Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Q81E (page 224)

In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO3)2 solution.

2Cl−(aq) + Hg(NO3)2(aq)⟶2NO3−(aq) + HgCl2(s)

What is the Cl− concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of 8.25×10−4MHg(NO3)2(aq) to reach the end point?

Short Answer

Expert verified

The requiredCl− concentration is 9.6 x 10-3 M

Step by step solution

01

Given Data

2Cl−(aq) + Hg(NO3)2(aq)⟶2NO3−(aq) + HgCl2(s)

Hg(NO3)2(aq) = 8.25×10−4 M

Volume of Hg(NO3)2 = 1.46 mL = 0.01146 L

Sample volume = 0.25 mL = 2.5 x 10 -4 L

Molarity(M) = mol/ L

So, no of mol of Hg(NO3)2 = M x L

= 8.25×10−4 M x 0.00146 L

=1.2045 x 10-6 Hg(NO3)2

02

Determine concentration of Cl−

\(\begin{aligned}{}\frac{{1.2045{\rm{ }}x{\rm{ }}{{10}^{ - 6}}Hg{{\left( {N{O_3}} \right)}_2} \times 2\,mol\,of\,C{l^ - }}}{{1\,mol\,Hg{{\left( {N{O_3}} \right)}_2}}}\\ = 2.409 \times {10^{ - 6}}\,mol\,of\,C{l^ - }\end{aligned}\)

Required concentration of Cl

\(\begin{aligned}{} = \frac{{2.409 \times {{10}^{ - 6}}\,mol\,of\,C{l^ - }}}{{2.5 \times {{10}^{ - 4}}L}}\\ = 9.6 \times {10^{ - 3}}M\end{aligned}\)

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide).

(a) Write an equation of the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water.

(b)The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solution of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.

Consider molecular, complete ionic and net ionic equations.

(a) What is the difference between these types of equations?

(b) In what circumstances would the complete ionic and net ionic equations for a reaction be identical?

Balance the following equations:

\(\begin{array}{l}\left( a \right)\,Ag\left( s \right) + {H_2}S\left( g \right) + {O_2}\left( g \right) \to A{g_2}S\left( s \right) + {H_2}O\left( l \right)\\\left( b \right)\,{P_4}\left( s \right) + {O_2}\left( g \right) \to {P_4}{O_{10}}\left( s \right)\\\left( c \right)\,Pb\left( s \right) + {H_2}O\left( l \right) + {O_2}\left( g \right) \to Pb{\left( {OH} \right)_2}\left( s \right)\\\left( d \right)\,Fe\left( s \right) + {H_2}O\left( l \right) \to F{e_3}{O_4}\left( s \right) + {H_2}\left( g \right)\\\left( e \right)\,S{c_2}{O_3}\left( s \right) + S{O_3}\left( g \right) \to S{c_2}{\left( {S{O_4}} \right)_3}\left( s \right)\\\left( f \right)\,C{a_3}{\left( {P{O_4}} \right)_2}\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to Ca{\left( {{H_2}P{O_4}} \right)_2}\left( {aq} \right)\\\left( g \right)\,Al\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to A{l_2}{\left( {S{O_4}} \right)_3}\left( s \right) + {H_2}\left( g \right)\\\left( h \right)\,TiC{l_4}\left( s \right) + {H_2}O\left( g \right) \to Ti{O_2}\left( s \right) + HCl\left( g \right)\end{array}\)

Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process.

(a)The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide.

(b)The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water.

(c)Solid calcium hydroxide is the added to the sea water, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride

(d)The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.

(e)Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

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.

Sign-up for free