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CHAPTER 15 BASIC HOMEWORK:

INTRO. ACIDS

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Question 1

What conducts electricity in metals? (One word answer) 

Select from: electrons, ions, neutrons, nucleus, positrons, and protons

 

Explanation

BRO COME ON...negatively charged particle found in atoms

 

Question 2

What conducts electricity in solutions? (One word answer)



 

Explanation

General word for both cations and anions...aka please don't embarrass me you know this 

 

Question 3

Which of the following statements about ionic compounds is FALSE?


Select one:


Correct


 

Explanation

 Ill let this one slide if you didn't know it, but come on can solid salt conduct electricity there answer is NO because the ions are not free to move around.

 

Question 4

Classify the following compounds as strong electrolyte, weak electrolyte, or non-electrolyte. Write strong, weak, or non, respectively in the space for the answer.

KCl(s)

Electrolytes defined

Qualitative electrolyte rules


 

Explanation

Does this completely dissociate?? YES IT DOES why because of the solubility rules that you should have memorized last semester

 

Question 5

CaCl2(s)

 

Explanation

 

Question 6

PbCl2(s)


 

 


 

Question 7


O2(g)

 


 

Question 8


HCl(g)

 
 

Question 9

Acetic acid (CH3COOH)

 



 

Question 10

What is the molarity of 0.77 mol of NaCl in enough water to make 5.0 L of solution?

Definition and examples of Molarity

 

Correct

 

Explanation

 0.77 mol NaCl / 5 L = 0.154 [NaCl]

 

Question 11


What is the molarity of the Al3+ ions when 0.42 mol of aluminum nitrate, Al(NO3)3, is dissolved in enough water to make 4.0 L of solution?

Correct

 

Explanation

 Al(NO3)3 is a strong electrolyte. ( 1 Mol of Aluminum ions per mol)


0.42/ 4 * 1 = 0.105

 

Question 12


What is the molarity of the nitrate ions when 0.47 mol of barium nitrate, Ba(NO3)2, is dissolved in enough water to make 3.0 L of solution?

Correct    

 

Explanation

 Ba(NO3)2 is a strong electrolyte.( 2 Mols of Nitrate ions per mol)


0.47/ 3 * 2  = 0.313

 

Question 13

Calculate the molarity of calcium hydroxide that has been prepared by dissolving 2.87 g of calcium hydroxide in water and diluting the solution to a final volume of 4.00 L.

Example molarity calculation

Correct

 

Explanation

 2.87 g Ca(OH)2 / 74.069  g/mol    =    0.0387  mol


0.0387 mol/ 4 L = 0.009696

 

Question 14

Calculate the molarity of the hydroxide ions in a solution that has been prepared by dissolving 27.5 g of barium hydroxide (Ba(OH)2) in water and diluting the solution to a final volume of 5.00 L. (M.W's: Ba 137.3 g/mol., O 16.0 g/mol, and H 1.0 g/mol)

Correct

 

Explanation

 Remember there are 2 moles of hydroxide for each mole of barium hydroxide.

 

Question 15

What is the molarity of the H+ ions in 0.50 M HCl?

Examples of acids and bases

Select one:



Correct

 

Explanation

 STRONG ACID FULLY DISSOCIATES

 

Question 16

What is the molarity of the H+ ions in 0.50 M acetic acid, CH3COOH?

Select one:


Correct

 

Explanation

 NOT STRONG ACID DOESNT FULLY DISSOCIATE

 

Question 17

What is the molarity of the H+ ions in 0.50 M hydrofluoric acid, HF?

Select one:


Correct

 

 

Explanation

 HF is a weak acid WHAT DOES THAT MEAN it will not fully dissociate aka very very little of it 

 

Question 18


What is the molarity of the H+ ions in 0.40 M nitric acid, HNO3?

Select one:




Correct

 

Explanation

 STROMG ACIDS FULLY DISSOCIATE

 

Question 19

What is the molarity of the NO3- ions in 0.40 M nitric acid, HNO3?

Select one:




  Correct

 

Explanation

 0.40 *1 = 0.40

 

Question 20

What is the molarity of the OH- ions in 0.040 M sodium hydroxide, NaOH?

Select one:



Correct

 

Explanation

 NaOH is a strong base and will therefore fully disscoaite 

 

Question 21

What is the molarity of the OH- ions in 0.040 M ammonia, NH3?

Select one:


Correct


 

Explanation

 NH3 is a weak base, meaning that it will not fully dissociate and have very very little hydroxide ions

 

Question 22

What is the molarity of the OH- ions in 0.040 M barium hydroxide, Ba(OH)2?

Assume the barium hydroxide is fully dissociated into ions in the dilute solution.


Select one:


 


Correct

 

Explanation

0.040*2 = 0.08

 

Question 23

Match correct answers.

H+ is more accurately represented by adding a water molecule, that is, as H3O+.

[H3O+] = [OH-] Correct

[H3O+] > [OH-] Correct

[H3O+] < [OH-]Correct

 

 

 

Question 24

Check those statements which are true.

Concentration of acids and bases

Select one or more:
 Correct
 Correct
 Correct

 

Explanation

 Use the equation -log[H+]=pH  

as well as  -log[H+] -log[OH-] = 14

 

Question 25

Calculate the hydroxide ion concentration, [OH-], in 0.014 M HBr.

Acid/base calculation

Correct

 

Explanation

 -log[0.014]+-log[OH-]=14

OH-= 7.14e-13

 

Question 26

Calculate the hydroxide ion concentration, [OH-], in 1.95 M HNO3.


Correct

 

Explanation

 -log[1.95]+-log[OH-]=14

OH-= 5.128e-15

 

Question 27

Calculate the hydrogen ion concentration, [H+], in 0.00486 M NaOH. 


Correct

 

Explanation

 pH+pOH=14

-log[OH-]=pOH

-log[0.00486 M]=pOH

-log[H+] -log[0.00486 M]=14

H+=2.0576e-12

 

Question 28

Calculate the hydrogen ion concentration, [H+], in 0.00688 M Ba(OH)2. Careful! 


Correct

 

Explanation

 pH+pOH=14

-log[OH-]=pOH

-log[2*0.00688]=pOH

-log[H+] -log[2*0.00688]=14

H+=7.267e-13

 

Question 29

The autodissociation of water to H+ and OH- is endothermic. At a higher temperature more of the water molecules have sufficient energy to dissociate. So, Kw is greater.

At 25oC, Kw = 1.0 x 10-14. (standard Kw)
At 65oC, Kw = 1.0 x 10-13.

Calculate the hydrogen ion concentration, [H+], in 0.0636 M LiOH at 65oC.


Correct

 

Explanation

 Kw= 1e-13 = [0.0636][H+]

[H+]=1.57e-12

 

Question 30

What is the pH of a solution where the [H+] =8.28 x 10-12 M?

REPORT pH TO 2 DECIMAL PLACES.

pH calculation

Correct

 

Explanation

 pH=-log[8.28e-12]

pH=11.08

 

Question 31

Which of the following statements are true?

pH and acidity

Select one or more:
Correct 
 Correct


Correct

Correct

 

 

 

Question 32

What is the pH of a solution where the [H+] =7.41 x 10-12 M?

REPORT pH TO 2 DECIMAL PLACES.


Correct

 

Explanation

 pH=-log[7.41e-12]

pH=11.13

 

Question 33

What is the pH of a solution where the [OH- ] =5.73 x 10-1 M?

REPORT pH TO 2 DECIMAL PLACES.

Finding pH from [OH- ]

Correct

 

Explanation

 pH+pOH=14

pH-log[5.73e-1]=14

pH=13.76

 

Question 34

What is the [H+] if the pH of a solution is 9.88?

Correct

 

Explanation

 9.88=-log[H+]

10^-9.88=10^log[H+]

1.318e-10=[H+]

 

Question 35

What is the [H+] if the pH of a solution is 2.44?

Correct

 

Explanation

 2.44 = - log[H+]

H+ = 0.00363