/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 32 Which of the following solutions... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 32

Which of the following solutions is the most basic? (a) \(0.6 \mathrm{M} \mathrm{NH}_{3}\), (b) \(0.150 \mathrm{M} \mathrm{KOH}\), (c) \(0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\).

Short Answer

Expert verified
The most basic solution among the given options is (a) 0.6 M NH3, as it has the highest concentration of hydroxide ions (0.6 M).

Step by step solution

01

Identify the number of hydroxide ions each solute releases in the solution

Each solute in the given solutions releases a certain amount of hydroxide ions when dissolved in water. NH3, being a weak base, reacts with water to form NH4+ and OH- ions. KOH and Ba(OH)2 are strong bases and dissociate completely in the solution, forming their respective cations and OH- ions. (a) NH3 - releases 1 OH- ion (b) KOH - releases 1 OH- ion (c) Ba(OH)2 - releases 2 OH- ions
02

Calculate the concentration of hydroxide ions for each solution

Now that we know the number of hydroxide ions each solute releases, we can calculate the concentration of hydroxide ions in each solution by multiplying the given concentration of the solute with the number of hydroxide ions released. (a) [OH-] in NH3 solution = 0.6 M * 1 = 0.6 M (b) [OH-] in KOH solution = 0.150 M * 1 = 0.150 M (c) [OH-] in Ba(OH)2 solution = 0.100 M * 2 = 0.200 M
03

Compare the concentration of hydroxide ions in the solutions and determine which is the most basic

It's time to compare the calculated concentrations of hydroxide ions in the three solutions to find out which solution is the most basic. The higher the concentration of hydroxide ions, the more basic the solution. [OH-] in NH3 solution = 0.6 M [OH-] in KOH solution = 0.150 M [OH-] in Ba(OH)2 solution = 0.200 M Since the NH3 solution has the highest concentration of hydroxide ions (0.6 M), it is the most basic among the given solutions. Therefore, the answer is: (a) 0.6 M NH3

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Basicity
Basicity refers to the ability of a substance to act as a base, which typically involves accepting protons or donating pairs of electrons. In aqueous solutions, a key indicator of basicity is the concentration of hydroxide ions (OH鈦�) present. The more OH鈦� ions a substance can generate, the stronger its basicity. Basicity is also often associated with the pH scale, where basic solutions have a pH greater than 7. When comparing solutions, the one with the higher concentration of OH鈦� ions is deemed more basic. For example, in the given solutions, the ammonia (\( \text{NH}_3 \)) solution has a high basicity due to its relatively large amount of hydroxide ions compared to the others.
Concentration of Hydroxide Ions
The concentration of hydroxide ions in a solution determines its basicity. It directly relates to how many hydroxide ions (\( \text{OH}^- \)) are available per liter of solution. When a base dissolves in water, its dissociation determines how many hydroxide ions are released.
  • Strong bases dissociate completely, releasing their maximum potential hydroxide ions.
  • Weak bases only partially dissociate, producing fewer hydroxide ions.
In the exercise provided, the concentration of hydroxide ions was calculated by multiplying the molarity of the solution by the number of hydroxide ions each solute releases:
  • For \( \text{NH}_3 \), which releases one OH鈦� ion: \[ \text{[OH}^-\text{] in } \text{NH}_3 = 0.6 \, \text{M} * 1 = 0.6 \, \text{M} \]
  • For \( \text{KOH} \), which also releases one OH鈦� ion: \[ \text{[OH}^-\text{] in KOH} = 0.150 \, \text{M} * 1 = 0.150 \, \text{M} \]
  • For \( \text{Ba(OH)}_2 \), releasing two OH鈦� ions: \[ \text{[OH}^-\text{] in } \text{Ba(OH)}_2 = 0.100 \, \text{M} * 2 = 0.200 \, \text{M} \]
This list shows how hydroxide ion concentration helps us determine that the \( \text{NH}_3 \) solution is the most basic due to its higher concentration of hydroxide ions.
Strong and Weak Bases
Bases are classified as either strong or weak based on their ability to dissociate in water and produce hydroxide ions. Strong Bases: These are characterized by their complete dissociation in water. They release all their potential hydroxide ions, making them highly basic. Examples include potassium hydroxide (\(\text{KOH}\)) and barium hydroxide (\(\text{Ba(OH)}_2\)). Because they dissociate fully, the concentration of OH鈦� equals their initial molarity (or is multiplied if more than one OH鈦� per molecule is released).Weak Bases: In contrast, weak bases do not fully dissociate in solution. They partially release hydroxide ions, which means their solutions usually have a lower hydroxide concentration compared to strong bases of similar molarity. An example is ammonia (\(\text{NH}_3\)), which partly converts to ammonium (\(\text{NH}_4^+\)) and hydroxide ions when dissolved.In practical terms, the more a base dissociates into hydroxide ions, the stronger it is considered to be, and this impacts our calculations of their respective hydroxide ion concentrations.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) \(\begin{aligned} \mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow & \longrightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+10 \mathrm{HCl}(a q) \end{aligned}\) (b) \(\mathrm{Br}_{2}(l)+2 \mathrm{~K}(s) \longrightarrow 2 \mathrm{KBr}(s)\) (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)\) (d) \(\mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+\) \(2 \mathrm{NaCl}(a q)\)

Indicate the concentration of each ion present in the solution formed by mixing (a) \(42.0 \mathrm{~mL}\) of \(0.170 \mathrm{M} \mathrm{NaOH}\) with \(37.6 \mathrm{~mL}\) of \(0.400 \mathrm{M} \mathrm{NaOH}\), (b) \(44.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\) with \(25.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{KCl}\), (c) \(3.60 \mathrm{~g} \mathrm{KCl}\) in \(75.0 \mathrm{~mL}\) of \(0.250 \mathrm{M} \mathrm{CaCl}_{2}\) solution. Assume that the volumes are additive.

A person suffering from hyponatremia has a sodium ion concentration in the blood of \(0.118 \mathrm{M}\) and a total blood volume of \(4.6 \mathrm{~L}\). What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to \(0.138 \mathrm{M}\), assuming no change in blood volume?

(a) How many grams of solid silver nitrate would you need to prepare \(200.0 \mathrm{~mL}\) of a \(0.150 \mathrm{M} \mathrm{AgNO}_{3}\) solution? (b) An experiment calls for you to use \(100 \mathrm{~mL}\) of \(0.50 \mathrm{MHNO}_{3}\) solution. All you have available is a bottle of \(3.6 \mathrm{M} \mathrm{HNO}_{3}\). How many milliliters of the \(3.6 \mathrm{M} \mathrm{HNO}_{3}\) solution and of water do you need to prepare the desired solution?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.