Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 74

What acid and what base would react in aqueous solution so that the following salts appear as products in the formula equation? Write the balanced formula equation for each reaction. a. potassium perchlorate b. cesium nitrate c. calcium iodide

Short Answer

Expert verified
a. HClO4(aq) + KOH(aq) -> KClO4(aq) + H2O(l) b. HNO3(aq) + CsOH(aq) -> CsNO3(aq) + H2O(l) c. 2HI(aq) + Ca(OH)2(aq) -> CaI2(aq) + 2H2O(l)

Step by step solution

01

Identify the Cation and Anion of the Salt

In potassium perchlorate, the cation is potassium (K+) and the anion is perchlorate (ClO4-).
02

Identify the Acid and Base

The acid and the base components that would form the potassium perchlorate salt are: - Acid: a compound that contains the ClO4- anion. A common acid with the perchlorate anion is perchloric acid (HClO4). - Base: a compound that contains the K+ cation. A common base with the potassium cation is potassium hydroxide (KOH).
03

Write the Balanced Formula Equation

Now, we'll write a balanced formula equation for the reaction between HClO4 and KOH in an aqueous solution: HClO4(aq) + KOH(aq) -> KClO4(aq) + H2O(l) b. cesium nitrate
04

Identify the Cation and Anion of the Salt

In cesium nitrate, the cation is cesium (Cs+) and the anion is nitrate (NO3-).
05

Identify the Acid and Base

The acid and the base components that would form cesium nitrate are: - Acid: a compound that contains the NO3- anion. A common acid with the nitrate anion is nitric acid (HNO3). - Base: a compound that contains the Cs+ cation. A common base with the cesium cation is cesium hydroxide (CsOH).
06

Write the Balanced Formula Equation

Now, we'll write a balanced formula equation for the reaction between HNO3 and CsOH in an aqueous solution: HNO3(aq) + CsOH(aq) -> CsNO3(aq) + H2O(l) c. calcium iodide
07

Identify the Cation and Anion of the Salt

In calcium iodide, the cation is calcium (Ca2+) and the anion is iodide (I-).
08

Identify the Acid and Base

The acid and the base components that would form calcium iodide are: - Acid: a compound that contains the I- anion. A common acid with the iodide anion is hydroiodic acid (HI). - Base: a compound that contains the Ca2+ cation. A common base with the calcium cation is calcium hydroxide (Ca(OH)2).
09

Write the Balanced Formula Equation

Now, we'll write a balanced formula equation for the reaction between HI and Ca(OH)2 in an aqueous solution. Note that you'll need two molecules of HI to balance the charges with the Ca2+ ion: 2HI(aq) + Ca(OH)2(aq) -> CaI2(aq) + 2H2O(l)

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

When organic compounds containing sulfur are bumed, sulfur dioxide is produced. The amount of \(\mathrm{SO}_{2}\) formed can be determined by the reaction with hydrogen peroxide: $$\mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{SO}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)$$ The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.302 -g sample of coal is burned and the \(\mathrm{SO}_{2}\) is collected in a solution of hydrogen peroxide. It took 28.44 \(\mathrm{mL}\) of a $0.1000-M \mathrm{NaOH}$ solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.

Balance the following oxidation–reduction reactions that occur in basic solution. a. $\mathrm{Al}(s)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{MnO}_{2}(s)+\mathrm{Al}(\mathrm{OH})_{4}-(a q)$ b. \(\mathrm{Cl}_{2}(g) \rightarrow \mathrm{Cl}^{-}(a q)+\mathrm{OCl}^{-}(a q)\) c. $\mathrm{NO}_{2}^{-}(a q)+\mathrm{Al}(s) \rightarrow \mathrm{NH}_{3}(g)+\mathrm{AlO}_{2}^{-}(a q)$

A 450.0 -mL sample of a \(0.257-M\) solution of silver nitrate is mixed with 400.0 \(\mathrm{mL}\) of 0.200\(M\) calcium chloride. What is the concentration of \(\mathrm{Cl}^{-}\) in solution after the reaction is complete?

The thallium (present as \(\mathrm{Tl}_{2} \mathrm{SO}_{4} )\) in a \(9.486-\mathrm{g}\) pesticide sam- ple was precipitated as thallium(I) iodide. Calculate the mass percent of \(\mathrm{TI}_{2} \mathrm{SO}_{4}\) in the sample if 0.1824 \(\mathrm{g}\) of TIII was recovered.

A student titrates an unknown amount of potassium hydrogen phthalate $\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}, \text { often abbreviated } \mathrm{KHP}\right)\( with 20.46 \)\mathrm{mL}$ of a 0.1000-M NaOH solution. KHP (molar mass 5 204.22 g/ mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

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