Question 1

Identify the spectator ions in the following molecular equation. K Br(aq)+ AgNO3(aq)→ Ag Br(s)+ KNO3(aq)

Accepted Answer

A)  Ag+ and Br- 
B)  K+ and NO3- 
C)  K+ and Br- 
D)  Ag+ and NO3- 
E)  There are no spectator ions in this reaction. 
A)  Ag+ and Br- 
B)  K+ and NO3- 
C)  K+ and Br- 
D)  Ag+ and NO3- 
E)  There are no spectator ions in this reaction.

Question 2

What is the concentration (M)of sodium ions in 4.57 L of a .533 M   P solution?

Accepted Answer

The answer of What is the concentration (M)of sodium ions...

Question 3

Identify Na Cl.

Accepted Answer

A)  weak acid 
B)  weak electrolyte 
C)  strong acid 
D)  strong electrolyte 
E)  nonelectrolyte 
A)  weak acid 
B)  weak electrolyte 
C)  strong acid 
D)  strong electrolyte 
E)  nonelectrolyte

Question 4

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:   (aq)+   (aq)→   (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion.How many milliliters of 3.550 M HI(aq)must be added to a solution containing 0.500 mol of   to completely precipitate the lead?

Accepted Answer

A)  3.55 × 10-3 mL 
B)  282 mL 
C)  141 mL 
D)  0.141 mL 
E)  0.282 mL 
A)  3.55 × 10-3 mL 
B)  282 mL 
C)  141 mL 
D)  0.141 mL 
E)  0.282 mL

Question 5

Choose the statement below that is TRUE.

Accepted Answer

A)  A weak acid solution consists of mostly nonionized acid molecules. 
B)  The term "strong electrolyte" means that the substance is extremely reactive. 
C)  A strong acid solution consists of only partially ionized acid molecules. 
D)  The term "weak electrolyte" means that the substance is inert. 
E)  A molecular compound that does not ionize in solution is considered a strong electrolyte. 
A)  A weak acid solution consists of mostly nonionized acid molecules. 
B)  The term "strong electrolyte" means that the substance is extremely reactive. 
C)  A strong acid solution consists of only partially ionized acid molecules. 
D)  The term "weak electrolyte" means that the substance is inert. 
E)  A molecular compound that does not ionize in solution is considered a strong electrolyte.

Question 6

According to the following reaction,what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2.
2 KCl(aq)+ Pb(NO3)2(aq)→ PbCl2(s)+ 2 KNO3(aq)

Accepted Answer

A)  7.19 g 
B)  3.59 g 
C)  1.80 g 
D)  5.94 g 
E)  1.30 g 
A)  7.19 g 
B)  3.59 g 
C)  1.80 g 
D)  5.94 g 
E)  1.30 g

Question 7

What volume (in mL)of 0.0887 M Mg Br2 solution is needed to make 275.0 mL of 0.0224 M Mg Br2 solution?

Accepted Answer

A)  72.3 mL 
B)  91.8 mL 
C)  10.9 mL 
D)  69.4 mL 
E)  14.4 mL 
A)  72.3 mL 
B)  91.8 mL 
C)  10.9 mL 
D)  69.4 mL 
E)  14.4 mL

Question 8

Define an electrolyte.

Accepted Answer

A substance that dis

Question 9

Calculate the concentration (M)of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250 mL.

Accepted Answer

The answer of Calculate the concentration (M)of sodium ions in...

Question 10

Determine the oxidation state of C in CO3-2.

Accepted Answer

A)  +4 
B)  +2 
C)  -2 
D)  -4 
E)  +6 
A)  +4 
B)  +2 
C)  -2 
D)  -4 
E)  +6

Question 11

A beaker contains 0.50 mol of potassium bromide in 600 mL of water.An additional 600 mL of water is added.The number of moles of potassium bromide in the beaker is

Accepted Answer

A)  0.50 mol. 
B)  0.83 mol. 
C)  0.25 mol. 
D)  1.2 mol. 
E)  0.42 mol. 
A)  0.50 mol. 
B)  0.83 mol. 
C)  0.25 mol. 
D)  1.2 mol. 
E)  0.42 mol.

Question 12

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

Accepted Answer

A)  1.50 M 
B)  1.18 M 
C)  0.130 M 
D)  0.768 M 
E)  2.30 M 
A)  1.50 M 
B)  1.18 M 
C)  0.130 M 
D)  0.768 M 
E)  2.30 M

Question 13

What causes a precipitation reaction to occur between two soluble compounds?

Accepted Answer

A precipitate,or insoluble com

Question 14

Identify the oxidation state of Ca in Ca Br2(aq). Ca(s)+ 2H Br(aq)→ Ca Br2(aq)+ H2(g)

Accepted Answer

A)  +1 
B)  +2 
C)  0 
D)  -1 
E)  -2 
A)  +1 
B)  +2 
C)  0 
D)  -1 
E)  -2

Question 15

How many ions are present in 30.0 mL of 0.600 M H2CO3 solution?

Accepted Answer

A)  3.25 × 1022 ions 
B)  2.17 × 1022 ions 
C)  1.08 × 1022 ions 
D)  5.42 × 1022 ions 
E)  3.61 × 1021 ions 
A)  3.25 × 1022 ions 
B)  2.17 × 1022 ions 
C)  1.08 × 1022 ions 
D)  5.42 × 1022 ions 
E)  3.61 × 1021 ions

Question 16

What is the concentration of magnesium ions in a 0.125 M Mg SO4 solution?

Accepted Answer

A)  0.125 M 
B)  0.0625 M 
C)  0.375 M 
D)  0.250 M 
E)  0.160 M 
A)  0.125 M 
B)  0.0625 M 
C)  0.375 M 
D)  0.250 M 
E)  0.160 M

Question 17

Which of the following is considered a strong electrolyte?

Accepted Answer

A)  NH4NO3 
B)  C12H22O11 
C)  Pb I2 
D)  HC2H3O2 
E)  CH3SH 
A)  NH4NO3 
B)  C12H22O11 
C)  Pb I2 
D)  HC2H3O2 
E)  CH3SH

Question 18

What precipitate is most likely formed from a solution containing Ba+2,K+1,OH-1,and CO3-2.

Accepted Answer

A)  KOH 
B)  BaCO3 
C)  K2CO3 
D)  Ba(OH)2 
A)  KOH 
B)  BaCO3 
C)  K2CO3 
D)  Ba(OH)2

Question 19

Determine the oxidation state of nitrogen in RbNO2.

Accepted Answer

A)  +5 
B)  +3 
C)  0 
D)  +2 
E)  +4 
A)  +5 
B)  +3 
C)  0 
D)  +2 
E)  +4

Question 20

What are the coefficients in front of NO3-(aq)and Mg(s)when the following redox equation is balanced in an acidic solution?
________ NO3-(aq)+ ________ Mg(s)→ ________ NO(g)+ ________ Mg2+(aq)?

Accepted Answer

A)  2, 3 
B)  2, 6 
C)  3, 4 
D)  3, 6 
A)  2, 3 
B)  2, 6 
C)  3, 4 
D)  3, 6

Exam 9: Introduction to Solutions and Aqueous Reactions

Identify the spectator ions in the following molecular equation. K Br(aq)+ AgNO3(aq)→ Ag Br(s)+ KNO3(aq)

What is the concentration (M)of sodium ions in 4.57 L of a .533 M P solution?

Identify Na Cl.

Choose the statement below that is TRUE.

According to the following reaction,what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2. 2 KCl(aq)+ Pb(NO3)2(aq)→ PbCl2(s)+ 2 KNO3(aq)

What volume (in mL)of 0.0887 M Mg Br2 solution is needed to make 275.0 mL of 0.0224 M Mg Br2 solution?

Define an electrolyte.

Calculate the concentration (M)of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250 mL.

Determine the oxidation state of C in CO3-2.

A beaker contains 0.50 mol of potassium bromide in 600 mL of water.An additional 600 mL of water is added.The number of moles of potassium bromide in the beaker is

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

What causes a precipitation reaction to occur between two soluble compounds?

Identify the oxidation state of Ca in Ca Br2(aq). Ca(s)+ 2H Br(aq)→ Ca Br2(aq)+ H2(g)

How many ions are present in 30.0 mL of 0.600 M H2CO3 solution?

What is the concentration of magnesium ions in a 0.125 M Mg SO4 solution?

Which of the following is considered a strong electrolyte?

What precipitate is most likely formed from a solution containing Ba+2,K+1,OH-1,and CO3-2.

Determine the oxidation state of nitrogen in RbNO2.

What are the coefficients in front of NO3-(aq)and Mg(s)when the following redox equation is balanced in an acidic solution? ________ NO3-(aq)+ ________ Mg(s)→ ________ NO(g)+ ________ Mg2+(aq)?

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Identify the spectator ions in the following molecular equation. K Br(aq)+ AgNO₃(aq)→ Ag Br(s)+ KNO₃(aq)

According to the following reaction,what mass of PbCl₂ can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO₃)₂. 2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

What volume (in mL)of 0.0887 M Mg Br₂ solution is needed to make 275.0 mL of 0.0224 M Mg Br₂solution?

Determine the oxidation state of C in CO₃^-2.

Identify the oxidation state of Ca in Ca Br₂(aq). Ca(s)+ 2H Br(aq)→ Ca Br₂(aq)+ H₂(g)

How many ions are present in 30.0 mL of 0.600 M H₂CO₃ solution?

What is the concentration of magnesium ions in a 0.125 M Mg SO₄ solution?

What precipitate is most likely formed from a solution containing Ba⁺²,K⁺¹,OH^-1,and CO₃^-2.

Determine the oxidation state of nitrogen in RbNO₂.

What are the coefficients in front of NO₃^-(aq)and Mg(s)when the following redox equation is balanced in an acidic solution? NO₃^-(aq)+ Mg(s)→ NO(g)+ Mg²⁺(aq)?