QuestionIn which of the following aqueous solutions would you expect AgBr to have the highest solubility? A) 0.15 M KBr B) 0.10 M LiBr C) pure water D) $0.10 \mathrm{M} \mathrm{AgNO}_{3}$ E) 0.20 M NaBr

Studdy Solution

STEP 1

What is this asking? Which solution lets silver bromide (AgBr) dissolve the most? Watch out! Don't forget that common ions reduce solubility!

STEP 2

1. Identify the common ion effect
2. Compare solubility in different solutions
3. Determine the highest solubility

STEP 3

Alright, let's break it down!
AgBr dissolves in water to form silver ions ( $\text{Ag}^+$ ) and bromide ions ( $\text{Br}^-$ ).
When you have other sources of these ions in the solution, it makes it harder for AgBr to dissolve.
This is called the common ion effect.
So, if a solution already has $\text{Br}^-$ or $\text{Ag}^+$ , AgBr won't dissolve as much.

STEP 4

Let's look at each option:
- Option A: $0.15 \, \text{M} \, \text{KBr}$ has $\text{Br}^-$ ions.
More $\text{Br}^-$ means less AgBr dissolves. - Option B: $0.10 \, \text{M} \, \text{LiBr}$ also has $\text{Br}^-$ ions.
Again, less solubility for AgBr. - Option C: Pure water has no extra ions, so nothing to stop AgBr from dissolving! - Option D: $0.10 \, \text{M} \, \text{AgNO}_3$ has $\text{Ag}^+$ ions.
More $\text{Ag}^+$ means less AgBr dissolves. - Option E: $0.20 \, \text{M} \, \text{NaBr}$ has $\text{Br}^-$ ions.
Even more $\text{Br}^-$ means even less solubility for AgBr.

STEP 5

Alright, so we know that the more common ions there are, the less AgBr dissolves.
Pure water doesn't have any of these ions, so AgBr can dissolve the most there!

STEP 6

The solution where AgBr has the highest solubility is C) pure water.

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QuestionIn which of the following aqueous solutions would you expect AgBr to have the highest solubility? A) 0.15 M KBr B) 0.10 M LiBr C) pure water D) $0.10 \mathrm{M} \mathrm{AgNO}_{3}$ E) 0.20 M NaBr

Studdy Solution

STEP 1

What is this asking? Which solution lets silver bromide (AgBr) dissolve the most? Watch out! Don't forget that common ions reduce solubility!

STEP 2

1. Identify the common ion effect
2. Compare solubility in different solutions
3. Determine the highest solubility

STEP 3

STEP 4

STEP 5

Alright, so we know that the more common ions there are, the less AgBr dissolves.
Pure water doesn't have any of these ions, so AgBr can dissolve the most there!

STEP 6

The solution where AgBr has the highest solubility is C) pure water.

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QuestionIn which of the following aqueous solutions would you expect AgBr to have the highest solubility? A) 0.15 M KBr B) 0.10 M LiBr C) pure water D) 0.10MAgNO30.10 \mathrm{M} \mathrm{AgNO}_{3}0.10MAgNO3​ E) 0.20 M NaBr

Studdy Solution

STEP 1

What is this asking? Which solution lets silver bromide (AgBr) dissolve the most? Watch out! Don't forget that common ions reduce solubility!

STEP 2

1. Identify the common ion effect2. Compare solubility in different solutions3. Determine the highest solubility

STEP 3

STEP 4

STEP 5

Alright, so we know that the more common ions there are, the less AgBr dissolves.Pure water doesn't have any of these ions, so AgBr can dissolve the most there!

STEP 6

The solution where AgBr has the highest solubility is **C) pure water**.

Get Studdy

Studdy solves anything!

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

QuestionIn which of the following aqueous solutions would you expect AgBr to have the highest solubility? A) 0.15 M KBr B) 0.10 M LiBr C) pure water D) $0.10 \mathrm{M} \mathrm{AgNO}_{3}$ E) 0.20 M NaBr

1. Identify the common ion effect
2. Compare solubility in different solutions
3. Determine the highest solubility

Alright, so we know that the more common ions there are, the less AgBr dissolves.
Pure water doesn't have any of these ions, so AgBr can dissolve the most there!

The solution where AgBr has the highest solubility is C) pure water.