Chemistry unit 8
Calculate the molarity of the solution. 4.32 x 102 moles of CH3COOH in 20.0 liters of water __M
21.6
Be sure to use proper significant figures for all remaining problems. How many grams of NaCl are present in 350 mL of 0.020 M NaCl solution? (Remember that 1 mole NaCl = 58.44 g/mole.) __g
0.41
Suppose that instead of a 1 M solution, you decided to make up a 0.5 M solution. How many moles of NaCl would there be in one liter?
0.5
With a 0.5 M solution: How many moles of NaCl would there be in 1,000 ml?
0.5
Look carefully at Data Table 1. Which requires more energy to dissolve, ionic or covalent compounds? covalent ionic
ionic
Solutions which can conduct electricity must contain: atoms molecules minerals ions
ions
Which expression defines molarity? #moles/Liter(solvent) #moles/#mole solution #moles/Liter solution none of these
#moles/Liter solution
Assign oxidation numbers to each element in this compound. KMnO₄ K = Mn = O =
+1 +7 -2
Assign oxidation numbers to each element in this compound. NO N = O =
+2 -2
Assign oxidation numbers to each element in this compound. MnO₂ Mn = O =
+4 -2
HBr + H₂SO₄ SO₂ + Br₂ + H₂O What is the oxidation number of the oxidizing agent? What is the oxidation number of the reducing agent?
+6 -1
SOLUTIONS
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QUIZ 1: TOOLBOX TO SOLUBILITY
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REDOX AND OXIDATION POTENTIALS
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THE DISSOLVING PROCESS
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THE SOLUBILITY CONSTANT
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PH CALCULATIONS
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QUIZ 2: TOOLBOX TO SOLUBILITY CONSTANT
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QUIZ 4: CHAPTER REVIEW
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TEST
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REDOX EQUILIBRIA
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ACID-BASE EQUILIBRIA
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PH SCALE
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QUIZ 3: TOOLBOX TO TITRATION
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TITRATION OF ACIDS AND BASES
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How many moles do 10.0 mg of CO represent?
0.000357
Which solution of NaI would be most dissociated? 0.1 M 0.8 M 0.3 M 0.6 M
0.1 M
Mass of Al wire before reaction = 3.96 g Mass of Al wire after reaction = 3.65 g Mass of Al lost = 0.31 g Moles of Al lost = 0.011 moles Mass of Pb + filter paper = 4.26 g Mass of filter paper = 0.92 g Mass of Pb = 3.34 g Moles of Pb formed = 0.016 moles Recall that there were 100 mL of solution. 0.016 moles of Pb were removed from the solution. What was the [Pb+2] for the saturated solution of PbCl2? Recall that there was 100 mL of solution. 0.016 moles of Pb were removed from the solution. Also recall the original equilibrium: PbCl2(s) <=> Pb+2(aq) + 2(Cl-)(aq) Since there are 2 Cl ions formed for every Pb ion, what was the [Cl-] for the saturated solution of PbCl2? __ M
0.16 0.32
A titration was performed in a lab situation. H2SO4 was titrated with NaOH. The following data was collected: mL of NaOH used = 43.2 mL concentration NaOH = 0.15 M mL H2SO4 = 20.5 mL Notice that H2SO4 releases 2 H+ per mole. What is the concentration of H2SO4? 0.036 M 0.16 M 0.63 M 6.3 M
0.16 M
The unknown concentration of NaOH was determined by titration with HCl. The following data was collected: mL NaOH = 34.8 mL mL of HCl used = 29.6 mL concentration of HCl = 0.19 M What is the concentration of the NaOH? 0.16 M 0.22 M 4.5 M 6.3 M
0.16 M
Complete the Data Table: Use these values: The atomic mass of Al is 27.0 g/mole. The atomic mass of Pb is 207.2 g/mole. Use two significant digits for your answers: Mass of Al wire before reaction = 3.96 g Mass of Al wire after reaction = 3.65 g Mass of Al lost = __ g Moles of Al lost = __ moles Mass of Pb + filter paper = 4.26 g Mass of filter paper = 0.92 g Mass of Pb = __ g Moles of Pb formed = __ moles
0.31 0.011 3.34 0.016
You now know that [Pb+2] = 0.17 M. Calculate [Cl-]. Refer to equations given in the text to determine the relationship between these ions. 0.17 M 0.26 M 0.34 M 0.51 M
0.34 M
What is the required molarity of a Ba(OH)₂ solution to prepare a 1.0 M OH⁻ solution? ____ M
0.5
Calculate the molarity of solution given the following information: 10.0 g of NaOH were dissolved in 500.0 mL of solution. 0.020 M 0.500 M 5.00 M 20.0 M
0.500 M
Determine the number of grams of NaCl necessary to make up 100 mL of a 0.10 M solution. 0.017 g 0.58 g 1.7 g 58 g
0.58 g
How many moles of CO2 are in 870 mL of a 0.75 M solution? ____ moles
0.65
How many grams of CO are in 125 mL of a 0.25 M solution? 0.87 g 1.1 g 14 g 880 g
0.87 g
What is the pH of a 0.1 M acid solution?
1
Complete the following table. Acid Molarity Moles of H⁺ released per liter HCl 1 H2SO4 1 H3PO4 1 H2SO4 0.5 H3PO4 3 HNO3 2
1 2 3 1 9 2
How many moles of NaOH are needed to make a 1 M solution? 1 mole 6.023 moles 39.998 moles
1 mole
If the [H+] changed from [1 x 10-7] to [1 x 10-4], what is the new [OH-]? 1 x 10 -7 1 x 10 -4 1 x 10 -3 1 x 10 -10
1 x 10 -10
In a solution with a pH of 4, the [OH-] is: 1 x 10 -10 4 1 x 10 -4 10 1 x 10 -8
1 x 10 -10
A solution with a pH of 11 has a [H+] of: 11 1 x 10 -3 1 x 10 -11 1 x 10 11 1 x 10 3
1 x 10 -11
If you made up a solution of NaOH by adding 0.010 mole of solid NaOH to 1.0 liter of distilled water, what would be the concentration of the OH-(aq)? 1 M 1 x 10 -1M 1 x 10 -2M 1 x 10 -4M
1 x 10 -2M
The pH of an acetic acid solution is 4.0. (10n = 1en). Calculate the [H+]. _____ moles/liter What is the [OH-? _____ moles/liter
1 x 10 -4 1 x 10 -10
A solution has a [Ag+(aq)] of 0.01 M. The chloride concentration in solution is 1 x 10-5 M. Based on the following reaction, answer the following questions: AgCl(s) Ag+(aq) + Cl-(aq), Ksp = 1.7 x 10-10 Calculate the value of the current solubility product. Is the K value obtained greater or less than Ksp? Will a precipitate of AgCl form?
1 x 10 -7 greater yes
Match the grams of each element or compound to the corresponding number of moles of that element or compound. 1. 10.0 g H 2. 0.25 g Na 3. 1.0 x 102 mg H2O
1-9.92 moles 2-0.011 3-0.0056
Match the acids with their common names. 1. HNO3 2. HCl 3. H2SO4 4. HF 5. H2CO3 6. H3PO4
1-Nitric 2-Hydrochloric 3-Sulfuric 4-Hydrofluoric 5-Carbonic 6-Phosphoric
Match the following. 1. the electrode within an electrochemical cell where oxidation occurs 2. the electrode within an electrochemical cell where reduction occurs 3. the voltage associated with the electron transfer within an electrochemical cell
1-anode 2-cathode 3-oxidation
1. increased surface area 2. like dissolves like 3. temperature 4. stirring
1-finely divided solute 2-matching polarity 3-rate proportional to kinetic energy 4-spreads solute throughout solution
Match these items. 1. moles per liter of solution 2. spreading out 3. substance being dissolved 4. general equilibrium constant 5. the substance doing the dissolving in a solution 6. solubility product constant
1-molarity 2-diffusion 3-solute 4-Keq 5-solvent 6-Ksp
1. The negative log of the hydrogen ion concentration of a solution; a scale ranging from 0 to 14 with 7 being neutral, values less than 7, acidic and greater than 7, basic 2. The product of a neutralization reaction, a substance consisting of a positive ion from the base and a negative ion from the acid 3. The reaction which occurs between acids and bases
1-pH 2-salt 3-neutralization
Match the following related items. 1. gain of electrons 2. low E0 3. loss of electrons 4. high E0 5. negative ions 6. positive ions 7. migrate to cathode 8. migrate to anode
1-reduction 2-strong oxidizer 3-oxidation 4-weak oxidizer 5-anion 6-cation 7- positive ions 8- negative ions
What is the atomic mass of one mole of H?
1.008 g/mole
A solution has a pH of 2.5. Answer the following questions. pOH = [H+] = [OH-] =
11.5 3.2 x 10 -3 3.2 x 10 -12
What is the pH of a 0.1 M basic solution?
13
The sum of pH and pOH for any aqueous solution equals .
14
Determine the molecular weight for Mg(NO3)2. 134.32 g 118.32 g 148.33 g 172.64 g
148.33 g
What is the atomic mass of one mole of O?
16.00 g/mole
Determine the molecular weight of H2O. 18 g 18.0 g 18.01 g 18.016 g
18.016 g
What is the molecular weight of one mole of H2O?
18.016 g/mole
Determine the number of ions produced in the dissociation of the compound listed. BaS
2
Determine the number of ions produced in the dissociation of the compound listed. CaO
2
Determine the number of ions produced in the dissociation of the compound listed. KCl
2
Determine the number of ions produced in the dissociation of the compound listed. NaF
2
For every Pb+2 ion that is formed, how many Cl- ions are formed? (Refer to the reaction in the lesson above.)
2
For every mole of Pb⁺² ions that are formed, how many moles of Cl⁻ ions are formed? (Refer to the reaction in the lesson above.)
2
Balance the reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coefficient is "1." __H₂O₂ → __H₂O + __O₂
2 2 blank
Balance this chemical equation. Choose "blank" for the box if no other coefficient is needed. Writing the symbol implies "1." __H2O2 → __H2O + __O2
2 2 blank
Balance the reactions which form ions. Choose "blank" if no other coefficient is needed. Writing the symbol implies "1." (NH4)2CO3 <=> __NH4+ + __CO3 -2
2 blank
Balance the reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coefficient is "1." __ HCl + __Zn →__ ZnCl2 + __H2
2 blank blank blank
When one mole of sodium chloride dissociates in water, it produces: 1 mole of ions ½ mole of sodium ions 2 moles of ions ½ mole of chloride ions none of these
2 moles of ions
Sulfuric acid dissolves in water as H2SO4 2 H+(aq) + SO2 -2(aq). Which of the following solutions of H2SO4 will conduct the most electricity? 1.0 M 1.0 N 2.0 M 0.5 M
2.0 M
If the pH value was 3.6, what is the [H+]? 2.5 x 10-4 4.0 x 103
2.5 x 10 -4
What is the atomic mass of one mole of Na?
22.99 g/mole
The molecular weight of CaCl2 is 110.98 g/mol. In order to make up 500. mL of a 0.500 M solution, you need: 55.6 g 27.7 g 222.2 g 111.1 g 34.4 g
27.7 g
Potassium fluoride (KF, a salt, has a molecular weight of 58.10 grams. How many grams would be needed to make 1.0 liter of 5.0 molar salt solution? 3.4 x 10-3 g 12 g 29 g 290 g
290 g
The equation for the reaction between Al(s) and Pb+2(aq) is: 2Al(s) + 3Pb+2(aq) <=> 2Al+2(aq) + 3Pb(s). Therefore, for each 2 moles of Al(s) that are used, how many moles of Pb(s) are formed? From the moles of Al(s) consumed, 0.011 moles, calculate the number of moles of Pb(s) that should have been formed: __ moles
3 0.017
N₂ + 3H₂ 2NH₃ How many molecules of H₂ are in the reactants? How many nitrogen atoms are present? How many moles of NH₃ are formed?
3 2 2
Balance the reactions which form ions. Choose "blank" if no other coefficient is needed. Writing the symbol implies "1." (NH4)3PO4 <=> __NH4+ + __PO4 +3
3 blank
What volume of 0.1 M NaOH is required to neutralize 30 mL of 0.1 M HCl? 15 mL 45 mL 30 mL 10 mL 60 mL
30 mL
Determine the molecular weight of Ca3(PO4)2. 278.18 g 279.21 g 310.18 g 430.42 g
310.18 g
3Fe + 4H2O Fe3O4 + 4H2 How many molecules of H2 are produced? How many oxygen atoms are required? How many moles of Fe3O4 are formed? What is the mole ratio of Fe to H2O? How many hydrogen atoms are involved in this reaction?
4 4 1 3/4 8
A solution has a [OH-] = 8.6 x 10-5. Answer the following questions. pOH = pH = [H+] =
4.1 9.9 1.3 x 10 -10
To verify the previous experiment, the chemistry student carried out the next experiment and recorded the data for you in the following Data Table. Directions: Place 100 mL of filtered, saturated PbCl2 in a 150 mL beaker and put it under a dryer to evaporate the water. Record the necessary data in the Data Table. Complete the Data Table. Molecular weight of PbCl2 = 278 g/mole Mass of beaker + PbCl2 = 62.19 g Mass of beaker = 57.77 g Mass of PbCl2 per 100 mL = __ g Moles PbCl2 per 100 mL = __ [Pb-2] based upon this investigation = __ M [Cl-] based upon this investigation = __ M
4.42 g 0.0159 0.159 0.318
If a solution had an [OH-] = 3.00 x 10-10 moles/liter, what would be the pH value of this solution? 3.53 4.48
4.48
Calculate the number of molecules in 0.75 moles of CH₄. _____ x 10²³ molecules
4.5
What would be the pH if the [H+] = 3.00 x 10-5 moles/liter? 4.52 5.48
4.52
Calculate the mass in grams of 0.800 mole of H2CO3. ___ g
49.6
Calculate the atomic mass in grams of 0.35 moles of CH4. 0.18 g 5.6 g 45 g
5.6 g
Potassium fluoride (KF), a salt, has a molecular weight of 58.10 grams. How many grams would be needed to mix 1.0 liter of 0.10 M salt solution? 0.17 g 580 g 17 g 5.8 g
5.8 g
A solution that is neutral has a pH of: 1 14 0 7 10
7
A neutral solution has a pH = . When a solution is basic, the pH is always greater than . When a solution is basic, the pOH is always less than .
7 7 7
What would the pOH of a solution be if the [H+] = 3.00 x 10-5 moles/liter? 8.52 9.48
9.48
The molecular weight of H2SO4 is: 49.078 g/mole 98.086 g/mole 194.296 g/mole
98.086 g/mole
Choose the strongest acid. Acid A, Ka = 2.3 x 10-8 Acid B, Ka = 2.5 x 10-6 Acid C, Ka = 8.3 x 10-7 Acid D, Ka = 1.4 x 10-7
Acid B, Ka = 2.5 x 10-6
Use the E0 values of the following elements: Zn, Cu, Pb, and Al. Which element is the most active reducing agent?
Al
Which of the following Gold compounds has the greatest solubility? Au(OH)3, Ksp = 1 x 10-53 AuCl3, Ksp = 3.2 x 10-25 AuCl, Ksp = 2.0 x 10-13 AuBr3, Ksp = 4.0 x 10-36
AuCl, Ksp = 2.0 x 10-13
Below are 5 sets of potential solutes for you to compare. Both members of each pair are very soluble in water. If you had equal molar concentrations of each solution, which member of each pair would theoretically be the better conductor of electricity? CsCl, CaCl2 CaS, Li2S KBr, AlCl3 AlCl3, MgC2 KI, K2S
CaCl2 Li2S AlCl3 AlCl3 K2S
Which of the following statements is true of cations? Cations are attracted to the anode. Cations undergo oxidation at the proper electrode. Cations undergo reduction at the proper electrode. Cations are negatively charged.
Cations undergo reduction at the proper electrode.
The reaction 2 Cu + O2 → 2 CuO has long been called an oxidation-reaction. Copper also reacts with chlorine: Cu + Cl2 → CuCl2. In such a reaction: Copper is also oxidized even though no oxygen is present. Chlorine is oxidized. Oxidation occurs, but reduction does not. There is no change in oxidation numbers.
Copper is also oxidized even though no oxygen is present.
Use the E0 values of the following elements: Zn, Cu, Pb, and Al. Which element is the most active oxidizing agent?
Cu
The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of NaCl. A white precipitate of PbCl2 formed. How will this affect the concentration of Pb+2? increase it decrease it remain constant
Decrease it(I said remain constant the first time and it was wrong)
2KClO3 2KCl + 3O2 In this equation, the number of atoms in the product is greater than the number of atoms in the reactant. True or False
False
2KClO3 2KCl + 3O2 The number of atoms in the product is greater than the number of atoms in the reactant. True or False
False
A base releases H+. True or False
False
A high percent of dissociation is always expected to yield a high conductivity. True or False
False
A salt will always precipitate out of solution when it is produced. True or False
False
A strong oxidizing agent will donate electrons readily. True or False
False
Acids should be tested by taste. True or False
False
All chemicals which contain OH in the formula are bases. True or False
False
Ammonia is a strong acid. True or False
False
An acid has OH- ions in its formula. True or False
False
Chemical reactions forming ions do not balance electrically. True or False
False
Covalent solutions are good conductors of electricity. True or False
False
Either oxidation or reduction can take place independently in any particular reaction. True or False
False
Hydrofluoric acid is listed in Table 10 as a weak acid; therefore, it is not very dangerous to handle. True or False
False
Ionic solutions are poor conductors of electricity. True or False
False
It is likely that Si and P would substitute for each other in a solid solution. True or False
False
Litmus turns blue in acidic solutions. True or False
False
Molarity is represented by the symbol m. True or False
False
Molecules are charged. True or False
False
Solid solutions are rare. True or False
False
Water has a large Ka value. True or False
False
When acids react with water, __ ions are released which then combine with water molecules to form ___.
H H3O+
Select the ion. Mg H+ HC2H3O2
H+
Select all that apply. Consider this system: CH3COOH(aq) H+(aq) + CH3COO- Ka = 1.8 x 10-5 What will happen to the equilibrium as OH- ions are added? H+ will combine with OH- to form water. [CH3COOH] will increase. The acid will dissociate to supply more H+. The reaction will move to the right. the reaction will move to the left.
H+ will combine with OH- to form water. The acid will dissociate to supply more H+. The reaction will move to the right.
Select the ion. HCl H2O H3O+1
H3O+1
How might you explain the difference between the pH values of the 0.01 M HCl (pH = 1.1) and the 0.01 M HC2H3O2 (pH = 3.6)? HCl produces less H+. HCl dissociates more. HC2H3O2 produces both H+ and OH-. HC2H3O2 produces more H+.
HCl dissociates more.
Which element must be present in an acid? hydrogen oxygen both hydrogen and oxygen
Hydrogen
The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of NaCl. A white precipitate of PbCl2 formed. You have ________ the Cl- concentration by adding NaCl.
Increased
Using a value of Ksp = 1.8 x 10-2 for the reaction PbCl2(s) Pb+2(aq) + 2Cl-(aq). The concentration of the products yields a value of 2.1 x 10-2. Select the TWO statements that are true. Ions are recombining to form a solid precipitate. The concentrations of Pb+2(aq) and Cl-(aq) are expected to decrease. The concentrations of Pb+2(aq) and Cl-(aq) are expected to increase. The concentration of PbCl2(s) is expected to increase. It is not possible to have a system with Ksp > 1.8 x 10-2.
Ions are recombining to form a solid precipitate. The concentrations of Pb+2(aq) and Cl-(aq) are expected to decrease.
What is the general equilibrium expression for an acid? Ka = [HB]/[H+][B-] Ka = [H+][B-]/[HB] Ka= [H+][A-]/[HA] Ka= [HA]/[H+][A-]
Ka = [H+][B-]/[HB]
Choose the Ksp expressions for the following reactions. Ca3(PO4)2(s) 3Ca+2 (aq) + 2PO4 -3(aq) Ksp = [Ca+2]2[PO4-3]2 Ksp = [Ca+2]3[PO4-3]3 Ksp = [Ca+2]3[PO4-3]2 Ksp = [Ca+2]2[PO4-3]3
Ksp = [Ca+2]3[PO4-3]2
Select all the species that are ions. HCl NaCl NH4+ H2PO4- CCl4 H3O+
NH4+ H2PO4- H3O+
The equation for the reaction between Al(s) and Pb+2(aq) is: 2Al(s) + 3Pb+2(aq) <=> 2Al+3(aq) + 3Pb(s) You know that 0.011 moles of Al(s) have been consumed and that 0.017 moles of Pb(s) have been formed. Calculate [Pb+2]. 0.0017 M 0.017 M 0.17 M 0.26 M
NOT 0.017 M
When a piece of magnesium is connected to an iron pipe, the iron is prevented from corroding. Which of the following is the best explanation? Magnesium reacts with the ground water to form a protective coat on the iron pipe of Mg(OH)2. Magnesium atoms replace the iron atoms lost when the iron corrodes. Electrons flow from the iron through the wire to the magnesium leaving a protective coating of Fe+3 on the pipe. When magnesium corrodes, electrons flow through the wire to the iron pipe, thus preventing the iron atoms from losing electrons. The electric current flowing through the ground from the magnesium to the iron kills the organisms which attack and corrode the pipe.
NOT Magnesium reacts with the ground water to form a protective coat on the iron pipe of Mg(OH)2. Probably Electrons flow from the iron through the wire to the magnesium leaving a protective coating of Fe+3 on the pipe.
When sodium sulfide dissociates in water, the sulfur ion reacts with water as follows: S-2 + H2O → OH- + SH- Which of the following statements is true? Na2S is a base because it ionizes to release OH-. Na2S is an acid because it is a proton donor. Na2S is a base because it increases the hydroxide concentration. none of these
NOT Na2S is a base because it ionizes to release OH- maybe Na2S is a base because it increases the hydroxide concentration.
Using a value of Ksp = 1.8 x 10-2 for the reaction PbCl2 Pb+2(aq) + 2Cl -(aq). If the value of Ksp was determined to be only 1.2 x 10-2: Too much solid has dissolved. Additional precipitate is forming. The solution is unsaturated. The ions are now combining to reduce their concentrations.
NOT the ions are now combining to reduce their concentrations maybe the solution is unsaturated
Compare the pH of 0.1 M Na2CO3 and 0.1 M NaHCO3. Select the statements that explain the difference. Na2CO3 is a stronger base. NaHCO3 is a stronger base. Na2CO3 puts more OH- ion into solution.
Na2CO3 is a stronger base. Na2CO3 puts more OH- ion into solution.
Select the compound in which chlorine is assigned the oxidation number +5. HClO4 HClO2 HCl NaClO3 HClO
NaClO3
Which of the following would be expected to form ionic solutions in water? CO2 C NaI CCl4 O2
NaI
Select all of the following that are salts. NaNO3 (NH4)2SO4 H2SO4 NH3 NH4OH NaCl NH4Cl
NaNO3 (NH4)2SO4 NaCl NH4Cl
Select the ion. Cu PO4-3 SO2
PO4-3
Select all the items on the following list that are ions. Cu PO4-3 HCO3- Al+3 Hg2+2 Na2CO3 Fe Zn
PO4-3 HCO3- Al+3 Hg2+2
HBr + H₂SO₄ SO₂ + Br₂ + H₂O Oxidizing agent = Reducing agent =
S Br
Sn = 0.14 (E0) Sn+2 = -0.15 (E0) Which form of tin is more likely to give up electrons? Sn Sn+2
Sn
Sn =0.14 (E0) Sn+2 = -0.15 (E0) Which form of tin is the stronger reducing agent? Sn Sn+2
Sn
Which of these solutions will be the best conductor of electricity? Solution A: All Neutral particles Solution B: Positive ions, Negative ions, and Neutral particles Solution C: Positive ions and Negative ions
Solution C
The values used in the scale of pH and pOH are derived from a system designed by ______. Gordonsen Sorenson Curie Dalton
Sorenson
If solid NaCl is added to a saturated water solution of PbCl2 at 20o C, a precipitate is formed. How would this affect the value of the Ksp for [Pb2+][Cl-] in solution? The Ksp increases. The Ksp decreases. The Ksp remains the same. none of the above.
The Ksp remains the same.
When [ ] are around an ion, what does it represent? It is an aqueous solution. The concentration of the ion is in moles/liter. The ion is reacting.
The concentration of the ion is in moles/liter.
Using a value of Ksp = 1.8 x 10-2 for the reaction PbCl2(s) Pb+2(aq) + 2Cl-(aq). If a solution has a current value of Keq of 1.2 x 10-2, which statement is true? Too much solid has dissolved. Additional precipitate is forming. The solution is unsaturated. The ions are now combining to reduce their concentrations.
The ions are now combining to reduce their concentrations.(I think, I said additional precipitate is forming the first time and it was wrong)
Ba(OH)2 Ba+2 + 2 OH- (dissolved in solution). Which will NOT happen to the equilibrium of this solution as H+ ions are added? H+ will combine with OH- to form water. The base will dissociate to form more OH-. The reaction will move to the right. The reaction will move to the left. The quantity of Ba(OH)2 will decrease.
The reaction will move to the left
Select all that apply. Values of Ksp greater than 1.0 infer: The solid phase is relatively insoluble. The solid phase is relatively soluble. The chemical reaction proceeds readily to the right. The chemical reaction proceeds readily to the left.
The solid phase is relatively soluble. The chemical reaction proceeds readily to the right.
Select the THREE answers that are correct concerning a saturated solution of PbCl2. PbCl2(s) Pb+2(aq) + 2Cl-(aq) The system is in equilibrium. The rate of dissolving is equal to the rate of recrystallization. The concentration of PbCl2 is greater than normal. The concentration of the products only is used to determine the Ksp.
The system is in equilibrium. The rate of dissolving is equal to the rate of recrystallization. The concentration of the products only is used to determine the Ksp.
Where do the OH- ions go as additional acid is added? They evaporate. They combine with excess H+ ions to form more water. They remain in the solution at the same concentration. They remain in the solution, but change concentration.
They combine with excess H+ ions to form more water.
A REDOX reaction is a process by which atoms change their ion charge. True or False
True
A chemical base may be defined as a compound which contributes hydroxide ions or increases the OH- concentration when dissolved in water. True or False
True
A large Ka favors the production of hydronium ions. True or False
True
A large Ka means a strong acid. True or False
True
A solution is a homogeneous mixture. True or False
True
A system is in equilibrium when the rate of the forward reaction is equal to the rate of the reverse reaction. True or False
True
Acids can be harmful to work with. True or False
True
Balanced equations illustrate Conservation of Mass. True or False
True
In a redox reaction, the oxidizing agent always undergoes reduction. True or False
True
Ions are charged atoms or groups of atoms. True or False
True
Ions can consist of more than one atom. True or False
True
Polar substances will usually dissolve in polar solvents. True or False
True
Precipitation occurs when the product of the ion concentrations exceeds the Ksp. True or False
True
Regarding the table of oxidation potentials, a reactant on the list can oxidize any agent above it and reduce any agent below it. True or False
True
The concentration of the particles in the solid phase always remains the same regardless of how much quantity is present. True or False
True
The concentration of the solid phase always remains the same, regardless of how much quantity is present. True or False
True
The degree of sour taste is due to the acid in the food. True or False
True
The equivalence point occurs when [H+] = [OH-]. True or False
True
The greater the amount of H+ released, the stronger the acid. True or False
True
Titration is a process of reacting an acid with a base until an equivalence point is reached. True or False
True
When a base is added to water, the [H+] is reduced. True or False
True
What relationship seems to be true? When ionic character increases, electrical conductivity decreases. When ionic character decreases, electrical conductivity decreases. When ionic character decreases, electrical conductivity increases. When ionic character increases, electrical conductivity stays the same.
When ionic character decreases, electrical conductivity decreases.
Which expression is the correct equilibrium for the reaction aA + bB cC + dD? [C]^c[d]^D/a[A][b]B [A]^a[B]^b/[C]^c[D]^d [C]^c[D]^d/[A]^a[B]^b C[C]d[D]/a[A]b[B}
[C]^c[D]^d/[A]^a[B]^b
Which is the strongest base? [H+] = 10 -9 [H+] = 10 -11 [H+] = 10 -10 [H+] = 10 -12
[H+] = 10 -12
The Ksp expression for the system PbCl2(s) Pb+2(aq) + 2 Cl-(aq) is: [PbC12][Pb+2][2Cl-] [Pb+2][Cl-]2 [Pb+2][2Cl-]2 [PbCl2][Pb+2][Cl-]2 [Pb+2][2Cl-]2[PbCl2]
[Pb+2][Cl-]2
An acid is: a proton acceptor any substance that reacts to keep blue litmus blue any compound containing hydrogen a proton donor a compound having hydrogen as a cation and oxygen as an anion.
a proton donor
A saturated solution occurs when _____. a solution can dissolve no more solute in a given volume a solution can dissolve no more solute at a given pressure a solution can dissolve no more solute at a given temperature a solution can dissolve no more solute in a given phase
a solution can dissolve no more solute at a given temperature
A substance that produces hydrogen ions in solution; alternatively, a proton donor
acid
Complete the word equation for making a salt. Metal + → salt + hydrogen
acid
Complete the word equation for making a salt. Metal oxide + ______ → salt + water
acid
The pH of a solution can be determined with an instrument called a pH meter. The following data was collected with the use of a pH meter. Study and analyze it carefully. Solution pH reading Acid or Base? 0.1 M HCl 0.1 0.01 M HCl 1.1 0.1 M Na2CO3 10.3 0.1 M NaOH 13.0 0.1M HC2H3O2 2.8 0.01 M HC2H3O2 3.6 0.1 M NaHCO3 8.2
acid acid base base acid acid base
What is the general word equation for salt formation by neutralization? _________ + __________ → salt + H2O acid + base metal + base metal + acid nonmetal + acid
acid + base
What is the general word equation for salt formation by neutralization? metal + nonmetal acid + metal base + nonmetal acid + base
acid + base
Solute will continue to dissolve in a solvent until: an equilibrium is reached it is all dissolved there is as much dissolved as there is not dissolved
an equilibrium is reached
What is a salt? A compound formed from a(n) _____ from an acid and a(n) _______ from a base.
anion cation
Which word would not make this statement true? "The first step in the two-step process of making a solution is the breakdown of the solute source into ____________." atoms molecules ions atomic particles
atomic particles
A substance that produces hydroxide ions in solution; alternatively, a proton acceptor
base
Balance the reactions which form ions. Choose "blank" if no other coefficient is needed. Writing the symbol implies "1." PbI2 <=> __Pb+2 + __I+1
blank 2
Balance the reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coefficient is "1." __Pb(NO₃)₂ + __NaI → __PbI₂ + __NaNO₃
blank 2 blank 2
Balance the reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coefficient is "1." 2AgNO₃ + __MgCl₂ <=> 2AgCl + __Mg(NO₃)₂
blank blank
The correct litmus test for an acid is: yellow litmus turns blue blue litmus turns red red litmus turns yellow red litmus turns blue
blue litmus turns red
A dissolved solute: consists of submicroscopic atoms or molecules consists of microscopic particles consists of small particles which settle out of the solution none of the above
consists of submicroscopic atoms or molecules
Consider the Zn(s) + Cu+2(aq) ---> Zn+2(aq) + Cu(s) system. Which element was the electron acceptor?
copper
As an acid is added to neutral water the [OH-] will .
decrease
Look carefully at Kw expression. If the [H+] changed from [1 x 10-7] to [1 x 10-4], the [OH-] will:
decrease
The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of lead acetate, Pb(C2H3O2)2. When the test tube was shaken, a white precipitate of PbCl2 formed. How will this affect the concentration of Cl-? increase it decrease it remain constant
decrease it(I think, I said increase it the first time and it was wrong)
The process of intermingling of the ions (molecules) of one substance into another is called: equilibrium diffusion ionization dissociation
diffusion
Electrolytes are defined as those compounds which: have covalent bonding produce less lowering at the freezing point than do compounds like sugar have only ionic bonds dissolve in a solvent such as water to produce a solution which conducts electric current easily
dissolve in a solvent such as water to produce a solution which conducts electric current easily
From the figure of the electrochemical cell, what is producing the current in the wire connecting the electrodes? electrons moving from Zn to Cu cations moving to the anode anions moving to the cathode voltage (E0) applied to the circuit
electrons moving from Zn to Cu
Reduction is a reaction which results in a _____ in electrons and a(n) ___________ in positive charge of the atom or ion.
gain decrease
M + e- ---> M-1 Has M lost or gained an electron?
gained
What caused the different pH values for the test solutions? Each solution has a different concentration of _____ ions.
hydrogen
Generally, you may expect ionization to be greater: in dilute solutions in 1 M solutions in high concentration solutions none of these
in dilute solutions
As an acid is added to neutral water the H+ will .
increase
Data Table 7 Compound Temperature, °C Ksp AgCl 4.7 0.21 x 10-10 AgCl 9.7 0.37 x 10-10 AgCl 25 1.56 x 10-10 AgCl 50 13.2 x 10-10 AgCl 100 215 x 10-10 From the data table, as the temperature increases, the Ksp value will __________ . Does the change in solubility data mean that the AgCl becomes more or less soluble at higher temperature?
increase more
The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of lead acetate, Pb(C2H3O2)2. When the test tube was shaken, a white precipitate of PbCl2 formed. You have ________ the Pb+2 concentration by adding lead acetate.
increased
As the concentration of a given salt solution increases, the conductivity of the solution: increases no way to predict remains the same increases then decreases decreases
increases
Electricity is conducted through a solution containing an electrolyte by: ions molecules water atoms neutrons
ions
Oxidation is a reaction in which there is a _____ of electrons which results in a(n) __________ in positive charge of the atom or ion.
loss increase
M ---> M+ + e- Has M lost or gained an electron?
lost
Choose the THREE items that are characteristic of a strong base. few OH- ions many OH- ions few H+ ions many H+ ions large Kb and small Ka large Ka and small Kb Kb = Ka
many OH- ions few H+ ions large Kb and small Ka
Complete the word equation for making a salt. _________ + __________ → salt metal + hydrogen nonmetal + water metal + nonmetal water + hydrogen
metal + nonmetal
Molarity is defined as ______ per liter.
moles
AlCl3 + Na NaCl + Al Did Cl change oxidation number? yes no
no
HBr + H₂SO₄ SO₂ + Br₂ + H₂O Did H change oxidation number?
no
HBr + H₂SO₄ SO₂ + Br₂ + H₂O Did O change oxidation number?
no
Determine the oxidizing and reducing agents after answering the following questions. First, determine the oxidation number of every atom on both sides of the arrow. KMnO4 + H2S + HCl KCl + MnCl2 + H2O + S8 Did Cl change oxidation number? Did Oxygen change oxidation number? Did H change oxidation number? Did Mn change oxidation number? Did S change oxidation number? oxidizing agent = reducing agent =
no yes yes no yes O S (one or more of these is wrong)
One mole of the acid HCl requires how many moles of OH- for neutralization? ____moles
not 0.5 maybe 3 `
If you made up a solution of NaOH by adding 0.010 mole of solid NaOH to 1.0 liter of distilled water, what would be the pH of the solution? pH =
not 2 maybe 12
M ---> M+ + e- The reaction represents .
oxidation
Use the E0 values of the following elements: Zn, Cu, Pb, and Al. Copper will ______ Pb.
oxidize
M ---> M+ + e- Is M oxidized or reduced?
oxidized
Cu + H₂O → CuO + H₂ This equation shows that Cu is . This equation shows that H₂ is .
oxidized reduced
Using the relative Eo values, determine which of the following reactions are electrically possible. Cu2+(aq) + Zn(s) Zn2+(aq) + Cu(s) This equation shows that Cu is . This equation shows that Zn is . Can this redox reaction take place?
oxidized reduced no (one or more of these could be wrong)
Consider the Zn(s) + Cu+2(aq) ---> Zn+2(aq) + Cu(s) system. The electron acceptor is the agent.
oxidizing
M + e- ---> M-1 Is M an oxidizing or reducing agent?
oxidizing
Which acid is the strongest? pH = 0.5 pH = 2.0 pH = 3.5 pH = 5
pH = 0.5
What relationship do you find between the pH number and the power of 10 used to express the [H+]? pH = exponent of concentration values pH = reciprocal of the H+ concentration pH = the negative of the exponent of concentration pH = the H+ concentration
pH = the negative of the exponent of concentration
Dissolving is a _______ change.
physical
When the Ka value is very large, the ________ are favored over the _________.
products reactants
Equilibrium is established in a reversible reaction when: the [product] = [reactants] rate of reaction of products = rate of reaction of reactants all the reactants dissolve or dissociate product is no longer produced
rate of reaction of products = rate of reaction of reactants
Use the E0 values of the following elements: Zn, Cu, Pb, and Al. Zinc will ______ Pb.
reduce
M + e- ---> M-1 Is M oxidized or reduced?
reduced
Using the relative E0 values, determine which of the following reactions are electrically possible. 2FeCl3 2FeCl2 + Cl2; (Fe+ 3 changes to Fe+ 2 Cl- changes to Cl0) This equation shows that Fe+ 3 is . This equation shows that Cl- is . Based on the values of E0, will this redox reaction take place?
reduced oxidized no
Consider the Zn(s) + Cu+2(aq) ---> Zn+2(aq) + Cu(s) system. The electron donor is the agent.
reducing
M ---> M+ + e- Is M an oxidizing or reducing agent?
reducing
Select all that apply. All the reactants listed in the table of oxidation potentials are: oxidizing agents reducing agents oxidized by the reaction reduced by the reaction
reducing agents oxidized by the reaction
M + e- ---> M-1 This reaction represents .
reduction
A characteristic of acids is that they react with metals to: form non-metals release water release hydrogen gas produce bases
release hydrogen gas
If a crystal of KNO3 is added to a saturated water solution of KNO3 at 20°C, the added crystal will dissolve quickly. cause the solution to all crystallize. remain apparently unchanged. lower the freezing point of the solution.
remain apparently unchanged
The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of NaCl. A white precipitate of PbCl2 formed. What happens to the value of Ksp when NaCl was added? increase it decrease it remain constant
remain constant
The Kw of water: varies with pH is only applicable to neutral water remains constant regardless of the pH ranges between 1.0 and 10-14
remains constant regardless of the pH
The ion product of water: varies with pH is only applicable to neutral water remains constant regardless of the pH ranges between 1.0 and 10-14
remains constant regardless of the pH
One mole of ANY element contains the: same mass as one mole of any other element same number of atoms as one mole of any other element same gram-formula-weight as one mole of any other element both the first and second choices
same number of atoms as one mole of any other element
How does the polarity of the solute affect how well a solvent will dissolve? it allows the solvent to absorb more heat it has no effect the freezing point of the solvent will increase the solute will ionize more completely within the solvent similar polarity makes the solvent more likely to dissolve
similar polarity makes the solvent more likely to dissolve
Which of the following choices is not a factor in the amount of electrical conductivity of a solution? concentration ionic character size of container potential number of ions type of solvent
size of container
Our body solution tests at a pH of about 6.8. This pH is: strongly acidic slightly basic strongly basic neutral slightly acidic
slightly acidic
The component which dissolves in a solution is called the .
solute
The substance that is dissolving is called the_______ .
solute
The liquid component that makes up the largest part of a solution is called the _______, and the substance that is dissolved is called the ________.
solvent solute
A mole or fraction of a mole represents a _________ number of atoms or molecules.
specific
Select all of the following choices that would be a nonconducting substance or solution. sucrose C12H22O11 (dissolved in water) CaCl2 (dissolved in water) BeF2 (dissolved in water) BaF2 (dissolved in water) distilled water
sucrose C12H22O11 (dissolved in water) distilled water
The method used to determine the equivalence point of an acid-base solution is called: neutralization precipitation titration hydration
titration
nonmetallic oxide + base → salt + ______
water
A neutralization reaction between an acid and a base will yield: a conjugate acid and a base water and a weak acid water and a weak base water and a salt
water and a salt
Select all that apply. When is Ksp determined for a system? at any time that the solid and liquid phases are both present only after all solid has been dissolved when equilibrium is established when the two phase system is saturated
when equilibrium is established when the two phase system is saturated
Select all that apply. At STP conditions, 0.25 moles of CO2(g), H2(g), NH3(g): will contain the same number of molecules will contain the same number of atoms will occupy the same volume will have the same g.f.w.
will contain the same number of molecules will occupy the same volume
HBr + H₂SO₄ SO₂ + Br₂ + H₂O Did Br change oxidation number?
yes
HBr + H₂SO₄ SO₂ + Br₂ + H₂O Did S change oxidation number?
yes
Reaction E0 Zn → 2e- + Zn2+ 0.76 2F- → 2e- + F2 -2.87 F2 + Zn → ZnF2 Will this redox reaction take place? yes no
yes
Consider the Zn(s) + Cu+2(aq) ---> Zn+2(aq) + Cu(s) system. Which element must be more willing to give up electrons?
zinc
Consider the Zn(s) + Cu+2(aq) ---> Zn+2(aq) + Cu(s) system. Which element was the electron donor?
zinc
Balance this chemical equation. Choose "blank" for the box if no other coefficient is needed. Writing the symbol implies "1." __HCl + __Zn → __ZnCl2 + __H2
2 blank blank blank
CHEMIST'S TOOLBOX
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ELECTRICAL NATURE OF SOLUTIONS
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SOLUBILITY
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SOLUTION CONCENTRATION: MOLARITY
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If water is added to 50 ml of a 0.04 M solution so that it fills a 200 ml beaker, what is the final concentration? __M
0.01
10 mL diluted to 100 mL 0.50 M NaCl in 10.0 mL -> +90 mL H2O -> __in 100.0 mL If 10.0 mL of the solution on the right are withdrawn from the 100 mL beaker and diluted again in a similar manner, what is the new concentration?
0.01(not 100% sure, I put 0.050 the first time and it was wrong)
10 mL diluted to 100 mL 0.50 M NaCl in 10.0 mL -> +90 mL H2O -> __in 100.0 mL When 10.0 mL of the 0.50 M solution is diluted to 100 mL as shown, what is the new concentration?
0.050
Calculate the molarity of the solution. 6.02 x 1022 molecules of HCl (molecular weight = 36.5 g/mole) in 2.0 liters of water __ M
0.050
The molecular weight of NaCl is 58.44 grams/mole. If you had a 1.0 molar solution (1.0 M), you would have to put 58.44 g of salt in 1.0 liter of solution. How many moles of NaCl would you have in 100 mL of this solution?
0.10
Calculate the molarity of the solution to 3 digits. 100. g of C12H22O11 (molecular weight = 342.28 g/mole) in 1.15 liters of solvent __ M
0.254
10 mL diluted to 100 mL 0.50 M NaCl in 10.0 mL -> +90 mL H2O -> __in 100.0 mL The molecular weight of NaCl is 58.44 grams/mole. How many grams of NaCl are in the beaker on the right? Round answer to 2 significant figures. __ g
0.29
Be sure to use proper significant figures. The molecular weight of NaCl is 58.44 grams/mole. With a 0.50 M solution: How many grams of NaCl would there be in 10.0 mL of solution?
0.29
Match the atoms which might substitute for one another. 1. Si 2. K 3. Nb 4. Cu 5. P 6. Mg
1-C 2-Na 3-V 4-Ag 5-As 6-Ca
1. A mixture that does not have a uniform composition and the individual components remain distinct. 2. A mixture that does have a uniform composition throughout and is always in the same state. 3. A substance that will not dissolve in a solvent. 4. A homogeneous mixture 5. A molecule with no internal charge variation due to bonding. 6. a molecule with an uneven distribution of charge due to unequal sharing of electrons during bonding 7. A solution which has dissolved as much solute as it can at a particular temperature. 8. A solution which is still able to dissolve solute.
1-heterogeneous 2-homogeneous 3-insoluble 4-solution 5-nonpolar 6-polar 7-saturated 8-unsaturated
Calculate the molarity of the solution. 29 g of NaCl in 0.25 liters of water (The molecular weight of NaCl is 58.44 g/mole.) __ M
2.0
Be sure to use proper significant figures. The molecular weight of NaCl is 58.44 grams/mole. To prepare a 0.50 M solution: You would need to have ___ grams of NaCl in 1,000 mL of water.
29.22(it says this is wrong, but after looking into it I don't understand how)
Determine the number of ions produced in the dissociation of the compound listed. CaCl2
3
Determine the number of ions produced in the dissociation of the compound listed. MgBr₂
3
N2 + 3H2 2NH3 How many molecules of H2 are represented in the reaction? How many nitrogen atoms are represented in the reactants? How many moles of NH3 are formed?
3 2 2
Balance this chemical equation. Choose "blank" for the box if no other coefficient is needed. Writing the symbol implies "1." __NH4OH + __AlCl3 → __Al(OH)3 + __NH4Cl
3 blank blank 3
Determine the number of ions produced in the dissociation of the compound listed. AlF3
4
Balance this chemical equation. Choose "blank" for the box if no other coefficient is needed. Writing the symbol implies "1." __Al + __O2 → __Al2O3
4 3 2
3Fe + 4H2O Fe3O4 + 4H2 How many molecules of H2 are produced? How many oxygen atoms are found in the products? How many moles of Fe3O4 are formed? What is the ratio of the number of moles of Fe atoms to the moles of H2O molecules? How many hydrogen atoms are found in the reactants?
4 4 1 3/4 8
Which of the following statements is NOT correct? 0.20 mole of O2 = 6.4 g 0.75 mole of H2CO3 = 47 g 3.42 moles CO = 95.8 g 4.1 moles Li2O = 94 g
4.1 moles Li2O = 94 g
Determine the number of ions produced in the dissociation of the compound listed. Al2S3
5
The molecular weight of NaCl is 58.44 grams/mole. If you had a 1.0 molar solution (1.0 M), you would have to put 58.44 g of salt in 1.0 liter of solution. 100 mL of this solution would have ___ grams of NaCl.
5.8
0.2 M in 10 mL--->0.04 M in ___mL What would be the final volume of the new solution if the 0.2 M solution on the left were diluted to 0.04 M? __ mL
50
What is the molecular weight of one mole of H2CO3?
62.026 g/mole
Which graph best depicts the relationship between concentration and dissociation?
A graph with a negative slope
Select the ion. NO2 H2SO4 Al+3
Al+3
Select all that apply. The requirements for one type of atom to substitute for another in a solid solution are: All substitutions must be limited to the same element. An atom must be identical in size. An atom must be similar in size. The substituting atom must be from the same period. The substituting atom must be from the same group.
An atom must be similar in size. The substituting atom must be from the same group.
Only metal alloys form solid solutions. True or False
False
Solid solutions are only formed with metals. True or False
False
Solutions are limited to homogeneous mixtures of liquids. True or False
False
The physical properties of a solution are not affected by the concentration of the components. True or False
False
The reduction in the freezing point of a solution is inversely proportional to molal concentration. True or False
False
The vapor pressure of water is not affected by the amount of salt added. True or False
False
________ molecules are likely to dissolve in nonpolar solvents.
Nonpolar
0.25 mole of O2 will contain the same number of molecules as 0.25 mole of NH3. True or False
True
2KClO3 2KCl + 3O2 In the reaction represented by this equation, two moles of KClO3 decompose to form 5 moles of product. True or False
True
2KClO3 2KCl + 3O2 In this equation, the number of molecules of product is greater than the number of molecules of reactant. True or False
True
8Fe + S8 8FeS In the reaction represented by this equation, nine moles of reactants form 8 mole of product. True or False
True
A homogeneous portion of a mixture that is characterized by uniform properties and capable of being separated by mechanical means is called a phase. True or False
True
A liquid solution can be made from solid, liquid, or gas solute. True or False
True
All gaseous mixtures are solutions. True or False
True
Alloys are examples of solid solutions. True or False
True
Crystallization is a good way to purify solids. True or False
True
Equilibrium systems exist throughout nature. True or False
True
Salt acts as an antifreeze. True or False
True
Solutions are a mixture of 2 or more compounds. True or False
True
The degree to which various compounds will dissociate in solution varies greatly. True or False
True
The orderly geometric arrangement of atoms is called a crystalline solid. True or False
True
The following are properties of compounds _____. vapor pressure density boiling point all of the above
all of the above
Select all that apply. The solvent is usually referred to as the component of a solution which is present: as one liter as the larger quantity as the liquid which dissolves a solid as the smaller quantity
as the larger quantity as the liquid which dissolves a solid
Define ionize: the process of becoming an ion a polar covalent molecule forming ions both of the above none of the above
both of the above
Consider again the solution made by diluting 10.0 mL of the 0.50 M NaCl by adding distilled water until 100 mL of solution are produced. Has the concentration of the diluted salt solution increased, decreased, or remained constant? increased decreased remained constant
decreased
The physical properties of a solution are ________ the properties of its individual components.
different from
Solutions which can conduct electricity are called: homogeneous electrolytes polar metallytes
electrolytes
A mole of the element U (uranium) and a mole of CO2: have the same molecular weight have the same atomic mass have an equal number of particles have an equal number of atoms
have an equal number of particles
A mixture which contains more than one phase is called
heterogeneous
Look carefully at Data Table 1. Do ionic or covalent substances tend to produce more ions in solution? ionic covalent
ionic
Look carefully at Data Table 1. Do solutions and liquids of ionic or covalent character tend to conduct electricity best? ionic covalent
ionic
The mass of one mole of any substance: is equal to 6.02 x 1023 g is equal to the sum of the atomic masses of every atom in the formula is the same for all elements but not molecules is the same for all elements and molecules
is equal to the sum of the atomic masses of every atom in the formula
An element or compound which occurs naturally in the earth is a .
mineral
Concerning the 10.0 mL of 0.50 M NaCl diluted to 100 mL of solution: When a solution is diluted, does the dilution change the number of grams dissolved? yes no
no
Concerning the 10.0 mL of 0.50 M NaCl to 100 mL of solution: When a solution is diluted, does it change the number of moles dissolved? yes no
no
Is it likely that an atom of Te would substitute for an atom of O in a solid compound? yes no indeterminate
no
Polar molecules are unlikely to dissolve in _______ solvents.
nonpolar
The purging of impurities from a compound by crystallization: occurs when the compound is put under great pressure occurs when the compound is vaporized occurs after the liquid melt cools back to a solid occurs after condensation from the vapor phase
occurs after the liquid melt cools back to a solid
Polar molecules will usually dissolve in ______ solvents.
polar
Look carefully at Data Table 1. Do covalent substances ionize while dissolving? yes no sometimes
sometimes(definitely not no)
Now dilute 10.0 mL of the 0.50 M NaCl by adding distilled water until 100 mL of solution are produced. Do the 100 mL of diluted NaCl have more, less, or the same quantity of NaCl as the original 10.0 mL of 0.50 M NaCl? more less the same
the same
Which characteristic is least likely to be used for predicting percent dissociation of a solid in a liquid? chemical properties of solute the type and polarity of the solvent the temperature concentration of solute
the temperature
Select all that apply. At STP conditions, 0.25 mole of CO2(g), H2(g), and NH3(g): will contain the same number of molecules will contain a different number of molecules will occupy the same volume will have the same molecular weight
will contain the same number of molecules will occupy the same volume
Concerning the 10.0 mL of 0.50 M NaCl to 100 mL of solution: Does dilution change the concentration? yes no
yes
