/*! 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 6 You drop an ice cube (made from ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 6

You drop an ice cube (made from pure water) into a saltwater solution at \(0^{\circ} \mathrm{C}\). Explain what happens and why.

Short Answer

Expert verified
When an ice cube made of pure water is dropped into a saltwater solution at \(0^{\circ}\mathrm{C}\), it begins to melt due to the surrounding saltwater solution having a lower freezing point than pure water. This is because dissolved salt ions interfere with the formation of the crystalline ice structure, making it harder for the water molecules to freeze. As the ice cube melts, it dilutes the saltwater solution, causing its freezing point to rise closer to that of pure water. Eventually, thermal equilibrium is reached and the ice cube may dissolve completely, unless the ice cube is too large or the saltwater solution is already at its maximum freezing point depression.

Step by step solution

01

Understanding the Components

Before we proceed, let's understand the two components involved in this scenario. First, we have an ice cube made of pure water, meaning it is frozen water without any contaminants. Second, we have a saltwater solution at 0 degrees Celsius. This means the solution has salt (typically NaCl) dissolved in water, and it is at the freezing point of pure water.
02

Melting Point Depression

In a saltwater solution, the presence of salt particles interferes with the formation of solid water structures and lowers the freezing point compared to that of pure water. This phenomenon is known as "melting point depression" or "freezing point depression". When salt is dissolved in water, the freezing point of the solution decreases because the dissolved salt ions interfere with the ability of the water molecules to form crystalline ice structures, making it harder for the water to freeze.
03

What Happens to the Ice Cube

When the ice cube is dropped into the saltwater solution, the surrounding liquid is at 0 degrees Celsius, which is the freezing point of pure water but not the freezing point of the saltwater solution. As a result, the ice cube begins to melt since it is now in contact with a solution that is warmer than its own freezing point.
04

What Happens to the Saltwater Solution

As the ice cube melts, the water from the ice cube will mix with the saltwater solution. This addition of pure water will dilute the saltwater solution slightly, causing its freezing point to rise closer to that of pure water. However, as long as the salt concentration remains higher than zero, the freezing point of the saltwater solution will still be lower than 0 degrees Celsius.
05

Equilibrium and Final Scenario

The melting of the ice cube will continue until thermal equilibrium is reached between the ice and the saltwater solution. At this point, the temperature of the saltwater solution may drop slightly due to the melting of the ice and the dilution of the salt concentration. In most cases, the ice cube will eventually dissolve completely in the saltwater solution, unless the ice cube is too large or the saltwater solution is already at its maximum freezing point depression.

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!

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

Consider a beaker of salt water sitting open in a room. Over time, does the vapor pressure increase, decrease, or stay the same? Explain.

You make \(20.0 \mathrm{~g}\) of a sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) and \(\mathrm{NaCl}\) mixture and dissolve it in \(1.00 \mathrm{~kg}\) water. The freezing point of this solution s found to be \(-0.426^{\circ} \mathrm{C}\). Assuming ideal behavior, calculate the nass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.

At a certain temperature, the vapor pressure of pure benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) is \(0.930\) atm. A solution was prepared by dissolving \(10.0\) \(\mathrm{g}\) of a nondissociating, nonvolatile solute in \(78.11 \mathrm{~g}\) of benzene at that temperature. The vapor pressure of the solution was found to be \(0.900\) atm. Assuming the solution behaves ideally, determine the molar mass of the solute.

A solid mixture contains \(\mathrm{MgCl}_{2}\) and \(\mathrm{NaCl}\). When \(0.5000 \mathrm{~g}\) of this solid is dissolved in enough water to form \(1.000 \mathrm{~L}\) of solution, the osmotic pressure at \(25.0^{\circ} \mathrm{C}\) is observed to be \(0.3950 \mathrm{~atm}\). What is the mass percent of \(\mathrm{MgCl}_{2}\) in the solid? (Assume ideal behavior for the solution.)

Anthraquinone contains only carbon, hydrogen, and oxygen. When \(4.80 \mathrm{mg}\) anthraquinone is burned, \(14.2 \mathrm{mg} \mathrm{CO}_{2}\) and \(1.65 \mathrm{mg} \mathrm{H}_{2} \mathrm{O}\) are produced. The freezing point of camphor is lowered by \(22.3^{\circ} \mathrm{C}\) when \(1.32 \mathrm{~g}\) anthraquinone is dissolved in \(11.4 \mathrm{~g}\) camphor. Determine the empirical and molecular formulas of anthraquinone.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic 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.