/*! 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} Q4.12P Question:聽State whether an aque... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Q4.12P (page 178)

Question:State whether an aqueous solution of each of the following substances conducts an electric current. Explain your reasoning.

(a) Caesium bromide (b) Hydrogen iodide

Short Answer

Expert verified

Answer

a) Yes, an aqueous solution of Caesium bromide conducts electric current.

b) Yes, an aqueous solution of Hydrogen iodide conducts electric current.

Step by step solution

01

Explain the solubility of ionic compounds in water

All the ionic compounds which dissociate into ions on dissolving in water conduct electricity because they contain charge and are free to move in the solution.

02

Determine the aqueous solution of given compounds conduct electricity or not

An aqueous solution of both the given compounds i.e.,

(a) Caesium bromide and (b) Hydrogen iodide can conduct electricity

Because both produce free moving charged ions on dissolving in water and conduct electric current.

In the case of Caesium bromide, it dissociates into CS+and Br-ions and conducts electricity.

In the case of Hydrogen iodide, it is a strong acid and dissociates completely in the water into H+and I_ ions through which it conducts electricity.

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

There are various methods for finding the composition of an alloy (a metal-like mixture). Show that calculating the mass % of Mg in a magnesium-aluminum alloy (d = 2.40 g/cm3) gives the same answer (within rounding) using each of these methods:

(a) a0.263-gsampleofalloy(dofMg=1.74g/cm3;dofAl=2.70g/cm3);

(b) an identical sample reacting with excess aqueous HCl forms 1.38x10-2molofH2;

(c) an identical sample reacting with excess O2 forms 0.483 g of oxide.

How many total moles of ions are released when each of the following samples dissolves completely in water?(a) 0.75 mol ofK3PO4 (b) 6.88脳10-3g ofNiBr2.3H2O (c) 2.23脳1022formula units ofFeCl3

To study a marine organism, a biologist prepares a 1.00-kg sample to simulate the ion concentrations in seawater. She mixes 26.5 g of NaCl, 2.40 g of MgCl2, 3.35 g of MgSO4, 1.20 g of CaCl2, 1.05 g of KCl, 0.315 g of NaHCO3, and 0.098 g of NaBr in distilled water.

(a) If the density of the solution is 1.025 g/cm3, what is the molarity of each ion?

(b) What is the total molarity of alkali metal ions?

(c) What is the total molarity of alkaline earth metal ions?

(d) What is the total molarity of anions?

Is the total ionic equation the same as the net ionic equation when Sr(OH)2(aq)and H2SO4(aq)react? Explain.

Question: In 1997, at the United Nations Conference on Climate Change, the major industrial nations agreed to expand their research efforts to develop renewable sources of carbon-based fuels. For more than a decade, Brazil has been engaged in a program to replace gasoline with ethanol derived from the root crop manioc (cassava).

(a) Write separate balanced equations for the complete combustion of ethanol (C2H5OH) and of gasoline (represented by the formula C8H18).

(b) What mass of oxygen is required to burn completely 1.00 L of a mixture that is 90.0% gasoline (d =0.742 g/mL) and 10.0% ethanol (d= 0.789 g/mL) by volume?

(c) If 1.00 mol of O2 occupies 22.4 L, what volume of O2 is needed to burn 1.00 L of the mixture?

(d) Air is 20.9% O2 by volume. What volume of air is needed to burn 1.00 L of the mixture?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

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.