Chem Final

Lactic acid

- CH3CHOHCOOH - weak - common uses: yogurt, acidulate (food additive to increase tartness); lotion additive

Acetic Acid

- CH3COOH - weak - common uses: vinegar, acidulant

Calcium hydroxide

- Ca(OH)2 - strong (not very soluble) - plaster; cement; water purification; agriculture

Lime

- CaO - produced by heating limestone

Limitations of the Arrhenius Theory

- H+ ions do not exist in water solution - Protons react with water to form hydronium ions - does not explain the basicity of ammonia - only applies to reactions in aqueous solutions

Carbonic Acid

- H2CO3 - weak - notes: unstable; formed in aqueous CO2

Sulfuric Acid

- H2SO4 - strong - leading chemical substance produced in the US (40 billion kg/year) - common uses: Battery acid, ore processing, fertilizer manufacturing, oil refining - notes: extremely corrosive

Boric Acid

- H3BO3 - very weak - antiseptic eye wash, roach poison

Phosphoric Acid

- H3PO4 - Moderate - Common uses: Manufacture of fertilizers; colas; rust removers

Hydrocyanic acid

- HCN - very weak - Common use: plastics manufacture; extremely toxic

Hydrochloric acid

- HCl - strong - annual US production = 4 billion kg/year - common uses: cleaning of meals, bricks; removing scale from boilers

Nitric Acid

- HNO3 - strong - common uses: manufacture of fertilizers, explosives

Hydrogen sulfate ion

- HSO4- - moderate - common uses: toilet bowl cleaners

Potassium hydroxide

- KOH - Strong - Making liquid soaps; absorbing CO2

Lithium Hydroxide

- LiOH - strong - alkaline storage batteries

Magnesium Hydroxide

- Mg(OH)2 - strong (not very soluble) - antacid, laxative

Ammonia

- NH3 - weak - production is about 11 billion kg/year - fertilizer, household cleansers

Sodium hydroxide

- NaOH - strong - aka "lye" - Annual US production is 9 billion kg - Acid neutralization; soap making; dehorning calve; Drano / Easy off

antacids

- Sodium bicarbonate (NaHCO3; baking soda) - calcium carbonate (CaCO3; Tums) - aluminum hydroxide ( Al(OH)3; amphojel) - magnesium hydroxide (Mg(OH)2; milk of magnesia)

Acids

- a molecular substance that ionizes in aqueous solution tp form Hydrogen ions -taste sour -turn litmus paper red -react with active metals to release hydrogen gas -react with bases to form water and a salt -can conduct electricity; are electrolytes

Bases

- a substance that produces hydroxide ions in aqueous solution -taste bitter - turn litmus paper blue - feel slippery -react with acids to from water and a salt

cement

- complex mixture of calcium and aluminum silicates - raw materials of limestone (CaCO3) and clay are mixed and heated

glass

- noncrystalline solid - made by heating sand, sodium carbonate, and limestone - properties can be varied by adding or replacing certain components - does not have sharp melting point

pH

- power of hydrogen - scale from 0 - 14 (acidic to basic) - negative logs - a means of expressing the acidity or basicity of a solution

Quartz

- pure silicon dioxide (SiO2) - macromolecular, extended lattice substance - ratio of oxygen to silicon is 2:1 - 3-D structure

Photochromic Glass

A type of smart glass that changes color when exposed to light; silver chloride (AgCl) and copper(I) chloride (CuCl) embedded in the glass.

A solution with a pH of 10 has a hydronium ion concentration of A) 10^-10 mol/L B) 10^10 mol/L C) 10 mol/L D) -10 mol/L

A) 10^-10 mol/L

Which substance is a common reducing agent used in the production of metals from ores? A) C B) Na2Cr2O7 C) H2O D) NaCl

A) C

When added to water, which of the following would produce a base? A) Na2O B) CO2 C) Cl2 D) SO3

A) Na2O

An unknown substance is added to a solution and the pH decreases. The substance is best described as a(n) A) acid B) base C) salt D) solvent

A) acid

Bronze is a(n) A) alloy. B) compound. C) element. D) pure substance.

A) alloy

Which of the following correctly summarizes the relative composition of the lithosphere with respect to inorganic and organic material? A) inorganic >> organic B) inorganic = organic C) inorganic << organic D) There is no organic matter in the lithosphere.

A) inorganic >> organic

Bronsted-Lowry Theory

Acids donate H+(protons) bases accept

Arrhenius Theory

Acids ionize in water to donate protons; bases ionize in water to produce hydroxide ions.

In the reaction Fe2O3 + 3 H2 → 2 Fe + 3 H2O the reducing agent is A) Fe2O3 B) H2 C) Fe D) H2O

B) H2

All of the following are bases EXCEPT A) KOH B) HNO3 C) LiOH D) Mg(OH)2

B) HNO3

HCN is classified as a weak acid in water. This means that it produces A) no hydronium ions B) a relatively small fraction of the maximum number of possible hydronium ions C) a relatively large fraction of the maximum number of possible hydronium ions D) 100% of the maximum number of possible hydronium ions

B) a relatively small fraction of the maximum number of possible hydronium ions

Many medicines have bitter taste which manufactures attempt to disguise. Many medicines are probably A) acids B) bases C) salts D) neutral

B) bases

Which material is characterized by a two dimensional sheet-like arrangement of SiO4 tetrahedra? A) asbestos B) mica C) glass D) quartz

B) mica

Aluminum is more reactive than iron, yet it is used today for a variety of applications in which iron would corrode (cans, rain gutters, etc.). The reason for the corrosion durability of aluminum is that A) aluminum does not react with oxygen. B) very unreactive aluminum oxide forms a thin layer on aluminum. C) aluminum does not undergo oxidation. D) all aluminum products are treated with a plastic coating.

B) very unreactive aluminum oxide forms a thin layer on aluminum.

In the photosynthesis reaction: 6 CO2 + 6 H2O → C6H12O6 + 6 O2, the substance that serves as the reducing agent is A) carbon dioxide. B) water. C) sunlight. D) glucose, C6H12O6.

B) water

An oxidizing agent that was used in older versions of the Breathalyzer test is A) NaHClO (sodium hypochlorite). B) O3 (ozone). C) K2Cr2O7 (potassium dichromate). D) AgBr (silver bromide).

C) K2Cr2O7 (potassium dichromate).

The lithosphere is the ________ part of the earth's crust. A) gaseous B) liquid C) solid D) water

C) Solid

In a reaction, the substance undergoing reduction serves as the A) electron donor. B) proton donor. C) oxidizing agent. D) reducing agent.

C) oxidizing agent.

The pH of a sample of water from a river is 6.0. A sample of effluent from a food processing plant has a pH of 4.0. The concentration of hydronium ion in the effluent is A) one and a half times (1.5x) larger than the river hydronium ion concentration. B) two times (2x) larger than the river hydronium ion concentration. C) four times (4x) larger than the river hydronium ion concentration. D) 100 times (100x) larger than the river hydronium ion concentration.

D) 100 times (100x) larger than the river hydronium ion concentration.

The black tarnish on silver is A) AgOH B) Ag2O C) AgCl D) Ag2S

D) Ag2S

This substance is a powerful oxidizing agent and a harmful pollutant; yet a layer of it in the upper stratosphere serves as a shield from harmful ultraviolet radiation from the sun. A) CO2 B) O2 C) SO3 D) O3 (ozone)

D) O3 (ozone)

What is the conjugate base of HSO3-? A) H2SO4 B) H2SO3 C) HSO4- D) SO3^2-

D) SO3^2-

The basic structural unit of silicates is A) SiO. B) SiO2. C) SiO3. D) SiO4.

D) SiO4.

As opposed to most solids, when glass is heated, it A) melts rapidly to a liquid over a narrow temperature range. B) goes directly into the gas phase; a process known as sublimation. C) separates into its individual components. D) gradually softens over a wide temperature range.

D) gradually softens over a wide temperature range.

H3O+ is the A) hydrate ion B) hydrogen ion C) hydroxide ion D) hydronium ion

D) hydronium ion

Hard water deposits (calcium carbonate) have built up around your bathroom sink. Which one of the following would be best to dissolve the deposit? A) ammonia B) bleach C) lye D) vinegar

D) vinegar

Oxidation

Loss of electrons, loss of hydrogen, gain of oxygen

Common Salts

Silver Nitrate, Calcium sulfate, Magnesium sulfate, Potassium permanganate, Zinc oxide, Ferrous Sulfate, Zinc Sulfate, Barium Sulfate

Common Bases

Sodium hydroxide, Potassium hydroxide, Lithium hydroxide, Calcium hydroxide, Magnesium hydroxide, Ammonia

Neutralization

When acid reacts with a base, the properties of each are neutralized and the products are water and a salt Acid + Base --> Water + Salt

Non metal oxides

acidic anhydrides

atmosphere

air surrounding earth

bronze

alloy of copper with about 10% tine; harder than copper

Which substance is the oxidizing agent in the following reaction? H2S + H2O2 → S + 2 H2O a. H2S b. H2O2 c. S d. H2O

b. H2O2

In the following reaction that takes place in batteries, which element is being reduced? Zn + 2 MnO2 + H2O → Zn2+ + Mn2O3 + 2 OH- a. Zinc b. Manganese c. The oxygen in MnO2 d. The oxygen in water e. The hydrogen in water

b. manganese

metal oxides

basic anhydrides

Which of the following processes would be considered oxidation? a. Addition of hydrogen b. Gain of electrons c. Loss of electrons d. Lowering of charge e. Loss of oxygen

c. loss of electrons

Chemical explosions

can be the result of redox reactions. Redox reactions that occur rapidly with the production of gases (such as nitrogen) are often explosive; fertilizer bomb

Oxidizing agents

cause oxidation

ceramics

clays (aluminum silicates) that have been shaped and fired to a hard, durable material

Micas

composed of linked SiO4 tetrahedra arranged in 2-D sheet-like array

conjugate acid-base pairs

compounds or ions that differ by one proton (H+) - related by loss and gain of H+ - one pair occurs in forward direction and the other in the reverse

buffer solutions

contain weak acid and conjugate base; capable of maintaining a nearly constant pH when small amounts of acid or base are added

malachite

copper hydroxide mineral

Earth's three main regions

core, mantle, crust

anodes

electrodes where oxidation occurs

cathodes

electrodes where reduction occurs

reduction

gain of electrons, gain of hydrogen, loss of oxygen

alkalosis

increase in the pH of blood because of excessive use of antacids

Fuel cells

interesting kind of battery. The fuel is oxidized at the anode and O2 is reduced at the cathode. The electrons are allowed to flow through a wire and do work.

Strong acids

ionize completely in water solution

lithosphere

land masses

core

largely iron and nickel; not accessible

organic lithosphere

living organisms, their waste and decomposition products, their fossilized remains

Anhydride

means "without water"; reactions its water produces an acid or a base

Weak acids

only partially ionize in water solution

photosynthesis

only process that produces the elemental oxygen that is essential for animals on Earth.

crust

outer shell; made up of lithosphere, hydrosphere and atmosphere

Top 3 elements that make up earth's surface

oxygen (53.3%); silicon (15.9%); Hydrogen (15.1%)

Acid rain

pH of less than 5.6; can destroy statues

electrodes

pieces of metal where electrons are transferred

Ozone (O3)

powerful oxidizing agent. In the lower atmosphere, it is harmful to both plants and animals. However, in the stratosphere, it serves to protect life on Earth from harmful ultraviolet radiation it is used in air and water purification

iron

produced from its ore using high temperature furnaces

self ionization

pure water has acid and base in it; a term describing the reaction in which two water molecules react to produce ions

Silicates

quartz, mica, asbestos

Silver tarnish

result of the oxide on the silver surface reacting with hydrogen sulfide in the air (H2S); leaving black film of silver sulfide (Ag2S0

inorganic part of lithosphere

rocks and minerals

mantle

silicates and a variety of metals

copper

sometimes found in the native, uncombined states; first metal to be obtained from its ore thought smelting

clinker

the stony residue from burnt coal or from a furnace

Nickel-cadmium batteries

used in portable radios and cordless appliances. They use cadmium anodes and nickel-oxide cathodes.

asbestos

various fibers silicates; best know as chyrotile (Magnesium silicate)

hydrosphere

water

hyperacidity

when the stomach secretes too much acid; antacids often taken to neutralize excess acid and reduce the symptoms