Question

3 of 15
Which of the following statements is true regarding the dissolution of a salt in a solvent?

A. An equilibrium constant can be described that is the product of the concentrations of the ions to the power of their coefficient.
B. The reaction does not have an equilibrium constant since all dissolution reactions are nonreversible.
C. Precipitates are included in the equilibrium constant.
D. The number of each ion does not affect the equilibrium constant.

Answer 1

@sweetburger

Answer 2

it's b

Answer 3

It is not b.

Answer 4

oops

Answer 5

All dissociation reactions will have Equilibrium constants in the form of Ksp values.

Answer 6

Besides that I believe the correct answer would be A. As B,C, and D are all incorrect. And A does make sense mathematically.

Answer 7

Thank you. This one?

Answer 8

Products over reactants and H2O is a liquid so it drops out

Answer 9

Hmm these answers seem off.

Answer 10

I'm almost completely sure it should be [H3O+][CH3COO-]/[CH3COOH]

Answer 11

Oh its C. I completely missed it XD.

Answer 12

I think the answer is B, because the Kc expression must apply for aqueous substances only and H2O is liquid.
Solids and liquids should be out.

Answer 13

Thank you it was C.

________equilibrium is a type of ________equilibrium which occurs when a reaction is ________.

A. Dynamic; chemical; irreversible
B. Dynamic; chemical; reversible
C. Chemical; dynamic; irreversible
D. Chemical; dynamic; reversible

Answer 14

I mean C.

Answer 15

It cannot be A or C. A dynamic equilibrium will always be reversible.

Answer 16

B

Answer 17

Im almost sure it should be D. As a chemical equilibrium would fall under the classification of a dynamic equilibirum.

Answer 18

lol
D

Answer 19

sorry
im multitasking

Answer 20

Yep, thanks it was D. This one?

Answer 21

C?

Answer 22

C looks good.

Answer 23

Which of the following choices is not a potential application of the solubility product constant?

A. Determine reactant concentrations that will allow a precipitate to form.
B. Determine ion concentrations that will prevent a precipitate from forming.
C. Determine ion concentrations that will allow a precipitate to form.
D. Use Ksp to find solubility.

Answer 24

Well you can use Ksp to find solubility so it cant be D.

Answer 25

I'm actually not to sure on this one. I'm trying to think through it, but not much is coming up.

Answer 26

Actually it cannot be C either as you can determine how much of a ion will cause a precipitate to form.

Answer 27

So it's either A or B?

Answer 28

Ya, I think so.

Answer 29

Which one is the most logical answer?

Answer 30

I'm leaning towards A after thinking through it, but I'm still not completely sure with this question.

Answer 31

It was A! :)

Answer 32

Haha, nice. :)

Answer 33

This one?

Answer 34

I think this is just a Ksp problem in disguise, but Im not completely sure. So im going to say that 1.5x10^-8=[x][x] and then take the square root of both sides and get that x=.000122. That is equivalent to saying that [Pb2+]=1.22x10^-4.

Answer 35

Thank you!

The solubility of a substance is the _____ amount of the substance that can dissolve to form a _____ in a given amount of a particular solvent at a specified temperature.

A. minimum; solution
B. minimum; precipitate
C. maximum; precipitate
D. maximum; stable solution

Answer 36

maximum amount to form a stable solution

Answer 37

thanks. how about this one?

Answer 38

No matter how insoluble we say a substance is something will always dissolve this even holds true for nonpolar substances being dissolved in polar substances and vice-versa. In this case the determined value of Ksp is so extremely small that we qualify it as insoluble.

Answer 39

So C.

Answer 40

What is the solubility product constant (Ksp)?

A. The equilibrium constant for the formation of any ionic compound
B. The equilibrium constant for the formation of a nearly insoluble ionic compound
C. The equilibrium constant for the dissolution of any ionic compound
D. The equilibrium constant for the dissolution of a nearly insoluble ionic compound

Answer 41

C.

Answer 42

It was D.

Answer 43

@sweetburger How about this one?

Answer 44

B. As CaCO4 Ksp is 2.4x10^-5 and PbSO4 Ksp is 1.7x10^-8 adn CaCO4 has the larger Ksp value meaning it will be more soluble.

Answer 45

Thank you.

Answer 46

Not so sure about this one. A or B maybe?

Answer 47

Yes, I believe it would be. Think about it like this the Keq value is Products/Reactants if there are more reactants than prodcuts and I am just using arbitrary number here you will see that 1/100 = .01 which is a much smaller value then for example 100/1= 100 if there were more products than reactants . So when there are far more reactants at equilbirum the Keq value will be far less than 1. So B should be the correct answer. As for this example the Keq values is 1x10^-3 which is far smaller than 1.

Answer 48

So A or B?

Answer 49

Im pretty sure B.

Answer 50

What does a dissolved salt look like?

A. The salt crystals are surrounded by water molecules.
B. The salt crystals separate into salt molecules in the water.
C. The ions in the salt are surrounded by water molecules.
D. The salt separates into ions that settle to the bottom.

Answer 51

This should be C. as the positive ions will be surrounded by polar negative Oxygens from H2O molecules and the negative ions will be surrounded by polar positive Hydrogens from the H2O molecules.

Answer 52

Question 15 of 15

What is solubility a measure of?

A. The energy needed for the solute to dissolve
B. The amount of solute that will dissolve
C. The type of solute that will dissolve
D. The rate at which the solute will dissolve

Answer 53

@rvc @Hoslos ???

Answer 54

D.

Answer 55

D

Answer 56

Ah it was B. Thanks though.

Answer 57

Yea Ksp has nothing to do with Kinetics

Answer 58

Thank you all so much for your help! I'm very thankful that you all helped me today! :)

@Hoslos :) @rvc :) @sweetburger :)

Answer 59

Np :) @vera_ewing sorry I wasnt here for the last question :/

Answer 60

No worries :)

Answer 61

All the best
@Hoslos @sweetburger thanks 4 helping me to help her

Answer 62

:)

Answer 63

I am glad.
It was a good team discussion here though.

Answer 64

Agreed @Hoslos . Well done to everybody :).