Skip to main content
Ch.13 - Properties of Solutions
Chapter 13, Problem 25d

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution: (d) Pb(NO3)2.

Verified Solution

Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility

Solubility is the maximum amount of a solute that can dissolve in a given quantity of solvent at a specific temperature. It is typically expressed in grams of solute per 100 grams of solvent. Understanding solubility is crucial for determining whether a solution can become saturated, meaning no more solute can dissolve in the solvent.
Recommended video:
Guided course
00:28
Solubility Rules

Saturated Solution

A saturated solution is one in which the maximum amount of solute has been dissolved in the solvent at a given temperature and pressure. When additional solute is added to a saturated solution, it will not dissolve and will remain undissolved. Identifying whether a solution is saturated is essential for predicting the behavior of solutes in a solvent.
Recommended video:
Guided course
01:11
Types of Aqueous Solutions

Ionic Compounds and Their Solubility

Ionic compounds, such as Pb(NO3)2, dissociate into their constituent ions when dissolved in water. The solubility of these compounds varies widely based on their chemical nature and the temperature of the solvent. Knowledge of the solubility rules for ionic compounds helps predict whether a specific ionic solid will dissolve in water, which is key to answering the question about saturation.
Recommended video:
Guided course
02:30
Soluble Ionic Solutes
Related Practice
Textbook Question

Two nonpolar organic liquids, hexane (C6H14) and heptane (C7H16), are mixed. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?

620
views
Textbook Question

KBr is relatively soluble in water, yet its enthalpy of solution is + 19.8 kJ/mol. Which of the following statements provides the best explanation for this behavior? (a) Potassium salts are always soluble in water. (b) The entropy of mixing must be unfavorable. (c) The enthalpy of mixing must be small compared to the enthalpies for breaking up water–water interactions and K–Br ionic interactions. (d) KBr has a high molar mass compared to other salts like NaCl.

2713
views
1
rank
Textbook Question

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution:(c) K2Cr2O7

403
views
Textbook Question

By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (b) Pb(NO3)2,

436
views
Textbook Question

By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (c) Ce2(SO4)3.

967
views
2
rank
Textbook Question

Oil and water are immiscible. Which is the most likely reason? (a) Oil molecules are denser than water. (b) Oil molecules are composed mostly of carbon and hydrogen. (c) Oil molecules have higher molar masses than water. (d) Oil molecules have higher vapor pressures than water. (e) Oil molecules have higher boiling points than water.

1609
views