CHEMISTRY-EQUILIBRIUM SYSTEMS
Which expression defines molarity? #moles/Liter(solvent) #moles/#mole solution #moles/Liter solution none of these
#moles/Liter solution
SOLUTIONS
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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 __in 100.0 mL If 10.0 mL of the solution on the right are withdrawn from the 100 mL beaker and diluted again in a similar manner, what is the new concentration?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
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
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
What is the atomic mass of one mole of H?
1.008 g/mole
What is the atomic mass of one mole of O?
16.00 g/mole
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
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 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
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
Calculate the molarity of the solution. 4.32 x 102 moles of CH3COOH in 20.0 liters of water __M
21.6
What is the atomic mass of one mole of Na?
22.99 g/mole
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.
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
A high percent of dissociation is always expected to yield a high conductivity. True or False
False
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
Select the ion. Mg H+ HC2H3O2
H+
Select the ion. HCl H2O H3O+1
H3O+1
________ molecules are likely to dissolve in nonpolar solvents.
Nonpolar
Select the ion. Cu PO4-3 SO2
PO4-3
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
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
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
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
The component which dissolves in a solution is called the .
solute
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
