   Chapter 16, Problem 67E

Chapter
Section
Textbook Problem

# The overall formation constant for HgI42− is 1.0 × 1030. That is, 1.0   ×   10 30   =   [ H g I 4 2 − ] [ H g 2 + ] [ I − ] 4 What is the concentration of Hg2+ in 500.0 mL of a solution that was originally 0.010 M Hg2+ and 0.78 M I−? The reaction is Hg 2+ ( a q )   +   4 I − ( a q )   ⇌   H g I 4 2 − ( a q )

Interpretation Introduction

Interpretation: The combination reaction of Hg2+ and I , the overall formation constant of HgI42 and concentration of Hg2+,I before the reaction is given. The concentration of Hg2+ in the given volume of a solution is to be calculated.

Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Explanation

To determine: The concentration of Hg2+ in 500mL of the given solution.

Given

Concentration of Hg2+ before reaction is 0.010M .

Concentration of I before reaction is 0.78M .

The overall formation constant for HgI42 is 1.0×1030 .

The reaction that takes place is,

Hg2+(aq)+4I(aq)HgI42(aq)

The reaction is assumed to be completed. The net reaction is,

Hg2++4IHgI42Beforereaction0.010M0.78M0Afterreaction00.78(4×0.010)=0

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 