/*! 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 5 Write the formula for each of th... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 5

Write the formula for each of the following acids and bases: a. magnesium hydroxide b. hydrofluoric acid c. phosphoric acid d. lithium hydroxide e. ammonium hydroxide f. sulfuric acid

Short Answer

Expert verified
a. Mg(OH)_2, b. HF, c. H_3PO_4, d. LiOH, e. NH_4OH, f. H_2SO_4

Step by step solution

01

- Understanding Magnesium Hydroxide

Magnesium hydroxide is a base formed from magnesium ions (Mg^{2+}) and hydroxide ions (OH^{-}). The chemical formula is determined by balancing the charges: hydroxide has a charge of -1, so we need two hydroxide ions to balance the +2 charge of magnesium. The formula is Mg(OH)_2.
02

- Writing Hydrofluoric Acid Formula

Hydrofluoric acid is formed from hydrogen ions (H^{+}) and fluoride ions (F^{-}). Since the charges are equal and opposite, one hydrogen ion pairs with one fluoride ion. The formula is HF.
03

- Writing Phosphoric Acid Formula

Phosphoric acid contains three hydrogen ions (H^{+}) and one phosphate ion (PO_4^{3-}). The chemical formula is obtained by balancing the charges: three hydrogen ions are needed to balance the -3 charge of phosphate. The formula is H_3PO_4.
04

- Understanding Lithium Hydroxide

Lithium hydroxide is a base formed from lithium ions (Li^{+}) and hydroxide ions (OH^{-}). Since the charges are equal and opposite, one lithium ion pairs with one hydroxide ion. The formula is LiOH.
05

- Writing Ammonium Hydroxide Formula

Ammonium hydroxide is formed from ammonium ions (NH_4^{+}) and hydroxide ions (OH^{-}). Since the charges are equal and opposite, one ammonium ion pairs with one hydroxide ion. The formula is NH_4OH.
06

- Understanding Sulfuric Acid

Sulfuric acid contains two hydrogen ions (H^{+}) and one sulfate ion (SO_4^{2-}). The chemical formula is derived by balancing the charges: two hydrogen ions balance the -2 charge of sulfate. The formula is H_2SO_4.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

chemical formulas
Understanding chemical formulas is fundamental in chemistry. A chemical formula represents the elements present in a compound and the ratio in which the atoms of these elements combine. For acids and bases:
  • A chemical formula consists of the symbols of the elements involved.
  • Subscripts indicate the number of each type of atom in the compound.
  • No subscript means one atom of that element.
For example, in the formula for sulfuric acid, H2SO4 means there are two hydrogen atoms (H), one sulfur atom (S), and four oxygen atoms (O) in each molecule of sulfuric acid.
acid-base chemistry
Acid-base chemistry studies substances that release hydrogen ions (H+) or hydroxide ions (OH-) in solution.
  • Acids typically release hydrogen ions when dissolved in water. For instance, hydrofluoric acid (HF) releases H+ and F- in water.
  • Bases typically release hydroxide ions when dissolved in water. Magnesium hydroxide (Mg(OH)2) releases Mg2+ and OH- ions.
The strength of an acid or base is determined by how completely it dissociates in water. Strong acids and bases dissociate completely, whereas weak acids and bases do not.
ionic compounds
Ionic compounds are formed by the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions).
In acid-base compounds:
  • Acids often contain hydrogen ions (H+) paired with anions. For example, sulfuric acid (H2SO4) contains H+ ions and sulfate ions (SO42-).
  • Bases often contain hydroxide ions (OH-) paired with cations. Lithium hydroxide (LiOH) contains Li+ ions and OH- ions.
Ionic compounds have high melting and boiling points due to the strong electrostatic forces between the ions.
charge balancing
Charge balancing is crucial when writing chemical formulas for acids and bases. The total positive charge must equal the total negative charge.

Here鈥檚 how to balance charges:
  • Identify the charges of the ions. For example, the hydroxide ion (OH-) has a -1 charge, and the magnesium ion (Mg2+) has a +2 charge.
  • Balance the charges by adjusting the number of ions. Magnesium hydroxide, Mg(OH)2, requires two OH- ions to balance one Mg2+ ion.
Always ensure the net charge of the compound is zero.
common acids and bases
Knowing the common acids and bases is essential in chemistry. Here are a few:
  • Hydrofluoric acid (HF) is a weak acid used in etching glass.
  • Phosphoric acid (H3PO4) is used in fertilizers and soft drinks.
  • Magnesium hydroxide (Mg(OH)2) is a base found in milk of magnesia, a common antacid.
  • Lithium hydroxide (LiOH) is used in lithium batteries and as a CO2 scrubber.
  • Ammonium hydroxide (NH4OH) is utilized in household cleaners.
  • Sulfuric acid (H2SO4) is a strong acid used in car batteries and industrial processes.
Familiarity with these compounds and their formulas is beneficial for many chemical applications.

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 acids or bases: a. \(\mathrm{HCl}\) b. \(\mathrm{Ca}(\mathrm{OH})_{2}\) c. \(\mathrm{H}_{2} \mathrm{CO}_{3}\) d. \(\mathrm{HNO}_{3}\) e. \(\mathrm{H}_{2} \mathrm{SO}_{3}\)

Identify the Br酶nsted-Lowry acid-base pairs in each of the following equations: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)\) b. \(\mathrm{CO}_{3}{ }^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{OH}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q)\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NH}_{3}(a q) \rightleftarrows \mathrm{NH}_{4}{ }^{+}(a q)+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)\)

Identify the stronger acid in each of the following pairs: a. \(\mathrm{NH}_{4}^{+}\) or \(\mathrm{H}_{3} \mathrm{O}^{+}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) or \(\mathrm{HCN}\) c. \(\mathrm{H}_{2} \mathrm{O}\) or \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

What is the molarity of a \(\mathrm{HCl}\) solution if \(5.00 \mathrm{~mL}\) is neutralized by \(28.6 \mathrm{~mL}\) of a \(0.145 \mathrm{M} \mathrm{NaOH}\) solution? $$ \mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$

A solution of \(0.162\) M \(\mathrm{NaOH}\) is used to neutralize \(25.0 \mathrm{~mL}\) of a \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution. If \(32.8 \mathrm{~mL}\) of the \(\mathrm{NaOH}\) solution is required, what is the molarity of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution? \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

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.