Equal volumes of 0.2⁢ M 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?

Pb 2+ (aq) + Br - (aq) → PbBr 2 (s)

K + (aq) + NO 3 - (aq) → KNO 3 (aq)

Pb 2+ (aq) + 2 NO 3 - (aq) + 2 K + (aq) + 2 Br - (aq) → 2 NO 3 - (aq) + 2 K + (aq) + PbBr 2 (s)

Pb(NO 3 ) 2 (aq) + 2 KBr(aq) → PbBr 2 (s) + 2 KNO 3 (aq)

The reaction between aqueous strontium chloride (SrCl 2 ) and aqueous potassium sulfate (K 2 SO 4 ) forms a precipitate of strontium sulfate (SrSO 4 ). Which of the following represents the net ionic equation for the reaction?

Sr 2+ (aq) + SO 4 - (aq) → SrSO 4 (s)

K + (aq) + Cl - (aq) → KCl(aq)

Sr 2+ (aq) + 2 Cl - (aq) + 2 K + (aq) + SO 4 - (aq) → 2 Cl - (aq) + 2 K + (aq) + SrSO 4 (s)

SrCl 2 (aq) + K 2 SO 4 (aq) → SrSO 4 (s) + 2 KCl(aq)

A 20. mL sample of 0.50 M HC 2 H 3 O 2 ( aq ) is titrated with 0.50 M NaOH( aq ). Which of the following best represents the species that react and the species produced in the reaction?

HC 2 H 3 O 2 ( aq ) + OH - ( aq ) → C 2 H 3 O 2 - ( aq ) + H 2 O( l )

H + ( aq ) + OH − ( aq ) → H 2 O( l )

H + ( aq ) + C 2 H 3 O 2 − ( aq ) + Na + ( aq ) + OH − ( aq ) → H 2 O( l ) + NaC 2 H 3 O 2 (aq)

HC 2 H 3 O 2 ( aq ) + NaOH( aq ) → H 2 O( I ) + Na + ( aq ) + C 2 H 3 O 2 - ( aq )

Which of the following describes the changes in forces of attraction that occur as H 2 O changes phase from a liquid to a vapor?

Hydrogen bonds between H 2 O molecules are broken.

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

Covalent bonds between H 2 O molecules are broken.

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

Covalent bonds between H + ions and H 2 O molecules become more effective.

A student places a sample of a pure metal in a crucible and heats it strongly in air. Data from the experiment are given in the table above. The final mass was determined after the sample was cooled to room temperature. 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 the 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?

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

The solution does not change color after stirring.

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

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

The table above summarizes data given to a student to evaluate the type of change that took place when substance X was mixed with water. The student claimed that the data did not provide enough evidence to determine whether a chemical or physical change took place and that additional tests were needed. 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

Fe(s) + 2 HCl(aq) → FeCl 2 (aq) + H 2 (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 H 2 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 FeCl 2 has been produced.

2F 2 (g) + 2 NaOH(aq) → OF 2 (g) + 2 NaF(aq) + H 2 O(l) A 2mol sample of F 2 (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 F 2 (g), which of the following is correct?

The amount of OF 2 (g) produced is halved.

The amount of OF 2 (g) produced is doubled.

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

The amount of NaF(aq) produced is doubled.

MgCl 2 (aq) + 2 NaOH(aq) → 2 NaCl(aq) + Mg(OH) 2 (s) A 100mL sample of 0.1 M MgCl 2 (aq) and a 100mL sample of 0.2 M NaOH(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 MgCl 2 (aq) and twice the volume of NaOH(aq)

Using the same volume of MgCl 2 (aq) but twice the volume of NaOH(aq)

Using twice the volume of MgCl 2 (aq) but half the volume of NaOH(aq)

Using twice the volume of MgCl 2 (aq) but the same volume of NaOH(aq)

Select a reaction in which the same reactant undergoes both oxidation and reduction

3 Br 2 ( aq ) + 6 OH - ( aq ) → 5 Br - ( aq ) + BrO 3 - ( aq ) + 3 H 2 O( l )

H 2 SeO 4 ( aq ) + 2 Cl - ( aq ) + 2 H + ( aq ) → H 2 SeO 3 ( aq ) + Cl 2 ( g ) + H 2 O( l )

S 8 ( s ) + 8 O 2 ( g ) → 8 SO 2 ( g )

Ca 2+ ( aq ) + SO 4 2- ( aq ) → CaSO 4 ( s )

PtCl 4 ( s ) + 2 Cl - ( aq ) → PtCl 6 2- ( aq )

Select a precipitation reaction

Pb 2+ ( aq ) + CrO 4 2- ( aq ) → PbCrO 4 ( s )

2 Mg( s ) + O 2 ( g ) → 2 MgO( s )

SO 3 ( g ) + 2 H 2 O( l ) → H 3 O + ( aq ) + HSO 4 - ( aq )

2 H 2 O( g ) → 2 H 2 ( g ) + O 2 ( g )

Ag + ( aq ) + 2 NH 3 ( aq ) → [Ag(NH 3 ) 2 ] + ( aq )

Which chemical or physical change occurs when aqueous solutions of ammonia and vinegar are mixed?

Brønsted-Lowry acid-base reaction

Which chemical or physical change occurs when solid sodium acetate, NaC 2 H 3 O 2 ( s ), is added to water?

Brønsted-Lowry acid-base reaction

Cu( s ) + 4 HNO 3 ( aq ) → Cu(NO 3 ) 2 ( aq ) + 2 NO 2 ( g ) + 2 H 2 O( l ) Which of the following is true about the reaction?

It is a redox reaction, because Cu( s ) is oxidized and the nitrogen atom in NO 3 − ( aq ) is reduced.

It is a Brønsted-Lowry acid-base reaction, because the solution is neutral at the end.

It is a Brønsted-Lowry acid-base reaction, because HNO 3 ( aq ) is a strong acid.

It is a redox reaction, because Cu( s ) is oxidized and H + ( aq ) is reduced.

Which of the following correctly identifies a Brønsted-Lowry conjugate acid-base pair in a solution prepared by mixing together HNO 2 (aq) and NH 3 (aq) ?

The acid is HNO 2 (aq), and the conjugate base is NO 2 − (aq).

The acid is HNO 2 (aq), and the conjugate base is NH 3 (aq).

The acid is NH 4 + (aq), and the conjugate base is NO 2 − (aq).

The acid is NH 3 (aq), and the conjugate base is NH 4 + (aq).

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

lower than the actual value, since NaOH absorbs water

unaffected, since KHP is a strong acid

unaffected, since water is routinely added before the titration

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

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

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

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

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

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 First Sample.....35.22 mL Second Sample.....36.14 mL Third Sample.....36.13 mL Fourth Sample .....36.15 mL Fifth Sample.....36.12 mL Which of the following is the most probable explanation for the variation in the student’s results?

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.

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

The student added too little indicator to the first sample.

AP Chem Unit 4

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AP Chem Unit 4

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TRA-1.A, TRA-1.B, TRA-2.A

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AP Chem Unit 4

40 questions

2 H₂O₂(l) → 2 H₂O(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 0.1M NaOH(aq) at 25°C was combined with 100. mL of 0.1M MgCl₂(aq) at 25°C. Which of the following hypotheses indicates that the student thought a chemical change would occur?

Which of the following is the balanced net-ionic equation for the reaction between Li(s) and water?

A 0.50g sample of Mg(s) was placed in a solution of HCl(aq), where it reacted completely.
Which of the following equations best represents the reacting species in the reaction described above?

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

Equal volumes of 0.2⁢M 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?

A 20. mL sample of 0.50 M HC₂H₃O₂(aq) is titrated with 0.50 M NaOH(aq). Which of the following best represents the species that react and the species produced in the reaction?

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AP Chem Unit 4

40 questions

2 H2O2(l) → 2 H2O(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 0.1M NaOH(aq) at 25°C was combined with 100. mL of 0.1M MgCl2(aq) at 25°C. Which of the following hypotheses indicates that the student thought a chemical change would occur?

Which of the following is the balanced net-ionic equation for the reaction between Li(s) and water?

A 0.50g sample of Mg(s) was placed in a solution of HCl(aq), where it reacted completely.Which of the following equations best represents the reacting species in the reaction described above?

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

Equal volumes of 0.2⁢M 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?

A 20. mL sample of 0.50 M HC2H3O2(aq) is titrated with 0.50 M NaOH(aq). Which of the following best represents the species that react and the species produced in the reaction?

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2 H₂O₂(l) → 2 H₂O(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 0.1M NaOH(aq) at 25°C was combined with 100. mL of 0.1M MgCl₂(aq) at 25°C. Which of the following hypotheses indicates that the student thought a chemical change would occur?

A 0.50g sample of Mg(s) was placed in a solution of HCl(aq), where it reacted completely.
Which of the following equations best represents the reacting species in the reaction described above?

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?

A 20. mL sample of 0.50 M HC₂H₃O₂(aq) is titrated with 0.50 M NaOH(aq). Which of the following best represents the species that react and the species produced in the reaction?