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Chapter 6: Problem 70

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
The balanced formula equations for the given salts are as follows: a. Potassium perchlorate: KOH + HClO4 → KClO4 + H2O b. Cesium nitrate: CsOH + HNO3 → CsNO3 + H2O c. Calcium iodide: Ca(OH)2 + 2HI → CaI2 + 2H2O

Step by step solution

01

Identify Cation and Anion in Potassium Perchlorate

The given salt is potassium perchlorate (KClO4). The cation is the potassium ion (K+) and the anion is the perchlorate ion (ClO4-). #Step 2: Determine Acid and Base for potassium perchlorate (a)#
02

Determine Acid and Base for Potassium Perchlorate Reaction

To form potassium perchlorate, the cation is contributed from a base containing potassium ions, such as potassium hydroxide (KOH), and the anion comes from an acid containing the perchlorate ion, such as perchloric acid (HClO4). #Step 3: Write balanced formula equation for potassium perchlorate (a)#
03

Balanced Formula Equation for Potassium Perchlorate Reaction

Now we'll write the balanced equation for the reaction between potassium hydroxide and perchloric acid, producing potassium perchlorate and water. The balanced equation is: KOH + HClO4 → KClO4 + H2O Now we will repeat the steps for cesium nitrate (b) and calcium iodide (c). #Step 1: Identify Cation and Anion for cesium nitrate (b)#
04

Identify Cation and Anion in Cesium Nitrate

The given salt is cesium nitrate (CsNO3). The cation is the cesium ion (Cs+) and the anion is the nitrate ion (NO3-). #Step 2: Determine Acid and Base for cesium nitrate (b)#
05

Determine Acid and Base for Cesium Nitrate Reaction

To form cesium nitrate, the cation is contributed from a base containing cesium ions, such as cesium hydroxide (CsOH), and the anion comes from an acid containing the nitrate ion, such as nitric acid (HNO3). #Step 3: Write balanced formula equation for cesium nitrate (b)#
06

Balanced Formula Equation for Cesium Nitrate Reaction

Now we'll write the balanced equation for the reaction between cesium hydroxide and nitric acid, producing cesium nitrate and water. The balanced equation is: CsOH + HNO3 → CsNO3 + H2O #Step 1: Identify Cation and Anion for calcium iodide (c)#
07

Identify Cation and Anion in Calcium Iodide

The given salt is calcium iodide (CaI2). The cation is the calcium ion (Ca2+) and the anion is the iodide ion (I-). #Step 2: Determine Acid and Base for calcium iodide (c)#
08

Determine Acid and Base for Calcium Iodide Reaction

To form calcium iodide, the cation is contributed from a base containing calcium ions, such as calcium hydroxide (Ca(OH)2), and the anion comes from an acid containing the iodide ion, such as hydroiodic acid (HI). #Step 3: Write balanced formula equation for calcium iodide (c)#
09

Balanced Formula Equation for Calcium Iodide Reaction

Now we'll write the balanced equation for the reaction between calcium hydroxide and hydroiodic acid, producing calcium iodide and water. The balanced equation is: Ca(OH)2 + 2HI → CaI2 + 2H2O

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Most popular questions from this chapter

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide

A solution was prepared by mixing \(50.00 \mathrm{mL}\) of \(0.100 \mathrm{M}\) HNO_and \(100.00 \mathrm{mL}\) of \(0.200 \mathrm{M}\) HNO \(_{3}\). Calculate the molarity of the final solution of nitric acid.

Balance each of the following oxidation-reduction reactions by using the oxidation states method. a. \(\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{Mg}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{Co}^{3+}(a q)+\mathrm{Ni}(s) \rightarrow \mathrm{Co}^{2+}(a q)+\mathrm{Ni}^{2+}(a q)\) d. \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\)

When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of \(5.0 \mathrm{M}\) HCl is required to react completely with \(3.00 \mathrm{g}\) of magnesium?

Describe how you would prepare 2.00 L of each of the following solutions. a. \(0.250 \mathrm{M}\) NaOH from solid \(\mathrm{NaOH}\) b. \(0.250 M\) NaOH from \(1.00 M\) NaOH stock solution c. \(0.100 M K_{2} C r O_{4}\) from solid \(K_{2} C r O_{4}\) d. \(0.100 M K_{2} C r O_{4}\) from \(1.75 M K_{2} C r O_{4}\) stock solution
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