How does shaking or stirring a mixture of solute and solvent affect a solution?
Answer: It increases the rate of dissolving
Chemistry Chapter | Multiple Choice | Questions and Answers | Test Bank
Answer: It increases the rate of dissolving
Answer: Agitating the solution
Answer: Boiling point elevation
Answer: Measure of the amount of solute in a specified quantity of solvent.
Answer: Standard heat of formation for a compound
Answer: Standard heat of formation
Answer: Remains constant
Answer: Molar heat of fusion
Answer: Heat of combustion
Answer: Pressure
Answer: Specific heat
Answer: Endothermic process
Answer: Amount of heat absorbed or released when a solid dissolves
Answer: Mix the reactants in a calorimeter and measure the temp change.
Answer: Its mass
Answer: Less than the specific heat of water
Answer: Greater than the energy stored in the bonds of the products
Answer: They are two different measures of amounts of energy.
Answer: Materials in the surroundings of the system
Answer: Evaporation
Answer: Heat flows from the warmer object to the cooler object until they reach the same temperature.
Answer: 1 x 10^-14
Answer: Neutral
Answer: The equivalence point has been reached
Answer: Ammonia
Answer: Weakly acid
Answer: Nitric acid
Answer: [HF] is greater than [H^+] [F^-]
Answer: Weak acid
Answer: Carbonic acid and sodium carbonate
Answer: Ionization constant
Answer: Degree of ionization
Answer: Equilibrium constant times the concentration of water
Answer: Complete ionization in water
Answer: Equal to [OH-]
Answer: OH^- and H3O^+
Answer: NH4^+ and NH3
Answer: H2O and HCN
Answer: 2
Answer: Brønsted lowry base
Answer: By dissociating into ions that have a different color than the molecular form
Answer: Accept a pair of electrons
Answer: Magnesium hydroxide
Answer: H^+
Answer: An elementary reaction converts reactants to products in a single step.
Answer: Intermediates
Answer: Third
Answer: Rate= k[A][B]^2
Answer: It is negative
Answer: Enthalpy and entropy change
Answer: It's endothermic
Answer: They all release free energy
Answer: Entropy and energy
Answer: The product of the concentrations of two ions exceeded the Ksp for the compound formed by the ions.
Answer: Entropy
Answer: 1.0 x 10^-18 M
Answer: Disorder
Answer: Free energy
Answer: Reactants are favored
Answer: Reversible; favoring products
Answer: The reaction makes more reactants
Answer: The reaction shifts toward the product gas
Answer: Some product; some reactant
Answer: 2.0 x 10^-10 M
Answer: Ksp=2[Ag^+][S^2-]
Answer: Lowering the activation energy barrier
Answer: A catalyst decreases the activation energy of reaction
Answer: When an activated complex exists
Answer: Transition state
Answer: 2 half rxns must be physically separated
Answer: Zn(s)
Answer: Volta
Answer: Cu2+
Answer: Mercury
Answer: Potassium
Answer: Mercury
Answer: Highly active metal
Answer: Platinum
Answer: Make electron changes of both half reactions equal
Answer: Write equation showing ions separately
Answer: Choose coefficients to make the change in oxidation number equal 0.
Answer: Assign oxidation numbers to all atoms
maximize migration differences
minimize spreading
A measure of the amount of mobile phase required to remove each component of the mixture from the column
Vr↑ = attracted to stationary phase
Vr↓ = attracted to mobile phase
mobile phase is solvent
stationary phase is the water
substances that follow "like dissolves like" with water will have a higher Rf value
Answer: Distance moved by the component / Distance moved by the mobile phase front
1)convert volume of CO2 to grams
2)Plug both numbers into absorption capacity equation
3)calculate
1)Rearrange PV=nRT to find the number of moles of CO2
2)Calculate n
3)Use stoichiometry to convert n to grams using molar mass conversion
Answer: A back titration is faster. Excess HCl is added to dissolve CaCO₃, then unreacted acid is titrated with a standard solution of base.
HCl(aq) + NaOH(aq) → NaCl (aq) + H₂O (l)
H⁺(aq) + OH⁻(aq)→H₂O(l)
Endpoint: yellow color → dark blue
Answer:
Serial: add 1 drop to well 1, 2 drops to well 2, ... (progression of titration)
Single: add 1 drop, observe, add another drop, observe. (higher precision)
Answer: BTB will keep longer and the color change is instantaneous. RCE needs to be kept cool to prevent degradation.
1. Acid/Base: acids react with bases to produce salt and H2O.
2. Precipitation: forms an insoluble product.
3. Redox: chemical species changing oxidation states.
4. Complexation: form a complex ion (metal ion with other substances covalently bonded to it.
Answer: The dissolved ammonia gas in the water comes out of solution very quickly and becomes NH₃(g) again.
1. Na₂CO₃(aq) + 2 H₂O(l)→2 NaOH(aq) + CO₂(aq) + H₂O(l)
2. AlCl₃(aq) + 3 H₂O(l)→Al(OH)₃(aq) + 3 HCl(aq)
3. KI(aq) + H₂O(l)→KOH(aq) + HI(aq)
Answer: A small puddle of each substance was placed on the reaction surface. Next, a sample of KI was placed in each puddle. KI is ionic and polar so it would dissolve in polar solvents. The polarity of the solvents would be ranked bases on how quickly the KI dissolved.
Answer: Polar substances are able to dissolve other polar substances. Water can dissolve salt because salt is an ion and ions break up completely in solution.
Answer: 2 Al(s) + 2 NaOH + 6H₂O → 3 H₂(g) + 2 NaAl(OH)₄
Answer: It confirms the identity of the compound and measures its purity. Impurities decrease the melting point and gives a bigger range of melting point.
Answer: Sulfate was tested for by reacting the alum with BaCl2. A white precipitate of BaSO4 formed. K and H2O were tested for by the flame test. The flame turned purple which shows K in it and a popping noise was heard as the water evaporated. Al was tested for by reacting it with KOH and checking for the Al(OH)4 precipitate and by Al having an acidic pH.
Answer: % yield = (g alum actually obtained / g alum theoretically produced) * 100 %
CO₂ + H₂O → H₂CO₃.
H₂CO₃ is carbonic acid.
Answer: 3 H₂SO₄ + 2 Al → Al₂(SO₄)₃ + 3 H₂.
H₂ is hydrogen gas (bubbles).
Answer: Iron corrodes relatively quickly while Al reacts with air to form a thin layer of aluminum hydroxide which slows corrosion. Iron will rust and corrode continuously.
Answer: Expensive: The bauxite deposits occur outside of the US and the Hall-Heroult process is extremely energy intensive.
Uses: writing paper, soap
When tap water was reacted, the solution turned yellow due to the high chlorine ion concentration. The Brita water turned a lighter shade of yellow due to the Cl⁻ ions being removed. The Cl⁻ was removed because it stuck to the activated carbons which have tiny pores so there is a high surface area to react.
(a) Be able to estimate the standard deviation for a set of data using the "2/3's rule" described in this experiment. (b) Also, know how to calculate a standard deviation by hand for a given set of data.
(a) 1. put the number in increasing order.
2. Find the average of the numbers.
3. 2/3 * # of data points
4. + or - two points on either side of the average.
5. Report answer
(b) [(∑(x-x1)^2)/(N-1)]^.5
Answer: C1V1=C2V2
Answer: The extra energy is removed continuously by the solvent molecules by bumping into the excited food dye molecules.
Answer: The process where a set of solutions of known concentrations of some light absorbing substance is placed in a series of containers. Unknown concentration solution can be determined by comparing with the calibration set.
Answer: The energy of a particular photon of visible light matches the energy needed to promote an electron from a low energy state to a higher one.
Answer: The observed color is the color transmitted, where the absorbed color is it's complementary color, which is not seen.
(a) ∙frequency= speed of light/wavelength
∙energy= frequency x Planck's constant.
(b) ΔE= -Rn x (1/nf^2 - 1/ni^2)
(c) % difference = [(actual - theoretical)/ actual] x 100%
1. Spectroscope constructed.
2. Sample of excited hydrogen gas was viewed through spect.
3. It was noted what line on the graph paper in the spec. each line of H's spectra was on.
4. Plot the # of graph paper lines vs. actual wavelength and an equation was determined.
(a) slit width wider = wider colors, size of spectrum stays the same.
(b) closer to the spectroscope = more intense light
White light is apparent 'colorless' light from 400-750 nm. (Ex. light from the sun).
Lowest to highest: ROYGBV
Answer: Electronic energy transitions. (valence electrons)
Continuous: contains all the frequencies of the emitted radiation within a region on the EM spectrum. (Ex. the sun)
Line spectrum: only includes certain frequencies emitted by atoms in the gas phase and is produced by excited atoms. (Ex. gases)
(150 lb)∙(.453C/mi-lb)=67.95 C/mi
(67.95C/mi)∙(1g/ 5.7 C) = 12g = 12 peanuts
A small calorie "c" is a scientific calorie and it is 1000x smaller than a food calorie. Food calorie is 1000c and is how food is measured.
Answer: E=energy, m=mass, c=specific heat, ΔT=change in temperature
Answer: 908 kJ/mol
Answer: 657 kJ/mol
Answer: 347 kJ/mol
Answer: triple bonds
Answer: single bonds
Answer: C, O, N
A) Li, Na, K
B) N, O, I
C) C, S, Pb
D) K, Fe, Br
Answer: B) N, O, I
A) iron sulfide
B) iron (I) sulfide
C) iron (I) sulfate
D) iron (II) sulfide
E) iron (II) sulfate
Answer: D) iron (II) sulfide
A) 8.59 mL
B) 7.40 mL
C) 11.6 mL
D) 12.4 mL
E) 13.5 mL
Answer: C) 11.6 mL
A) C4H5N2O
B) C8H10N4O2
C) C8H10N2O
D) C8H12N4O2
Answer: B) C8H10N4O2
A) CHO
B) C5H2O
C) C6HO3
D) C3H7O
E) C3H6O
Answer: E) C3H6O
A) 2 CH3 (g) + 5 O (g) → 2 CO (g) + 3 H2O (g)
B) C2H6 (g) + 7 O (g) → 2 CO2 (g) + 3 H2O (g)
C) 2 C2H6 (g) + 5 O2 (g) → 4 CO (g) + 6 H2O (g)
D) C2H6 (g) + 5 O (g) → 2 CO (g) + 3 H2O (g)
E) 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g)
Answer: (C) 2 C2H6 (g) + 5 O2 (g) → 4 CO (g) + 6 H2O (g)
A) Law of the Conservation of Mass
B) First Law of Thermodynamics
C) Law of Multiple Proportions
D) Law of Modern Atomic Theory
E) Law of Definite Proportions
Answer: C) Law of Multiple Proportions
A) 18
B) 12
C) 16
D) 15
E) 19
Answer: A) 18
A) 2+
B) 1-
C) 4+
D) 1+
E) 2-
Answer: B) 1-
A) Ca
B) Zn
C) Co
D) P
E) Cs
Answer: D) P
A) K
B) N
C) Ar
D) Br
E) O
Answer: C) Ar
A) Cu
B) Ti
C) Br
D) Cs
E) Mg
Answer: E) Mg
A) 40.08
B) 112.41
C) 20
D) 48
Answer: B) 112.41
A) 70.932 amu
B) 70.928 amu
C) 70.920 amu
D) 70.924 amu
Answer: D) 70.924 amu
A) 10.0 g Mg
B) 10.0 g Ne
C) 10.0 g Kr
D) 10.0 g Ar
E) 10.0 g He
Answer: E) 10.0 g He
A) 4.27 × 1022 Li atoms
B) 5.90 × 1025 Li atoms
C) 7.09 × 1021 Li atoms
D) 8.49 × 1024 Li atoms
E) 4.18 × 1024 Li atoms
Answer: D) 8.49 × 1024 Li atoms
A) 2.4 × 102 g
B) 6.5 × 102 g
C) 3.9 × 102 g
D) 1.5 × 102 g
E) 3.2 × 102 g
Answer: B) 6.5 × 102 g
A) 9.44 L
B) 0.106 L
C) 31.2 L
D) 0.0320 L
Answer: A) 9.44 L
A) carbon dioxide
B) rust
C) water
D) sodium chloride
E) helium
Answer: E) helium
A) cola
B) salsa
C) mud
D) salad dressing
E) ice water
Answer: A) cola
A) coffee brewing
B) water boiling
C) salt dissolves in water
D) leaves turning color in the fall
E) None of the above are chemical changes.
Answer: D) leaves turning color in the fall
A) Aluminum has a tendency to "rust."
B) Mercury is a silvery liquid at room temperature.
C) Butane is highly flammable.
D) Sodium metal is extremely reactive with chlorine gas.
E) Argon has an unreactive nature.
Answer: B) Mercury is a silvery liquid at room temperature.
A) Her results are precise, but not accurate.
Her results are accurate, but not precise.
B) Her results are neither precise nor accurate.
C) Her results are both precise and accurate
D) It isn't possible to determine with the information given.
Answer: B) Her results are precise, but not accurate.
Answer: 0.760 nm
A) polyethylene.
B) nylon.
C) Teflon.
D) polystyrene.
Answer: B) nylon.
A) The PVC monomer has a chlorine atom, but the PE monomer does not.
B) The PVC monomer has two chlorine atoms, but the PE monomer does not.
C) The PE monomer has one chlorine atom, and the PVC monomer has two chlorine atoms.
D) The PVC monomer has a triple bond, and the PE monomer has a double bond.
Answer: A) The PVC monomer has a chlorine atom, but the PE monomer does not.
A) film
B) nonstick cookware
C) bullet-proof vests
D) garbage bags
Answer: B) nonstick cookware
A) Teflon.
B) polyethylene.
C) PVC.
D) Bakelite.
Answer: C) PVC.
A) polyvinyl chloride.
B) polystyrene.
C) polyethylene.
D) bakelite plastic.
Answer: B) polystyrene.
A) polyacetylene.
B) polyethylene.
C) polyvinyl chloride.
D) polystyrene.
Answer: A) polyacetylene.
A) H2CCH2.
B) Cl2CCH2.
C) H2CCHCl.
D) F2CCF2.
Answer: C) H2CCHCl.
A) H2CCH2.
B) Cl2CCH2.
C) H2CCHCl.
D) F2CCF2.
Answer: D) F2CCF2.
A) is of lighter weight.
B) is easier to handle and cut.
C) is more resistant to corrosion.
D) All of the above are advantages of PVC.
Answer: D) All of the above are advantages of PVC.
A) one atom.
B) two atoms.
C) three atoms.
D) four atoms.
Answer: A) one atom.
A) CH2CH2.
B) CH2CHCH3.
C) CH3CH3.
D) CH3CH2CH3.
Answer: B) CH2CHCH3.
A) HDPE has a higher density than LDPE does.
B) HDPE holds its shape better than LDPE does when they are put into boiling water.
C) HDPE is more flexible than LDPE is.
D) HDPE has fewer side chains branching off from the main chains than LDPE does.
Answer: C) HDPE is more flexible than LDPE is.
A) The polymer has the same properties as the monomer.
B) The polymer has alternating double and single bonds between carbons, while the monomer has only single bonds between carbons.
C) The polymer has alternating double and single bonds between carbons, while the monomer has only double bonds between carbons.
D) The polymer has only single bonds between carbons, while the monomer has only double bonds between carbons.
Answer: D) The polymer has only single bonds between carbons, while the monomer has only double bonds between carbons.
A) polyethylene.
B) polypropylene.
C) polystyrene.
D) polyvinyl chloride.
Answer: A) polyethylene.
A) two or more different monomers.
B) different polymers linked end to end.
C) different polymers cross-linked.
D) none of the above
Answer: A) two or more different monomers.
A) polyethylene.
B) polyvinyl chloride.
C) polystyrene.
D) polytetrafluoroethylene (Teflon).
Answer: A) polyethylene.
A) high-density polyethylene.
B) hot-dipped polyethylene.
C) high-dose polyethylene.
D) highly-diffuse polyethylene.
Answer: A) high-density polyethylene.
A) linearly dense polyethylene.
B) light diffuse polyethylene.
C) low-density polyethylene.
D) lightly doped polyethylene.
Answer: C) low-density polyethylene.
A) food wrap.
B) rigid containers.
C) drain pipes.
D) television cabinets.
Answer: A) food wrap.
A) food wrap.
B) rigid containers.
C) squeeze bottles.
D) garbage bags.
Answer: B) rigid containers.
A) primarily linear, unbranched chains of polyethylene in a close packing arrangement.
B) primarily highly branched, non-linear chains of polyethylene in a diffuse packing arrangement.
C) a mixture of polyethylene and polystyrene.
D) polyethylene with low density plasticizers added to increase density.
Answer: B) primarily highly branched, non-linear chains of polyethylene in a diffuse packing arrangement.
A) primarily linear, unbranched chains of polyethylene in a close packing arrangement.
B) primarily highly branched, non-linear chains of polyethylene in a diffuse packing arrangement.
C) a mixture of polyethylene and polystyrene.
D) polyethylene with high density plasticizers added to increase density.
Answer: A) primarily linear, unbranched chains of polyethylene in a close packing arrangement.
A) polymethane
B) polyethylene
C) polyvinyl chloride
D) polystyrene
Answer: B) polyethylene
A) cellulose
B) polyesters
C) nucleic acids
D) proteins
Answer: D) proteins
A) composites
B) nylon
C) starch
D) None of the above is a naturally occurring polymer.
Answer: C) starch
A) proteins.
B) carboxylic acids.
C) esters.
D) nucleic acids.
Answer: D) nucleic acids.
A) mer
B) mono
C) poly
D) tetra
Answer: C) poly
A) They have the same chemical and physical properties.
B) They have different chemical and physical properties.
C) The monomer is usually a solid, while the polymer is usually a liquid or gas.
D) They have the same chemical formula.
Answer: B) They have different chemical and physical properties.
A) one bond.
B) one unit.
C) many bonds.
D) many rings.
Answer: B) one unit.
A) parts.
B) sides.
C) rings.
D) carbons.
Answer: A) parts.
A) small building blocks of polymers.
B) small polymers.
C) ethylene.
D) all of the above
Answer: A) small building blocks of polymers.
A) ammonia
B) bleach
C) lye
D) vinegar
Answer: D) vinegar
A) acidosis
B) alkalosis
C) hyperacidity
D) anemia
Answer: B) alkalosis
A) AlOH.
B) Al(OH)2.
C) Al(OH)3.
D) Al3OH.
Answer: C) Al(OH)3.
A) acids.
B) bases.
C) neutral.
D) salts.
Answer: B) bases.
A) baking soda.
B) baking powder.
C) washing soda.
D) cherry soda.
Answer: A) baking soda.
A) 9.5
B) 9.0
C) 7
D) 1.5
Answer: D) 1.5
A) below 4.
B) below 5.6.
C) below 7.
D) above 8.5
Answer: B) below 5.6.
A) ammonia, NH3
B) sulfur dioxide, SO2
C) nitrogen dioxide, NO2
D) nitric oxide, NO
Answer: A) ammonia, NH3
A) coal-burning power plants
B) lightning
C) volcanic eruptions
D) All of the above contribute to acid rain.
Answer: D) All of the above contribute to acid rain.
A) less than 7.
B) equal to 7.
C) greater than 7.
D) 0.
Answer: A) less than 7.
A) resists changes in pH when small amounts of a strong acid or a strong base are added.
B) is made up of a weak acid and its conjugate base.
C) is made up of a weak base and its conjugate acid.
D) All of the above are true.
Answer: D) All of the above are true.
A) acid-base indicator.
B) buffer.
C) antacid.
D) acid rain.
Answer: B) buffer.
A) H atom.
B) O atom.
C) pH unit.
D) proton.
Answer: D) proton.
A) H2SO4
B) H2SO3
C) HSO4-
D) SO32-
Answer: D) SO32-
A) H2SO4
B) H2SO3
C) HSO4-
D) SO32-
Answer: B) H2SO3
A) H2SO4 and SO42-
B) H3O+ and OH-
C) H2SO4 and HSO4-
D) CH4 and CH3OH
Answer: C) H2SO4 and HSO4-
A) blood
B) lemon juice
C) unpolluted rainwater
D) NaOH (4% solution)
Answer: B) lemon juice
A) acid.
B) base.
C) salt.
D) solvent.
Answer: B) base.
A) acid.
B) base.
C) salt.
D) solvent.
Answer: A) acid.
A) strongly acidic.
B) weakly acidic.
C) strongly basic.
D) weakly basic.
Answer: C) strongly basic.
A) weakly basic.
B) strongly basic.
C) weakly acidic.
D) strongly acidic.
Answer: A) weakly basic.
A) 10-10 mol/L.
B) 1010 mol/L.
C) 10 mol/L.
D) -10 mol/L.
Answer: A) 10-10 mol/L.
A) H3O+
B) SO42-
C) OH-
D) HSO4-
Answer: A) H3O+
A) colorless
B) green
C) pink
D) yellow
Answer: C) pink
A) colorless
B) green
C) pink
D) yellow
Answer: A) colorless
A) Ba(OH)2 + H2SO4 → BaSO4 + 2 H2O
B) BaOH + H2SO4 → BaSO4 + 2 H2O
C) BaOH2 + H2SO4 → BaSO4 + H2O
D) Ba(OH)2 + 2 H2SO4 → Ba(SO4)2 + 2 H2O
Answer: A) Ba(OH)2 + H2SO4 → BaSO4 + 2 H2O
A) Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O
B) BaOH2 + 2 HCl → BaCl2 + H2O
C) Ba(OH)2 + HCl → BaCl2 + H2O
D) BaOH + HCl → BaCl + H2O
Answer: A) Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O
A) 4.
B) 5
C) 1.
D) 2.
Answer: D) 2.
A) 2.
B) 1.
C) 3.
D) 4.
Answer: A) 2.
A) 3.
B) 1.
C) 2.
D) 44.
Answer: B) 1.
A) is present in low concentration in solution.
B) is present in high concentration in solution.
C) ionizes only slightly in solution.
D) ionizes completely in solution.
Answer: C) ionizes only slightly in solution.
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.
Answer: B) a relatively small fraction of the maximum number of possible hydronium ions.
A) is very concentrated.
B) makes acid-base indicators change color.
C) ionizes completely in water.
D) causes metals to corrode.
Answer: C) ionizes completely in water.
A) dilute acid.
B) concentrated acid.
C) weak acid.
D) strong acid.
Answer: C) weak acid.
A) hydrochloric acid.
B) sulfuric acid.
C) nitric acid.
D) acetic acid.
Answer: D) acetic acid.
A) sour.
B) bitter.
C) salty.
D) sweet.
Answer: C) salty.
A) no hydroxide ions.
B) a relatively small fraction of the maximum number of possible hydroxide ions.
C) a relatively large fraction of the maximum number of possible hydroxide ions.
D) 100% of the maximum number of possible hydroxide ions.
Answer: D) 100% of the maximum number of possible hydroxide ions.
A) no hydroxide ions.
B) a relatively small fraction of the maximum number of possible hydroxide ions.
C) a relatively large fraction of the maximum number of possible hydroxide ions.
D) 100% of the maximum number of possible hydroxide ions.
Answer: B) a relatively small fraction of the maximum number of possible hydroxide ions.
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.
Answer: D) 100% of the maximum number of possible hydronium ions.
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.
Answer: B) a relatively small fraction of the maximum number of possible hydronium ions.
A) a weaker acid than acetic acid.
B) a stronger acid than acetic acid.
C) equal in acid strength to acetic acid.
D) a base.
Answer: B) a stronger acid than acetic acid.
A) salty
B) acidic
C) neutral
D) basic
Answer: D) basic
A) salty
B) acidic
C) neutral
D) basic
Answer: B) acidic
A) Na
B) MgO
C) NH3
D) SO3
Answer: D) SO3
A) CO2
B) NaOH
C) K2O
D) H2SO4
Answer: A) CO2
A) CaO
B) CaOH
C) Ca2OH
D) Ca(OH)2
Answer: D) Ca(OH)2
A) KOH
B) K2OH
C) KH
D) KH2
Answer: A) KOH
A) Na2O
B) CO2
C) Cl2
D) SO3
Answer: A) Na2O
A) buffer.
B) catalyst.
C) elecrolyte.
D) indicator.
Answer: C) elecrolyte.
A) CaOH
B) Ca2OH
C) Ca(OH)2
D) CaOH2
Answer: C) Ca(OH)2
A) Bases produce hydronium ions.
B) Bases are proton donors.
C) Bases produce hydroxide ions.
D) Bases are proton acceptors.
Answer: D) Bases are proton acceptors.
A) OH-
B) H+
C) H3O+
D) H2O-
Answer: A) OH-
A) transfer of protons.
B) transfer of electrons.
C) conversion of protons into electrons.
D) ionization of atoms.
Answer: A) transfer of protons.
A) KOH.
B) HNO3.
C) NH3.
D) Mg(OH)2.
Answer: B) HNO3.
A) H3PO4.
B) H4PO3.
C) H2PO4.
D) HPO4.
Answer: A) H3PO4.
A) SO4
B) HSO4
C) H2(SO)4
D) H2SO4
Answer: D) H2SO4
A) acid.
B) base.
C) salt.
D) solvent.
Answer: A) acid.
A) Acids produce hydronium ions.
B) Acids are proton donors.
C) Acids produce hydroxide ions.
D) Acids are proton acceptors.
Answer: B) Acids are proton donors.
A) hydronium ion.
B) proton.
C) electron.
D) hydrate.
Answer: B) proton.
A) hydrate ion.
B) hydrogen ion.
C) hydroxide ion.
D) hydronium ion.
Answer: D) hydronium ion.
A) Acids are defined as compounds that produce H+ ions in water solution.
B) Bases are defined as compounds that produce OH- ions in water solution.
C) Arrhenius theory only applies to reactions in aqueous solution.
D) Acids are defined as compounds that produce OH- ions in water solution.
Answer: D) Acids are defined as compounds that produce OH- ions in water solution.
A) amphiprotic.
B) an acid-base indicator.
C) a buffer.
D) protonated.
Answer: B) an acid-base indicator.
A) taste bitter
B) reacts with acids to form salts
C) produce hydroxide ions when added to water
D) All are characteristics of bases.
Answer: D) All are characteristics of bases.
A) taste sour
B) turn litmus red
C) react with bases to form salts
D) All are characteristics of acids.
Answer: D) All are characteristics of acids.
A) bitter
B) sweet
C) salty
D) sour
Answer: D) sour
A) acids.
B) bases.
C) salts.
D) neutral.
Answer: B) bases.
A) basic.
B) acidic.
C) neutral.
D) caustic.
Answer: B) acidic.
A) taste bitter
B) turn litmus red
C) react with acids to form salts
D) produce hydroxide ions when added to water
Answer: B) turn litmus red
A) taste bitter
B) turn litmus red
C) react with bases to form salts
D) react with active metals to form H2 gas
Answer: A) taste bitter