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Chapter 4: Problem 19

Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound? Write the chemical equation for the ionization of HCOOH.

Short Answer

Expert verified
The solutes present in an aqueous solution of formic acid (HCOOH) are H+ and HCOO- ions. The chemical equation for the ionization of HCOOH is: HCOOH \(\rightleftharpoons\) H+ + HCOO-

Step by step solution

01

Identify the ions present in formic acid

Formic acid (HCOOH) is a weak acid, and when it ionizes in water, it will lose one hydrogen ion (H+) and form a formate ion (HCOO-). So the solutes present in an aqueous solution of formic acid are H+ and HCOO- ions.
02

Write the chemical equation for the ionization of formic acid

Now that we have identified the ions present in formic acid, we can write the equation for its ionization. Since it's a weak electrolyte, we will use a double arrow to indicate the partial ionization. The chemical equation for the ionization of formic acid (HCOOH) in water is: HCOOH \(\rightleftharpoons\) H+ + HCOO-

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Most popular questions from this chapter

(a) How many grams of solid silver nitrate would you need to prepare \(200.0 \mathrm{~mL}\) of a \(0.150 \mathrm{M} \mathrm{AgNO}_{3}\) solution? (b) An experiment calls for you to use \(100 \mathrm{~mL}\) of \(0.50 \mathrm{MHNO}_{3}\) solution. All you have available is a bottle of \(3.6 \mathrm{M} \mathrm{HNO}_{3}\). How many milliliters of the \(3.6 \mathrm{M} \mathrm{HNO}_{3}\) solution and of water do you need to prepare the desired solution?

Consider the following reagents: zinc, copper, mercury (density \(13.6 \mathrm{~g} / \mathrm{mL}\) ), silver nitrate solution, nitric acid solution. (a) Given a \(500-\mathrm{mL}\) Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?

True or false: (a) Oxidation can occur without oxygen. (b) Oxidation can occur without reduction.

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of \(1.049 \mathrm{~g} / \mathrm{mL}\) at \(25^{\circ} \mathrm{C}\). Calculate the molarity of a solution of acetic acid made by dissolving \(20.00 \mathrm{~mL}\) of glacial acetic acid at \(25^{\circ} \mathrm{C}\) in enough water to make \(250.0 \mathrm{~mL}\) of solution.

Suppose you have \(5.00 \mathrm{~g}\) of powdered magnesium metal, \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) potassium nitrate solution, and \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) silver nitrate solution. (a) Which one of the solutions will react with the magnesium powder? (b) What is the net ionic equation that describes this reaction? (c) What volume of solution is needed to completely react with the magnesium? (d) What is the molarity of the \(\mathrm{Mg}^{2+}\) ions in the resulting solution?
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