/*! 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 37 List the sulfates of the Group 2... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 21: Problem 37

List the sulfates of the Group 2 A metals in order of increasing solubility in water. Explain the trend. (Hint: You need to consult a chemistry handbook.)

Short Answer

Expert verified
In general, the solubility of Group 2A sulfates decreases from BeSO鈧� to BaSO鈧� as the ion size increases from Be to Ba. This is due to a decrease in hydration energy and relatively constant lattice energy as we move down the group.

Step by step solution

01

Retrieving Solubility Data

Consult a reliable chemistry handbook or a related resource and find the solubility of the sulfates of Group 2 A metals. Group 2 A metals include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), and Barium (Ba). So, find the solubilities of BeSO鈧�, MgSO鈧�, CaSO鈧�, SrSO鈧�, and BaSO鈧�, and list them down.
02

Organizing Solubility Data

Organize this data in increasing order of solubility. That means starting with the metal sulfate having the least solubility and ending with the one having the greatest solubility.
03

Explaining the Trend

The solubility trends in water for Group 2 A metal sulfates typically reflect the hydration energy and the lattice energy of the sulfates. As we move down the group, the size of the cation increases, which decreases the effective charge density, thus, the hydration energy decreases. But, the lattice energy changes less significantly. So, the solubility decreases on moving down the group in Group 2 A elements.

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.

Solubility Trend
In the realm of chemistry, solubility refers to the ability of a substance to dissolve in a solvent, forming a solution. For Group 2 A metal sulfates, this is an intriguing topic as you journey down the periodic table. The trend you observe in their solubility is primarily influenced by two factors: hydration energy and lattice energy. When looking at the sulfates of Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), and Barium (Ba), an intriguing pattern emerges.
  • BeSO鈧� exhibits considerable solubility.
  • MgSO鈧� is also quite soluble in water.
  • Moving to CaSO鈧�, a noticeable decrease in solubility occurs.
  • The decline becomes more pronounced with SrSO鈧� and BaSO鈧�.
These observations suggest that as you move down Group 2 A, the solubility of sulfates decreases due to the changing balance between lattice and hydration energy.
Hydration Energy
Hydration energy is a key player in the solubility equation. It refers to the energy released when ions dissolve in water and become surrounded by water molecules. For Group 2 A metals, this energy is strongly linked to the size of the cation in question. As the cation size increases from Beryllium to Barium, the charge density decreases. This results in lower hydration energy because larger ions are less effective at drawing water molecules around them.
  • Higher hydration energy makes a substance more soluble.
  • In Group 2 A, smaller ions like Beryllium attract more hydration energy.
  • Conversely, larger ions such as Barium exhibit lower hydration energy.
Therefore, the observed decrease in solubility as we move down the group relates directly to the drop in hydration energy.
Lattice Energy
To fully grasp the solubility trend, lattice energy must also be understood. Lattice energy is the energy needed to separate the ions in a solid for them to dissolve in a solution. The interaction between ions, and hence lattice energy, is more pronounced in smaller ions. Consequently, in Group 2 A metals, lattice energy diminishes less significantly than hydration energy as you move down the group.
  • High lattice energy means strong ion attractions in the solid, reducing solubility.
  • Even as cation size increases (and enhances lattice energy), the predominant decline in hydration energy dictates the overall solubility trend.
  • This interplay determines that the solubility pattern emerges as is observed when ordering the sulfates.
Understanding lattice energy helps explain why the solubility decreases even when the cation size increases.
Chemistry Handbook
A chemistry handbook is your treasure trove for reliable and accurate data. It's an essential tool when you need detailed information about chemical compounds, like the solubility of metal sulfates.
  • Handbooks provide systematic data, including solubility values.
  • They serve as a guide for scientific inquiries, offering explanations about trends, effects, and implications.
  • In exercises involving Group 2 A metal sulfates, consulting a chemistry handbook gives you the data you need to observe and verify trends.
When working through chemical problems, using such a resource allows you to cross-check your findings and ensure that they align with documented scientific knowledge.

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

What is wrong with the following procedure for obtaining magnesium?$$\begin{aligned}& \mathrm{MgCO}_{3} \longrightarrow \mathrm{MgO}(s)+\mathrm{CO}_{2}(g) \\\\\mathrm{MgO}(s)+\mathrm{CO}(g) & \longrightarrow \mathrm{Mg}(s)+\mathrm{CO}_{2}(g)\end{aligned}$$

Complete and balance the following equations: (a) \(\mathrm{K}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\operatorname{NaH}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow\) (d) \(\mathrm{K}(s)+\mathrm{O}_{2}(g) \longrightarrow\)

Although iron is only about two-thirds as abundant as aluminum in Earth's crust, mass for mass it costs only about one-quarter as much to produce. Why?

How is sodium prepared commercially?

In steelmaking, nonmetallic impurities such as \(\mathrm{P}, \mathrm{S}\) and \(\mathrm{Si}\) are removed as the corresponding oxides. The inside of the furnace is usually lined with \(\mathrm{CaCO}_{3}\) and \(\mathrm{MgCO}_{3},\) which decompose at high temperatures to yield \(\mathrm{CaO}\) and \(\mathrm{MgO}\). How do \(\mathrm{CaO}\) and \(\mathrm{MgO}\) help in the removal of the nonmetallic oxides?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Physical 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.