Equal volumes of 0.2M solutions of lead(II) nitrate and potassium bromide are combined to form lead(II) bromide as a yellow precipitate. Which of the following is the correct net ionic equation for the reaction?

A Pb2+ (aq) + 2Br− (aq) → PbBr2(s)

B K+(aq) + NO3−(aq) → KNO3(aq)

C Pb2+aq) + 2NO3−(aq) + 2K+(aq) + 2Br−(aq) → 2K+(aq) + 2NO3−(aq) + PbBr2(s)

D Pb(NO3)2(aq) + 2KBr(aq) → PbBr2(s) + 2KNO3(aq)

The reaction between aqueous strontium chloride (SrCl2) and aqueous potassium sulfate(K2SO4) forms a precipitate of strontium sulfate (SrSO4) . Which of the following represents the net ionic equation for the reaction?

B Sr2+(aq) + SO42−(aq) → SrSO4(s)

A Cl−(aq) + K+(aq) → KCl(aq)

C Sr2+(aq) + 2Cl−(aq) + SO42−(aq) + 2K+(aq) → SrSO4(s) + 2Cl−(aq) + 2K+(aq)

D SrCl2(aq) + K2SO4(aq) → SrSO4(s) + 2KCl(aq)

Which of the following statements related to the experiment is correct?

The mass of the sample increased, so a chemical change occurred when bonds formed between the metal and another substance.

The mass of the sample decreased, so physical changes occurred as the metal first melted and then boiled out of the crucible.

There was nothing for the metal to react with, so only a physical change could have occurred.

The sample was only heated, so neither a physical nor a chemical change occurred.

A student mixes 20.0g of white KCl crystals with distilled water in a beaker. After the mixture was stirred, no crystals are visible and the solution is clear. After several days, all of the water evaporates and white crystals are found in the beaker. Which of following pieces of experimental evidence would best help the student to confirm that a new compound had not been made and that only a physical change occurred?

D After the water has evaporated, the white crystals in the beaker have a mass of 20.0g

A The solution does not change color after stirring.

B The KCl crystals are no longer visible after mixing with water.

C There is a temperature change in the solution during the dissolving process.

Which of the following identifies the best way to gather evidence to support the type of change that occurred when water and X were mixed?

Measuring the electrical conductivities of X and the mixture of water and X .

Measuring the melting point of the mixture of water and X

Adding another substance to the mixture of water and X to see whether a solid forms

Measuring and comparing the masses of the water, X, and the mixture of water and X

Which of the following describes the changes in forces of attraction that occur as H2 O changes phase from a liquid to a vapor?

B Hydrogen bonds between H2 O molecules are broken.

A H – O bonds break as H – H and O – O bonds form.

C Covalent bonds between H2 O molecules are broken.

D Ionic bonds between H+ ions and OH- ions are broken.

E Covalent bonds between H+ ions and H2 O molecules become more effective.

2F2(g) + 2NaOH(aq) → OF2(g) + 2NaF(aq) + H2 O(l) A 2 mol sample of F2(g) reacts with excess NaOH(aq) according to the equation above. If the reaction is repeated with excess NaOH(aq) but with 1 mol of F2(g), which of the following is correct?

The amount of OF2(g) produced is halved.

The amount of OF2(g) produced is doubled.

The amount of NF(aq) produced remains the same.

The amount of NF(aq) produced is doubled.

MgCl2(aq) + 2NaOH(aq) → 2NaCl(aq) + Mg(OH)2(s) A 100mL sample of 0.1M MgCl2(aq) and a 100mL sample of 0.2MNaOH(aq) were combined, and Mg(OH)2(s) precipitated, as shown by the equation above. If the experiment is repeated using solutions of the same molarity, which of the following changes in volume will double the amount of Mg(OH)2(s) produced?

Using twice the volume of MgCl2(aq) and twice the volume of NaOH(aq)

Using the same volume of MgCl2(aq) but twice the volume of NaOH(aq)

Using twice the volume of MgCl2(aq) but half the volume of NaOH(aq)

Using twice the volume of MgCl2(aq) but the same volume of NaOH(aq)

C6H12O6 + 6O2 → 6CO2 + 6H2O The reaction between C6H12O6and O2is represented by the balanced equation above. In anexperiment, 0.30 mol of CO2was produced from the reaction of 0.05 mol of C6H12O6withexcess O2. The reaction was repeated at the same temperature and in the same container, but this time0.60 mol of CO2was produced. Which of the following must be true?

The initial amount of C6 H12O6 in the container must have been 0.10 mol

Exactly 0.30 mol of C6 H12O6 must have reacted because C atoms were conserved.

Exactly 0.40 mol of O2 must have reacted because the temperature and container volume are the same.

More than 0.60 mol of O2 must have reacted because it was present in excess.

Fe(s) + 2HCl(aq) →FeCl2(aq) + H2(g) When a student adds 30.0 mL of 1.00 M HCl to 0.56 g of powdered Fe, a reaction occurs according to the equation above. When the reaction is complete at 273 K and 1.0 atm, which of the following is true?

0.22 L of H2 has been produced.

HCl is in excess, and 0.100 mol of HCl remains unreacted.

HCl is in excess, and 0.020 mol of HCl remains unreacted.

0.015 mol of FeCl2 has been produced.

MnO4− + 5 Fe2+ + 8 H+ → Mn2+ + 5 Fe3+ + 4 H2O In the reaction represented above, the number of MnO4- ions that react must be equal to which of the following?

A One-fifth the number of Fe2+ ions that are consumed

B Eight times the number of H+ ions that are consumed

C Five times the number of Fe3+ ions that are produced

D One-half the number of H2 O molecules that are produced

Potassium hydrogen phthalate, KHP, is used as a primary standard for determining the concentration of a solution of NaOH by titration. If the KHP has not been dried before weighing, the calculated molarity of the NaOH would be

higher than the actual value, since water is included in the apparent mass of KHP

higher than the actual value, since the presence of water requires a larger volume of titrant

C lower than the actual value, since NaOH absorbs water

D unaffected, since KHP is a strong acid

E unaffected, since water is routinely added before the titration

5 H2O2(aq) + 2 MnO4-(aq) + 6 H+(aq) → 2 Mn2+(aq) + 8 H2O(l)+ 5 O2(g) In a titration experiment, H2O2(aq) reacts with aqueous MnO4-(aq) as represented by the equation above. The dark purple KMnO4solution is added from a buret to a colorless,acidified solution of H2O2(aq) in an Erlenmeyer flask. (Note: At the end point of thetitration, the solution is a pale pink color.) Which of the following best describes what happens to the pH of the H2 O2solution as thetitration proceeds?

C As H+ ions are consumed, the solution becomes less acidic and the pH increases.

A The +2 charge on the manganese ions maintains the acidity of the solution.

B The production of water dilutes the solution, making it basic.

D As H+ ions are consumed, the solution becomes less acidic and the pH decreases.

When a buret is rinsed before a titration, which of the techniques below is the best procedure?

D Rinse the buret two times: each time with some of the titrant solution.

A Rinse the buret one time with some of the titrant solution.

B Rinse the buret one time with some of the titrant solution and then dry the buret in an oven.

C Rinse the buret two times: once with some of the titrant solution, then once with distilled water.

E Rinse the buret two times: each time with distilled water.

A student pipetted five 25.00–milliliter samples of hydrochloric acid and transferred each sample to an Erlenmeyer flask, diluted it with distilled water, and added a few drops of phenolphthalein to each. Each sample was then titrated with a sodium hydroxide solution to the appearance of the first permanent faint pink color. The following results were obtained. Volumes of NaOH Solution: 35.22 mL , 36.14 mL , 36.13 mL , 36.15 mL and 36.12 mL Which of the following is the most probable explanation for the variation in the student’s results?

D The pipette was not rinsed with the HCI solution.

The burette was not rinsed with NaOH solution.

The student misread a 5 for a 6 on the burette when the first sample was titrated.

C A different amount of water was added to the first sample.

E The student added too little indicator to the first sample.

I2(aq) + C6H8O6(aq) → C6H6O6(aq) + 2I−(aq) + 2H+(aq) The compound C6H8O6reacts with I2according to the reaction represented by the equation above. The reaction is correctly classified as which of the following types?

D Oxidation-reduction, because I2 is reduced.

A Acid-base, because H+ ions are produced.

B Precipitation, because there are only two reactants but there are three products.

C Double replacement, because both H and I appear as ions in the products.

2 H2 O2(aq) → 2 H2 O(l) + O2(g) The decomposition of H2 O2(aq) is represented by the equation above. Which of the following identifies the element(s) being oxidized and reduced in the reaction?

C Oxygen is both oxidized and reduced.

A Hydrogen is oxidized and oxygen is reduced.

B Oxygen is oxidized and hydrogen is reduced.

D No elements are oxidized or reduced; the reaction is not a redox reaction.

5 H2O2(aq) + 2 MnO4-(aq) + 6 H+(aq) → 2 Mn2+(aq) + 8 H2O(l)+ 5 O2(g) In a titration experiment, H2 O2(aq) reacts with aqueous MnO4 - (aq) as represented by the equation above. The dark purple KMnO4solution is added from a buret to a colorless, acidified solution of H2 O2(aq) in an Erlenmeyer flask. (Note: At the end point of the titration, the solution is a pale pink color.) Which element is being oxidized during the titration, and what is the element’s change in oxidation number?

A Oxygen, which changes from -1 to 0

B Oxygen, which changes from 0 to -2

C Manganese, which changes from -1 to +2

D Manganese, which changes from +7 to +2

Unit 4 Test Study Guide

Authored by Amanda Oldson

Science

12th Grade

NGSS covered

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following best describes the change that takes place immediately after the
CH3
OH(l) is introduced into the previously evacuated vessel?

A A chemical change takes place because covalent bonds are broken.

B A chemical change takes place because intermolecular attractions are overcome.

C A physical change takes place because covalent bonds are broken.

D A physical change takes place because intermolecular attractions are overcome.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

2 H2 O2(l) → 2 H2 O(l) + O2(g)
The exothermic process represented above is best classified as a

A physical change because a new phase appears in the products.

B physical change because O2(g) that was dissolved comes out of solution

C chemical change because entropy increases as the process proceeds.

D chemical change because covalent bonds are broken and new covalent bonds are

formed.

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

HCl(aq) + NaOH(aq) → NaCl(aq) + H2 O(l)
A student had two dilute, colorless solutions, HCl(aq) and NaOH(aq), which were at the same
temperature. The student combined the solutions, and the reaction represented above
occurred. Which of the following results would be evidence that a chemical reaction took
place?

A The resulting solution is colorless.

B The temperature of the reaction mixture increases.

C The total volume of the mixture is approximately equal to the sum of the initial

volumes.

D The resulting solution conducts electricity.

Tags

NGSS.MS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A student was asked to formulate a hypothesis about what would happen if 100.mL of
0.1MNaOH(aq) at 25°C was combined with 100.mL of 0.1MMgCl2(aq) at 25°C .
Which of the following hypotheses indicates that the student thought a chemical change
would occur?

A The volume of the resulting solution will be equal to the sum of the volumes of the

original solutions.

B The mass of the resulting solution will be equal to the sum of the masses of the original

solutions.

C The resulting solution would contain a precipitate.

D The resulting solution will be clear.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A student was studying physical and chemical changes. The student carried out some
procedures in the laboratory and recorded observations. For one of the procedures,
the student concluded that a physical change took place, but not a chemical change.
Which of the following could have been the results of the procedure?

A A cube of metal was changed into a flat sheet of metal.

B When two liquids at room temperature were combined in a beaker, the beaker became hot.

C When two clear liquids were combined, the resulting mixture was cloudy.

When a colorless liquid was added to a blue liquid, the resulting solution was yellow.

Tags

NGSS.MS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

At 127°C, the pressure in vessel 1 is found to be higher than that in vessel 2. Which of the
following reactions best accounts for the observation?

A NaHCO3(s) → Na(s) + HCO3(s)

B NaHCO3(s) → NaH(s) + CO3(s)

C 2 NaHCO3(s) → Na2 CO3(s) + CO2(g) + H2 O(g)

D 2 NaHCO3(s) + N2(g) → 2 NaNO3(s) + C2 H2(g)

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following is the net ionic equation for the reaction between aqueous sodium fluoride and hydrochloric acid?

A NaF(aq) + HCl(aq) → NaCl(aq) + HF(aq)

B Na+ (aq) + F− (aq) + H+(aq) + Cl−(aq) → Na+(aq) + Cl− (aq) + HF(aq)

C Na+(aq) + Cl−(aq) → NaCl(aq

D F−(aq) + H+(aq) → HF(aq)

Tags

NGSS.HS-PS1-7

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Unit 4 Test Study Guide

Which of the following best describes the change that takes place immediately after theCH3OH(l) is introduced into the previously evacuated vessel?

2 H2 O2(l) → 2 H2 O(l) + O2(g)The exothermic process represented above is best classified as a

A student was asked to formulate a hypothesis about what would happen if 100.mL of0.1MNaOH(aq) at 25°C was combined with 100.mL of 0.1MMgCl2(aq) at 25°C .Which of the following hypotheses indicates that the student thought a chemical changewould occur?

At 127°C, the pressure in vessel 1 is found to be higher than that in vessel 2. Which of thefollowing reactions best accounts for the observation?

Which of the following is the net ionic equation for the reaction between aqueous sodium fluoride and hydrochloric acid?

Equal volumes of 0.2M solutions of lead(II) nitrate and potassium bromide arecombined to form lead(II) bromide as a yellow precipitate. Which of the following is thecorrect net ionic equation for the reaction?

The reaction between aqueous strontium chloride (SrCl2) and aqueous potassium sulfate(K2SO4) forms a precipitate of strontium sulfate (SrSO4) . Which of the followingrepresents the net ionic equation for the reaction?

. . . C10H12O4 S(s) + . . . O2(g) → . . . CO2(g) + . . . SO2(g) + . . . H2O(g)When the equation above is balanced and all coefficients are reduced to their lowestwhole-number terms, the coefficient for O2(g) is

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Which of the following best describes the change that takes place immediately after the
CH3
OH(l) is introduced into the previously evacuated vessel?

2 H2 O2(l) → 2 H2 O(l) + O2(g)
The exothermic process represented above is best classified as a

A student was asked to formulate a hypothesis about what would happen if 100.mL of
0.1MNaOH(aq) at 25°C was combined with 100.mL of 0.1MMgCl2(aq) at 25°C .
Which of the following hypotheses indicates that the student thought a chemical change
would occur?

At 127°C, the pressure in vessel 1 is found to be higher than that in vessel 2. Which of the
following reactions best accounts for the observation?

Equal volumes of 0.2M solutions of lead(II) nitrate and potassium bromide are
combined to form lead(II) bromide as a yellow precipitate. Which of the following is the
correct net ionic equation for the reaction?

The reaction between aqueous strontium chloride (SrCl2) and aqueous potassium sulfate(K2SO4) forms a precipitate of strontium sulfate (SrSO4) . Which of the following
represents the net ionic equation for the reaction?

. . . C10H12O4 S(s) + . . . O2(g) → . . . CO2(g) + . . . SO2(g) + . . . H2O(g)
When the equation above is balanced and all coefficients are reduced to their lowest
whole-number terms, the coefficient for O2(g) is