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Chapter 6: Problem 69

Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid \(\left[\mathrm{HClO}_{4}(a q)\right]\) and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid

Short Answer

Expert verified
The balanced formula equations for the given acid-base reactions are: a. KOH(aq) + HNO₃(aq) -> KNO₃(aq) + H₂O(l) b. Ba(OH)₂(aq) + 2HCl(aq) -> BaCl₂(aq) + 2H₂O(l) c. 3HClO₄(aq) + Fe(OH)₃(s) -> Fe(ClO₄)₃(aq) + 3H₂O(l) d. AgOH(s) + HBr(aq) -> AgBr(s) + H₂O(l) e. Sr(OH)₂(aq) + 2HI(aq) -> SrI₂(aq) + 2H₂O(l)

Step by step solution

01

Write chemical formulas

Write the chemical formulas of reactants and products: Potassium hydroxide (aqueous): KOH(aq) Nitric acid: HNO₃(aq) The products for an acid-base reaction are salt and water.
02

Balance the equation

Write an unbalanced equation and then balance it: KOH(aq) + HNO₃(aq) -> KNO₃(aq) + H₂O(l) The equation is already balanced with coefficients 1 for all the reactants and products. #b. barium hydroxide (aqueous) and hydrochloric acid#
03

Write chemical formulas

Write the chemical formulas of reactants and products: Barium hydroxide (aqueous): Ba(OH)₂(aq) Hydrochloric acid: HCl(aq)
04

Balance the equation

Write an unbalanced equation and then balance it: Ba(OH)₂(aq) + HCl(aq) -> BaCl₂(aq) + H₂O(l) Balance the equation: Ba(OH)₂(aq) + 2HCl(aq) -> BaCl₂(aq) + 2H₂O(l) #c. perchloric acid and solid iron(III) hydroxide #
05

Write chemical formulas

Write the chemical formulas of reactants and products: Perchloric acid: HClO₄(aq) Solid Iron(III) hydroxide : Fe(OH)₃(s)
06

Balance the equation

Write an unbalanced equation and then balance it: HClO₄(aq) + Fe(OH)₃(s) -> Fe(ClO₄)₃(aq) + H₂O(l) Balance the equation: 3HClO₄(aq) + Fe(OH)₃(s) -> Fe(ClO₄)₃(aq) + 3H₂O(l) #d. solid silver hydroxide and hydrobromic acid#
07

Write chemical formulas

Write the chemical formulas of reactants and products: Solid silver hydroxide: AgOH(s) Hydrobromic acid: HBr(aq)
08

Balance the equation

Write an unbalanced equation and then balance it: AgOH(s) + HBr(aq) -> AgBr(s) + H₂O(l) The equation is already balanced with coefficients 1 for all the reactants and products. #e. aqueous strontium hydroxide and hydroiodic acid#
09

Write chemical formulas

Write the chemical formulas of reactants and products: Aqueous strontium hydroxide: Sr(OH)₂(aq) Hydroiodic acid: HI(aq)
10

Balance the equation

Write an unbalanced equation and then balance it: Sr(OH)₂(aq) + HI(aq) -> SrI₂(aq) + H₂O(l) Balance the equation: Sr(OH)₂(aq) + 2HI(aq) -> SrI₂(aq) + 2H₂O(l)

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Most popular questions from this chapter

In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing \(10.0,25.0,50.0,75.0,\) and \(100 .\) ppm of copper from a commercially produced 1000.0 -ppm solution? Assume each solution has a final volume of \(100.0 \mathrm{mL}\). (See Exercise 123 for definitions.)

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{KMnO}_{4}\) f. \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) b. \(\mathrm{NiO}_{2}\) g. \(\mathrm{XeOF}_{4}\) c. \(\mathrm{Na}_{4} \mathrm{Fe}(\mathrm{OH})_{6}\) h. \(\mathrm{SF}_{4}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) i. \(\mathrm{CO}\) e. \(\mathrm{P}_{4} \mathrm{O}_{6}\) j. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

Many oxidation-reduction reactions can be balanced by inspection. Try to balance the following reactions by inspection. In each reaction, identify the substance reduced and the substance oxidized. a. \(\mathrm{Al}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{CH}_{4}(g)+\mathrm{S}(s) \rightarrow \mathrm{CS}_{2}(l)+\mathrm{H}_{2} \mathrm{S}(g)\) c. \(C_{3} H_{8}(g)+O_{2}(g) \rightarrow C O_{2}(g)+H_{2} O(l)\) d. \(\mathrm{Cu}(s)+\mathrm{Ag}^{+}(a q) \rightarrow \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\)

How would you prepare 1.00 L of a \(0.50-M\) solution of each of the following? a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from "concentrated" \((18 \mathrm{M})\) sulfuric acid b. HCl from "concentrated" (12 M) reagent c. \(\mathrm{NiCl}_{2}\) from the salt \(\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. HNO_ from "concentrated" (16 M) reagent e. Sodium carbonate from the pure solid

In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A \(0.256-\mathrm{g}\) sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it had a mass of 0.308 g. A second sample of 0.416 g of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was 0.145 g. a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.
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