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Chapter 4: Problem 68

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 ions in the salt

Potassium perchlorate has a chemical formula of KClO4. It consists of a potassium ion (K+) and a perchlorate ion (ClO4-).
02

Identify the acidic and basic components

The acidic component would provide the ClO4- ion, which is a part of perchloric acid (HClO4). The basic component would provide the K+ ion and is found in potassium hydroxide (KOH).
03

Write the balanced formula equation for the reaction

When HClO4 and KOH react, they neutralize each other to produce water and the salt, potassium perchlorate. The balanced formula equation for this reaction is: HClO4(aq) + KOH(aq) → KClO4(aq) + H2O(l) b. cesium nitrate
04

Identify the ions in the salt

Cesium nitrate has a chemical formula of CsNO3. It consists of a cesium ion (Cs+) and a nitrate ion (NO3-).
05

Identify the acidic and basic components

The acidic component would provide the NO3- ion, which is a part of nitric acid (HNO3). The basic component would provide the Cs+ ion and is found in cesium hydroxide (CsOH).
06

Write the balanced formula equation for the reaction

When HNO3 and CsOH react, they neutralize each other to produce water and the salt, cesium nitrate. The balanced formula equation for this reaction is: HNO3(aq) + CsOH(aq) → CsNO3(aq) + H2O(l) c. calcium iodide
07

Identify the ions in the salt

Calcium iodide has a chemical formula of CaI2. It consists of a calcium ion (Ca2+) and two iodide ions (I-).
08

Identify the acidic and basic components

The acidic component would provide the I- ion, which is a part of hydroiodic acid (HI). The basic component would provide the Ca2+ ion and is found in calcium hydroxide (Ca(OH)2).
09

Write the balanced formula equation for the reaction

When HI and Ca(OH)2 react, they neutralize each other to produce water and the salt, calcium iodide. Since the calcium ion has a charge of 2+, we will need two HI molecules in the reaction. The balanced formula equation for this reaction is: 2HI(aq) + Ca(OH)2(aq) → CaI2(aq) + 2H2O(l)

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Most popular questions from this chapter

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

In a 1-L beaker, \(203 \mathrm{~mL}\) of \(0.307 \mathrm{M}\) ammonium chromate was mixed with \(137 \mathrm{~mL}\) of \(0.269 \mathrm{M}\) chromium(III) nitrite to produce ammonium nitrite and chromium(III) chromate. Write the balanced chemical reaction occurring here. If the percent yield of the reaction was \(88.0 \%\), what mass of chromium(III) chromate was isolated?

A \(10.00-\mathrm{mL}\) sample of sulfuric acid from an automobile battery requires \(35.08 \mathrm{~mL}\) of \(2.12 \mathrm{M}\) sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? Sulfuric acid contains two acidic hydrogens.

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{UO}_{2}^{2+}\) f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) b. \(\mathrm{As}_{2} \mathrm{O}_{3} \quad\) g. \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) c. \(\mathrm{NaBiO}_{3}\) h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) d. As i. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) e. \(\mathrm{HAsO}_{2}\)

A \(25.00\) -mL sample of hydrochloric acid solution requires 24\. 16 mL of \(0.106 M\) sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?
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