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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) + HNO鈧�(aq) -> KNO鈧�(aq) + H鈧侽(l) b. Ba(OH)鈧�(aq) + 2HCl(aq) -> BaCl鈧�(aq) + 2H鈧侽(l) c. 3HClO鈧�(aq) + Fe(OH)鈧�(s) -> Fe(ClO鈧�)鈧�(aq) + 3H鈧侽(l) d. AgOH(s) + HBr(aq) -> AgBr(s) + H鈧侽(l) e. Sr(OH)鈧�(aq) + 2HI(aq) -> SrI鈧�(aq) + 2H鈧侽(l)

Step by step solution

01

Write chemical formulas

Write the chemical formulas of reactants and products: Potassium hydroxide (aqueous): KOH(aq) Nitric acid: HNO鈧�(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) + HNO鈧�(aq) -> KNO鈧�(aq) + H鈧侽(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)鈧�(aq) Hydrochloric acid: HCl(aq)
04

Balance the equation

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

Write chemical formulas

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

Balance the equation

Write an unbalanced equation and then balance it: HClO鈧�(aq) + Fe(OH)鈧�(s) -> Fe(ClO鈧�)鈧�(aq) + H鈧侽(l) Balance the equation: 3HClO鈧�(aq) + Fe(OH)鈧�(s) -> Fe(ClO鈧�)鈧�(aq) + 3H鈧侽(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) + H鈧侽(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)鈧�(aq) Hydroiodic acid: HI(aq)
10

Balance the equation

Write an unbalanced equation and then balance it: Sr(OH)鈧�(aq) + HI(aq) -> SrI鈧�(aq) + H鈧侽(l) Balance the equation: Sr(OH)鈧�(aq) + 2HI(aq) -> SrI鈧�(aq) + 2H鈧侽(l)

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Most popular questions from this chapter

A sample may contain any or all of the following ions: \(\mathrm{Hg}_{2}^{2+}\) \(\mathrm{Ba}^{2+},\) and \(\mathrm{Mn}^{2+}\) a. No precipitate formed when an aqueous solution of \(\mathrm{NaCl}\) was added to the sample solution. b. No precipitate formed when an aqueous solution of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) was added to the sample solution. c. A precipitate formed when the sample solution was made basic with NaOH. Which ion or ions are present in the sample solution?

A solution is prepared by dissolving \(10.8 \mathrm{g}\) ammonium sulfate in enough water to make \(100.0 \mathrm{mL}\) of stock solution. A \(10.00-\) mL sample of this stock solution is added to \(50.00 \mathrm{mL}\) of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

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

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.)

A stock solution containing \(\mathrm{Mn}^{2+}\) ions was prepared by dissolving 1.584 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution: For solution \(A, 50.00 \mathrm{mL}\) of stock solution was diluted to \(1000.0 \mathrm{mL}\) For solution \(B, 10.00 \mathrm{mL}\) of solution \(A\) was diluted to \(250.0 \mathrm{mL}\). For solution \(C, 10.00 \mathrm{mL}\) of solution \(B\) was diluted to \(500.0 \mathrm{mL}\). Calculate the concentrations of the stock solution and solutions \(A, B,\) and \(C .\)
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