Chemistry Solutions and Reactions Quiz

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Questions and Answers

How many grams of solute are present in 450 g of a 25% (w/w) solution?

112.5 g (correct)

125 g

112 g

75 g

If the density of a substance is 1.45 kg/dm³, what is the mass of 250 cm³ of this substance?

325 g

289 g

362.5 g (correct)

362 g

What is the mass fraction (w/w) of a solution with 112.5 g solute in 450 g of solution?

0.15

0.30

0.25 (correct)

0.20

What does the '25%' in a 25% (w/w) solution indicate?

25 g of solute in 100 g of solution Signup and view all the answers

How can the mass of a solute be derived from a 25% w/w solution?

Multiply the total mass by the solute percent converted to decimal Signup and view all the answers

What is the mass in grams of a substance with a density of 1.45 kg/dm³ and a volume of 0.25 dm³?

362.5 g Signup and view all the answers

If a substance has a density of 1.45 kg/dm³, how much volume in dm³ would 362.5 g of this substance occupy?

0.25 dm³ Signup and view all the answers

What is the density of a substance whose mass is 362.5 g and volume is 250 cm³?

1.45 kg/dm³ Signup and view all the answers

How many cubic centimeters are in 0.25 dm³?

250 cm³ Signup and view all the answers

What mass of substance can be measured if only 0.25 dm³ is available with a density of 1.45 kg/dm³?

362.5 g Signup and view all the answers

What is the process in which a compound loses electrons called?

Oxidation Signup and view all the answers

In a galvanic cell, which electrode is defined as the positive electrode?

Cathode Signup and view all the answers

According to Arrhenius theory, what defines an acid?

A compound that produces H+ ions in water Signup and view all the answers

What is the simplified form of the ion product of water at 25 °C?

Kw = [H3O+] x [OH-] Signup and view all the answers

What does Le Chatelier-Braun principle describe about equilibrium?

A system at equilibrium reacts to counteract changes applied to it. Signup and view all the answers

What happens to cations in a galvanic cell?

They move from the salt bridge to the cathode. Signup and view all the answers

What is defined as the process where metals are oxidized to oxides and sulphides?

Corrosion Signup and view all the answers

What does the pH formula -log [H+] represent?

The acidity of a solution Signup and view all the answers

What is the volume of a substance with a mass of 250 g and a density of 1.45 kg/dm³?

0.1724 dm³ Signup and view all the answers

Which formula represents the compound formed by the ions nitrite (NO2-) and iron (II) (Fe2+)?

Fe2(NO2)3 Signup and view all the answers

What is the mass of a substance that has a volume of 0.1724 dm³ and a density of 1.45 kg/dm³?

250 g Signup and view all the answers

What is the chemical formula for the compound formed from ammonium (NH4+) and carbonate ions (CO32-)?

NH4CO3 Signup and view all the answers

How is the volume of a substance related to its mass and density?

V = m/ρ Signup and view all the answers

Which ions combine to form the sulfate ion (SO42-)?

Sulphur and oxygen Signup and view all the answers

What is the density of a substance if its mass is 0.25 kg and its volume is 0.1724 dm³?

1.45 kg/dm³ Signup and view all the answers

Which of the following ions has a 3+ charge?

Iron (III) Signup and view all the answers

What defines a strong acid in chemistry?

An acid that completely dissociates in solution Signup and view all the answers

Which components make up an acidic buffer solution?

Weak acid and its salt Signup and view all the answers

What is the primary function of a buffer solution?

To maintain a constant pH Signup and view all the answers

Which term describes a mixture that contains a dispersed phase and a dispersion medium?

Colloidal system Signup and view all the answers

What process occurs when a salt is mixed with water breaking the ionic bond?

Hydrolysis Signup and view all the answers

Which of the following is an example of a strong base?

Calcium hydroxide Signup and view all the answers

What characterizes a weak acid?

It partially dissociates into ions Signup and view all the answers

What is hydration in chemistry?

A reaction involving water and a substance Signup and view all the answers

What factors influence the solubility of a gas in liquids?

Pressure Signup and view all the answers

How is osmotic pressure defined?

The pressure required to prohibit osmosis Signup and view all the answers

What characterizes an isotonic solution?

Equal concentration of solutes across a semipermeable membrane Signup and view all the answers

What is a hypertonic solution?

One with a higher concentration of solutes compared to the inside of a cell Signup and view all the answers

Which factors influence the reaction rate in a chemical reaction?

Temperature Signup and view all the answers

What is the definition of half-life in a chemical reaction?

The time required for the concentration to drop to half its initial value Signup and view all the answers

What describes catalysis?

A substance that increases the rate of a reaction Signup and view all the answers

What is the process of electrolysis?

Passed electric current through a substance to cause chemical change Signup and view all the answers

Study Notes

Unit Conversions

Mass conversions: milligrams (mg) to grams (g) and grams (g) to kilograms (kg)
A milligram (mg) is 1/1000 of a gram, and a gram (g) is 1/1000 of a kilogram.
Volume conversions: cubic centimeters (cm³) to cubic decimeters (dm³) and cubic decimeters (dm³) to cubic meters (m³)
A cubic centimeter (cm³) is 1/1000 of a cubic decimeter (dm³), and a cubic decimeter (dm³) is 1/1000 of a cubic meter (m³).
Amount of substance conversions: millimoles (mmol) to moles (mol)
A millimole (mmol) is 1/1000 of a mole.
Density conversions: grams per cubic centimeter (g/cm³) to kilograms per cubic meter (kg/m³)
Multiplying g/cm³ by 1000 converts it to kg/m³.
Pressure conversions: mega Pascals (MPa) to kiloPascals (kPa) and kiloPascals (kPa) to Pascals (Pa)
A megaPascal (MPa) is 1000 kiloPascals (kPa), and a kiloPascal (kPa) is 1000 Pascals (Pa).

Simple Calculation Tasks

Mass percentage/mass fraction: Calculate one quantity from given data.
- Mass fraction = (mass of substance) / (mass of substance + mass of water)
- Mass percentage = mass fraction x 100
Molar percentage/molar fraction: Calculate one quantity from given data.
- Molar fraction = (moles of substance)/(moles of substance + moles of solvent)
- Molar percentage = molar fraction x 100
Amount concentration (c): Amount concentration (c) = moles of substance / volume of solution (L)
Density (p): Density (p) = Mass of substance / Volume of solution (L or cm³)
Mass concentration (y): Mass concentration (y) = Mass of substance / Volume of solution (L or dm³)

Use of Mixing Equations

Calculating solute mass from solution mass and percentage.
Calculating mass from density and volume, or volume from mass and density.

Formulas of Inorganic Compounds

Provides formulas for various inorganic compounds based on given ions.

Inorganic Chemistry

Chlorine-containing disinfectants: Formulas and names.
Chlorine-free disinfectants: Formulas and names.
Ions causing water hardness: Mg²⁺, Ca²⁺.
Components of bleach: NaOCl, H₂O
Formula for chlorinated lime: Ca(OCl)₂

Kinetics

Defining reaction rate: The change in concentration of reactants or products per unit time.
Factors influencing reaction rates: Temperature, pressure, and concentration.
Defining half-life: The time taken for the concentration of a reactant to decrease to half of its initial value.
Defining catalysis: A substance that speeds up a chemical reaction without being consumed. Catalysis works by providing an alternative reaction path with a lower activation energy.
Defining inhibition: A substance that slows down or stops a chemical reaction by interfering with a catalyst. Inhibition typically involves blocking the catalyst's active site.

Electrolysis

Definition of electrolysis: The process of using an electric current to drive a non-spontaneous chemical reaction.
Explanation of galvanic cells: Cells that convert chemical energy to electrical energy through oxidation-reduction reactions.
Anode: The negative electrode where oxidation occurs, producing electrons (e⁻).
Cathode: The positive electrode where reduction occurs, consuming electrons (e⁻).
Oxidation: The loss of electrons.
Reduction: The gain of electrons.

Electrolysis (continued)

Combined electrode components (pH measurements): Glass electrode (depends on H⁺ concentration) and a reference electrode (known constant).
Metal corrosion: The oxidation of metals due to exposure to the environment.
Local cell formation: A galvanic cell that forms on a metal surface due to differences in its composition or environment.

Equilibria

Mass action law (e.g., for N₂ + 3H₂ = 2NH₃): K = [NH₃]² / ([N₂] x [H₂]³) indicating the equilibrium constant based on product concentration over reactant concentration.
Le Chatelier-Braun principle: Equilibrium shifts to counteract applied changes.
Acid definitions (Arrhenius, Brønsted-Lowry): Different ways to classify acids based on their behavior in water (producing H⁺ ions).

Equilibria (continued)

Ion product of water (K_w): 1.0 x 10⁻¹⁴ at 25°C and derived from the self-ionization constant of water.
Definition of pH: The negative decadic logarithm of the hydrogen ion concentration.
Definition of pOH: The negative decadic logarithm of the hydroxide ion concentration.
Weak acid: Partially dissociates into its ions in solution.
Strong acid: Completely dissociates into its ions in solution.

Buffers

Buffer solution use: Maintain a nearly constant pH despite additions of small amounts of acid or base.
Acidic buffer components: A weak acid and its conjugate base (salt).
Basic buffer components: A weak base and its conjugate acid (salt).
Hydrolyzing salts: Salts that react with water to produce an acidic or basic solution.

Acids and Bases

Examples of weak acids: Acetic, formic, phosphoric.
Examples of strong acids: Hydrochloric, sulfuric, nitric.
Examples of strong bases: Sodium hydroxide, potassium hydroxide, calcium hydroxide.
Examples of weak bases: Ammonia, lead(II) hydroxide, magnesium hydroxide.

Colloids

Defining colloidal systems: Mixtures with particles between 1 nm and 500 nm.
Emulsion: A mixture of immiscible liquids.
Suspension: A heterogeneous mixture of a solid dispersed in a liquid.
Defining adsorption: The change in concentration of a substance at a phase interface.
Hydration: A chemical reaction in which a substance reacts with water.

Miscellaneous

Defining chemical compound: The result of combining atoms with the same ratios.
Defining isotope: Atoms with the same atomic number but different numbers of neutrons.
Defining valence electrons: Electrons in the outermost shell of an atom.
Molecules where hydrogen bonding occurs: Involves F, O, or N atoms covalently bonded with hydrogen atoms.

Thermochemistry

Exothermic process: A process that releases heat to the surroundings, transferring thermal energy outward.
Endothermic chemical process: A process requiring heat to proceed, absorbing thermal energy from the surroundings.
Heat of combustion: The heat released when a substance is burned (oxidized) in excess oxygen.

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Description

Test your knowledge on solutions, mass fractions, and the properties of substances in this Chemistry quiz. It covers concepts such as weight/weight solutions, density calculations, and definitions related to acids and electrodes in galvanic cells. Perfect for students reviewing fundamental chemistry concepts!