2x / (1 - x), solve for x when K = 10?
This type of solution has not reached the maximum amount of solute that can dissolve at a given temperature.
What is an unsaturated solution?
If K is much greater than 1, the reaction favors which side?
What are the products?
This type of acid dissociates completely in water and produces a high concentration of H⁺.
What is a strong acid?
For the reaction A ⇌ B, if [A] = 0.10 M and [B] = 0.40 M at equilibrium, what is K?
What is 4.0?
(K = [B]/[A] = 0.40/0.10)
This type of solution resists changes in pH when small amounts of acid or base are added.
What is a buffer?
You have 2.0 L of a 0.50 M NaCl solution. How many moles of NaCl are present?
What is 1.0 mole?
According to Le Châtelier’s Principle, increasing the concentration of a reactant will shift the equilibrium in this direction.
What is to the right (toward the products)?
What is the pH of a solution with [H⁺] = 1.0 × 10⁻⁴ M?
What is 4?
Find the [H⁺] concentration of a solution with pH = 3.2.
What is 6.3 × 10⁻⁴ M?
([H⁺] = 10⁻³.²)
Calculate the pH of a buffer that is 0.25 M acetic acid (Ka = 1.8×10⁻⁵) and 0.30 M sodium acetate.
What is pH ≈ 4.86?
(Use Henderson–Hasselbalch: pH = pKa + log([A⁻]/[HA])
pKa = –log(1.8×10⁻⁵) ≈ 4.74
→ pH = 4.74 + log(0.30/0.25))
Adding salt to water increases this property and decreases the freezing point.
What is the boiling point?
For the reaction: N₂ + 3H₂ ⇌ 2NH₃, if [N₂] = 0.2 M, [H₂] = 0.3 M, and [NH₃] = 0.4 M, what is the value of K?
What is K = (0.4)² / (0.2)(0.3)³ = 0.16 / 0.0054 ≈ 29.63?
You titrate 25.0 mL of HCl with 0.100 M NaOH. It takes 30.0 mL of NaOH to reach the endpoint. What is the molarity of the HCl?
What is 0.120 M? (Use M₁V₁ = M₂V₂)
If it takes 25.0 mL of 0.200 M NaOH to neutralize 50.0 mL of an HCl solution, what is the molarity of the HCl?
What is 0.100 M?
(M₁V₁ = M₂V₂ → (0.200)(25.0) = M₁(50.0))
You have a 0.0025 M HNO₃ solution.
Calculate the pH of this solution.
(Assume complete dissociation; HNO₃ is a strong acid.)
What is pH ≈ 2.60?