CHEM132- Final Exam Review

Covalent Bond

Atoms shared are between atoms

A student carried out a mole ratio experiment where she varied the volume of a 0.1 M NaOH and 0.1M unknown acid. The greatest temperature change was recorded using 20 ml of 0.1 M unknown acid and 40 mL of 0.1 M NaOH. What is the identity of the unknown acid? A.)H3PO4 B.)H2SO4 C.)HCl

B

Which of the following acids is monoprotic? A.)H2CO3 B.)HCl C.)H2SO4 D.)H2PO4

B

CaCO3 dissolves upon the addition of HCl. The CaCO3 can now be separated from SiO2 by _______ as the CaCO3 is now found in the ________. The CaCO3 is reconstituted by _______.

Decantation, supernatant, and addition of potassium carbonate

As the volume of the heated solution ______, the risk of splattering _______.

Decreases and Increases

Potassium

Edges darken when cut; in water, immediately bursts into a lavender flame

If a double displacement reaction takes place between solutions of lead (II) chloride and copper (II) sulfate, the two possible products are _________ and ________.

lead (II) sulfate and copper (II) chloride

A more reactive metal ____ electrons _____ readily than a less reactive metal. Therefore, a reaction _______ be observed when a less active metal placed into a ______ solution of a more reactive metal.

loses, more, will not, and cation

Solubility

max mass of a substance dissolving in a volume of another

The bonding of naphthalene is _______ ; the bonding in water is ________. Naphthalene _______ be soluble in water.

non-polar covalent, polar covalent, and will not.

If a double displacement reaction takes place between solutions of sodium sulfite and cobalt (II) sulfate, the two possible products are _________ and ________.

sodium sulfate and cobalt (II) sulfite

solute

substance that which is dissolved

solvent

substance which does the dissolving

Erichrome Black EBT

the indicator us used

EDTA

the titrant in the experiment; it complexes with free Zn2+

solution

uniform mixture of two or more substances

When colorless solutions of calcium iodide and zinc sulfate are mixed, an insoluble precipitate ______ form. The color of the solution will be _______; that of the solid be _______.

will not, colorless and NR

When solutions of pink cobalt chloride and colorless sodium hydroxide are mixed a precipitate _______ form. The color of the solution will be _______; the solid will be _______.

will, colorless and rose-red

When solutions of colorless lead nitrate and colorless magnesium iodide are mixed, an insoluble precipitate _______ form. The color of the solution will be ______; that of the solid will be _______.

will, colorless, and yellow

Consider the following components which might appear in a mixture to be separated: CaCO3, CaSO4, Ca(NO3)2. Which one can be separated from the others using HCl?

CaCO3

Potassium is a Group IA metal; it has _______ valence electrons; its cation has the electron configuration of a _______.

1 and noble gas.

Based on the atomic composition of the following molecules, which is likely to be flammable? A.)1-hexanol B.)sucrose C.)Potassium Nitrate D.)Ammonium sulfate

1-hexanol

The chemical formula of sodium phosphate is Na3PO4 because the cation has a charge of _________ and the anion has a charge of ______.

+1 and -3

The chemical formula of magnesium nitrate is Mg(NO3)2 because the cation has a charge of ________ and the anion has a charge of ________.

+2 and -1

25.0 mL of 1.00 M HCl at 23.5oC react with 25.0 mL 1.00 M NaOH in a styrofoam calorimeter whose calorimeter constant is 48.8 J/C. The final temperature is 30.0oC. Assume the density of the solution product is 1.00 g/mL and the specific heat of the solution is 4.18 J/goC. The heat of this neutralization reaction is [x].

-1700 J

25.0 mL of 1.00 M HCl at 24.3oC react with 25.0 mL 1.00 M NaOH in a styrofoam calorimeter whose calorimeter constant is 70 J/oC. The final temperature is 31.8oC. Assume the density of the solution product is 1.00 g/mL and the specific heat of the solution is 4.18 J/goC. The heat of this neutralization reaction is [x].

-2100 J

3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 19.21°C. Calculate ∆H for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g･°C and the density of the solution is 1.20 g/mL).

-4.59 kJ??

A zinc chloride solution is prepared by dissolving 0.316 g in 100.0 mL. 19.97 mL of the above solution is transferred into a beaker and titrated with a 0.0225 M EDTA solution.The endpoint is reached after 19.72 mL of the EDTA solution is added. EDTA is known to complex in a 1:1 mole ratio with multivalent cations. What is the mass of zinc titrated? The molar mass of ZnCl2 is 136.315 g/mol The molar mass of Zn is 65.38 g/mol The molar mass of Cl is 35.45 g/mol

0.0290 g

A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of H2O. Upon titrating a 19.97 mL aliquot of the above solution with 19.72 mL of a 0.0225 M EDTA solution it is determined that the aliquot contains 0.0290 g Zn2+. What mass of Cl- is contained in the same aliquot? The molar mass of ZnCl2 is 136.315 g/mol The molar mass of Zn is 65.38 g/mol The molar mass of Cl is 35.45 g/mol

0.0341 g

A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of H2O. What mass of zinc chloride is present in 19.97 mL of that solution.

0.0631 g

Magnesium is a Group IIA metal; it has ______ valence electrons; it's cation has the electron of a _________.

2 and noble gas

Strontium is a Group IIA metal; it has ________ valence electrons; its cation has the electron configuration of _________.

2 and noble gas

There will be two waste containers in the hood for the Solubility and Polarity portion of this experiment...one labeled "aqueous" waste and the other "organic waste". Which of the following mixtures should be put into the "aqueous" waste container? A.)sucrose in water B.)ethanol in hexane C.)naphthalene in water D.)calcium chloride in hexane

A

Which of the following does not describe one of the ways the color of ionic solutions is explored in this experiment? A.)Whether colored ions are more likely to be constituents of insoluble ionic salts B.)Whether the cation or anion of an ionic salt is responsible for the salt's color C.)the relationship between the color of an ionic salt solution and the energy of the light absorbed by the solution D.)Whether the color of a dry salt is related to the color of the solution it forms

A

Which of the following is not consistent with the role water plays in dissociating ionic compounds? A.)The oxygen atom of water pulls electron strength from the hydrogen atoms toward itself, leaving it with a partial positive charge and the hydrogen atoms with partial negative charges. B.)Water is a polar covalent solvent; electrons forming the bond between its hydrogen and oxygen atoms are not shared equally. C.)When an ionic salt dissolves, the polar ends of water are attracted to oppositely charged ions in solution, surrounding them and preventing them from recombining. D.)Possible Answer While a polar covalent solvent like water does not carry an electrical charge, a dipole exists between each hydrogen atom and the single oxygen atom

A

A known volume of a solution prepared by dissolving a known mass of zinc chloride to a final volume of 100.0 mL will be titrated. The volume of the titrant, EDTA, needed to complex free Zn2+ in the sample is used to calculate the #moles of Zn in the sample, and indirectly, the moles Cl present. Which of the following mathematical operations gives you the mass of chlorine in the sample titrated? A.)mass = mass zinc chloride x volume of sample titrated 100.0 mL B.)mass = #moles EDTA used to titrate sample X (1 mole Zn / 1 mole EDTA) X molar mass of zinc C.)mass = mass of sample titrated - mass of Zn complexed D.)volume EDTA x [EDTA] (moles / L) x (1 mole Zn / 1 mole EDTA)

C

A known volume of a solution prepared by dissolving a known mass of zinc chloride to a final volume of 100.0 mL will be titrated. The volume of the titrant, EDTA, needed to complex free Zn2+ in the sample is used to calculate the #moles of Zn in the sample, and indirectly, the moles Cl present. Which of the following mathematical operations gives you the mass of zinc chloride being titrated? A.)mass = #moles EDTA used to titrate sample X (1 mole Zn / 1 mole EDTA) X molar mass of zinc B.)mass = mass of sample titrated - mass of zinc complexed C.)mass = mass zinc chloride x volume of sample titrated 100.0 mL D.)volume EDTA x [EDTA] (moles / L) x (1 mole Zn / 1 mole EDTA

C

A known volume of a solution prepared by dissolving a known mass of zinc chloride to a final volume of 100.0 mL will be titrated. The volume of the titrant, EDTA, needed to complex free Zn2+ in the sample is used to calculate the #moles of Zn in the sample, and indirectly, the moles Cl present. Which of the following mathematical operations gives you the number of moles of zinc which were titrated? A.)mass = #moles EDTA used to titrate sample X (1 mole Zn / 1 mole EDTA) X molar mass of zinc B.)mass = mass of sample titrated - mass of zinc complexed C.)volume EDTA x [EDTA] (moles / L) x ( 1 mole Zn / 1 mole EDTA) D.)mass = mass zinc chloride x volume of sample titrated 100.0 mL

C

A student carried out a mole ratio experiment where she varied the volume of a 0.1 M NaOH and 0.1M H3P04. In one of the test tubes, the student mixed 20 ml of 0.1M H3P04 and 40 ml of 0.1 M NaOH to produce Na3PO4 and H20. In this test tube which reactant is the limiting reactant. A.)H20 B.)Na3PO4 C.)NaOH D.)H3PO4

C

A student carried out a mole ratio experiment where she varied the volume of a 0.1 M NaOH and 0.2M unknown acid. The greatest temperature change was recorded using 20 ml of 0.2M unknown acid and 40 ml of 0.1 M NaOH. What is the identity of the unknown acid? A.)H2SO4 B.)H3PO4 C.)HCl

C

Because water is a [x] molecule, it can act to disrupt the bonds of ionic salts, resulting in free ions in solution which can then undergo a double displacement reaction. A.)precipitate B.)solvate C.)polar covalent D.)dissociate E.)net ionic equation

C

Consider the following information: The weak acid, carbonic acid (H2CO3) spontaneously decomposes to give CO2 and H2O in solution. If acidic lemon juice were added to baking soda (NaHCO3) what evidence of chemical reaction might be observed. A.)formation of a precipitate B.)color change C.)bubbles form or a smell is detected D.)temperature change

C

Which of the following acids is triprotic? A.)H2SO4 B.)CH3COOH C.)H3PO4 D.)HCl

C

A known volume of a solution prepared by dissolving a known mass of zinc chloride to a final volume of 100.0 mL will be titrated. The volume of the titrant, EDTA, needed to complex free Zn2+ in the sample is used to calculate the #moles of Zn in the sample, and indirectly, the moles Cl present. Which of the following mathematical operations gives you the mass of zinc titrated? A.)mass = mass zinc chloride x volume of sample titrated 100.0 mL B.)mass = mass of sample titrated - mass of Zn complexed C.)volume EDTA x [EDTA] (moles / L) x (1 mole Zn / 1 mole EDTA) D.)mass = #moles EDTA used to titrate sample X (1 mole Zn / 1 mole EDTA) X molar mass of zinc

D

Consider the following information: In general, spontaneous chemical reactions produce products that are more energetically stable than the reactants which form them. A strong acid reacts with a strong base to produce water and the free ions of a salt. Which of the following evidence of a chemical reaction might be observed when a strong acid is mixed with a strong base? A.)formation of a precipitate B.)color changes C.)bubbles form or a smell is detected D.)temperature change

D

Sodium

Dances on the water and then bursts into a yellow flame

Enthalpy of reaction (Δ H), or heat flow, is defined as the amount of heat that would have to enter, or leave, a system in order to bring the temperature back to its initial value. Therefore (Δ H) is positive for an endothermic reaction because the heat would have to [x] the system to bring the temperature back to the original value.

Enter

In this experiment, molarity is varied for the two reactants and the volume is kept constant. True or False

False

In this experiment, the NaOH was added to the unknown acid as seen in the video True or False

False

In this experiment, the initial temperature of the NaOH was much greater than the unknown acid before mixing. True or False

False

Is the amount of heat that must exit a system to return to starting temperature in an endothermic reaction? True or False

False

In filtration, the liquid which passes through filter paper is called ______; the material remaining in the paper is ______.

Filtrate and Residue

Lithium

Less dense than water; dances rapidly across the surface of water

Beer's Law

Linear relations between the absorbance and the concentration of absorbing species

Two liquids which are partially soluble in each other are _______; with mixing, a ______ solution will form.

Partially miscible and uniform

Spectrum

Pattern of visible wavelength colors

Identify the change described in the following as either chemical or physical: A cake batter is made by folding milk and eggs into flour, sugar, salt and cocoa.

Physical

Identify the change described in the following as either chemical or physical: When cold water is placed in a pot and heated, bubbles rise through the water to the top and escape into the atmosphere long before it boils.

Physical

Because sugar contains six hydroxyl groups, its bonding is ______; the bonding water is _______. Therefore, the sugar ______ be soluble in water.

Polar covalent, polar covalent, and will

Upon the introduction of zinc powder a CuSO4 solution loses its blue color, becoming totally colorless, and reddish precipitate forms on the bottom of the beaker. -Metallic zinc act as a __________. -The copper ions present in solution undergo ________ as the ions are chemically changed to a solid red elemental metal. -During this process, the charge on copper ________ to _______.

Reducing agent; reduction; +2 and 0

electronegativity

Relative ability of atoms to attract bonding electrons

Blank

Sample containing everything other than the light absorbed material.

In the experiment, you will combine different volumes of NaOH and unknown acid and measure the temperature for each combination. The ratios of volumes that give the highest temperature change on the graph will be equal to________________________

Stoichiometric ratio

Absorbance

The quantity of light absorbed by a solution

% Transmission

The ratio of the initial intensity of light and which reaches the detector

The _____ of ______ electrons from a ______ atom to a _____ atom forms two charged ions.

Transfer, valence, metal, and non-metal.

Cobalt is a _______ metal; it has _____ valence electrons; its cations has the electron configuration of ____________.

Transition, 2, and partially filled d-shell

Enthalpy is dependent only on changes in a system between initial and final states? True or False

True

Is calculated as the heat of reaction as a function of the # moles of limiting reagent which reacted? True or False

True

In extraction, solid components are separated from each other by adding a specific solvent which _______ only one component, which is then found in the _______ following filtration.

dissolves and filtrate

red EBT

evidence of the presence of free ZN2+ in solution

blue EBT

evidence that all ZN2+ has been complexed by EDTA

polar covalent compound

atoms shared between atoms are shared unequally

The electrostatic ______ of a positively-charged _______ for a negatively-charged _______ forms an ______ bond.

attraction, cation, anion, and ionic

non-polar covalent compound

bonding electrons between the atoms are shared equally