Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 110

Carbonic acid occurs in carbonated beverages. When allowed to react with lithium hydroxide, it produces lithium carbonate. Lithium carbonate is used to treat depression and bipolar disorder. Write chemical formulas for carbonic acid, lithium hydroxide, and lithium carbonate.

Short Answer

Expert verified
The chemical formulas for the given compounds are: Carbonic acid: \(H_2CO_3\) Lithium hydroxide: \(LiOH\) Lithium carbonate: \(Li_2CO_3\)

Step by step solution

01

Identify element symbols and charges

First, we need to identify the symbols and charges of each element involved. Carbonic acid consists of hydrogen, carbon, and oxygen, which have the respective symbols H, C, and O. Lithium hydroxide consists of lithium and hydroxide (which itself consists of oxygen and hydrogen), having the symbols Li, O, and H. Lastly, lithium carbonate is made up of lithium, carbon, and oxygen, so the symbols are Li, C, and O.
02

Determine oxidation states

Now, we need to determine the oxidation states, or charges, of each element. Hydrogen typically has a charge of +1, carbon in carbonate has a charge of +4, oxygen in both carbonate and hydroxide has a charge of -2, and lithium has a charge of +1.
03

Write the chemical formula for carbonic acid

We start by writing the chemical formula for carbonic acid (H₂CO₃). Carbonic acid is an acid, so we begin with hydrogen. Since hydrogen has a charge of +1 and we need a total charge of +4 to balance out the -2 charge from each of the three oxygen atoms, we will need two hydrogen atoms (2 * +1 = +2). Next, we add one carbon atom (+4) and three oxygen atoms (3 * -2 = -6), which results in a total charge of 0. Therefore, the formula for carbonic acid is H₂CO₃.
04

Write the chemical formula for lithium hydroxide

To write the chemical formula for lithium hydroxide (LiOH), we combine one lithium atom with one hydroxide group. Lithium has a charge of +1 and hydroxide (OH) has a charge of -1, which results in a total charge of 0. Therefore, the formula for lithium hydroxide is LiOH.
05

Write the chemical formula for lithium carbonate

Lastly, we write the chemical formula for lithium carbonate (Li₂CO₃). Since lithium has a charge of +1 and carbonate (CO₃) has a charge of -2, we will need two lithium atoms (2 * +1 = +2) to balance out the charge of one carbonate group (-2). Thus, the formula for lithium carbonate is Li₂CO₃. In conclusion, the chemical formulas for the given compounds are as follows: Carbonic acid: H₂CO₃ Lithium hydroxide: LiOH Lithium carbonate: Li₂CO₃

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

Name each of the following oxides. Assuming that the compounds are ionic, what charge is associated with the metallic element in each case? \((\mathbf{a})\) \(\mathrm{NiO},(\mathbf{b}) \mathrm{MnO}_{2},(\mathbf{c}) \mathrm{Cr}_{2} \mathrm{O}_{3}\) \((\mathbf{d}) \mathrm{MoO}_{3}\)

Elements in the same group of the periodic table often form oxyanions with the same general formula. The anions are also named in a similar fashion. Based on these observations,suggest a chemical formula or name, as appropriate, for each of the following ions:\((\mathbf{a}) \mathrm{BrO}_{4}^{-},(\mathbf{b}) \mathrm{SeO}_{3}^{2-}\) \((\mathbf{c})\) arsenate ion, \((\mathbf{d})\) hydrogen tellurate ion.

Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass \(=84.9118\) amu; abundance \(=72.15 \%\) ) and rubidium-87 (atomic mass = 86.9092 amu; abundance = 27.85\(\%\) ). Calculate the atomic weight of rubidium.

Selenium, an element required nutritionally in trace quantities, forms compounds analogous to sulfur. Name the following ions: (a) \(\operatorname{SeO}_{4}^{2-},(\mathbf{b}) \mathrm{Se}^{2-},(\mathbf{c}) \mathrm{HSe}^{-},(\mathbf{d}) \mathrm{HSeO}_{3}^{-}\)

There are two different isotopes of bromine atoms. Under normal conditions, elemental bromine consists of Br_{2} \text molecules, and the mass of a Br \(_{2}\) molecule is the sum of the masses of the two atoms in the molecule. The mass spectrum of Br_{2} consists of three peaks:(a) What is the origin of each peak (of what isotopes does each consist)? (b) What is the mass of each isotope? (c) Determine the average molecular mass of a Br_ molecule. (d) Determine the average atomic mass of a bromine atom. (e) Calculate the abundances of the two isotopes.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

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