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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 the hydrogen ion (H⁺) and the formate ion (HCOO⁻). The ionization equation for formic acid is: \( HCOOH_{(aq)} \rightleftharpoons H^+_{(aq)} + HCOO^-_{(aq)} \).

Step by step solution

01

Identify the ions produced from the dissociation of formic acid

Let's first identify the ions formed when HCOOH ionizes. Formic acid, HCOOH, is a weak acid that partially dissociates into a hydrogen ion (H⁺) and a formate ion (HCOO⁻).
02

Write the chemical equation for the ionization of HCOOH

Now we can write the chemical equation for the ionization of formic acid in water: \( HCOOH_{(aq)} \rightleftharpoons H^+_{(aq)} + HCOO^-_{(aq)} \) In this equation, the double arrow (\(\rightleftharpoons\)) indicates that the reaction is reversible, meaning that the ions formed can also recombine to form formic acid. This reversibility is a property of weak electrolytes, as they do not dissociate completely in water. In conclusion, the solutes present in an aqueous solution of formic acid (HCOOH) are the hydrogen ion (H⁺) and the formate ion (HCOO⁻), as shown in the ionization equation: \( HCOOH_{(aq)} \rightleftharpoons H^+_{(aq)} + HCOO^-_{(aq)} \).

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Most popular questions from this chapter

The distinctive odor of vinegar is due to aceticacid, \(\mathrm{CH}_{3} \mathrm{COOH},\) which reacts with sodium hydroxide according to: $$\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NaOH}(a q) \longrightarrow_{\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaCH}_{3} \mathrm{COO}(a q)}$$ If 3.45 \(\mathrm{mL}\) of vinegar needs 42.5 \(\mathrm{mL}\) of 0.115 \(\mathrm{M} \mathrm{NaOH}\) to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00 -qt sample of this vinegar?

(a) You have a stock solution of 14.8 \(\mathrm{M} \mathrm{NH}_{3}\) . How many milliliters of this solution should you dilute to make 1000.0 \(\mathrm{mL}\) of 0.250 \(\mathrm{MNH}_{3} ?(\mathbf{b})\) you take a 10.0 -mL portion of the stock solution and dilute it to a total volume of \(0.500 \mathrm{L},\) what will be the concentration of the final solution?

Glycerol, \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3},\) is a substance used extensively in the manufacture of cosmetic s, foodstuffs, antifreeze, and plastics. Glycerol is a water-soluble liquid with a density of 1.2656 \(\mathrm{g} / \mathrm{mL}\) at \(15^{\circ} \mathrm{C}\) . Calculate the molarity of a solution of glycerol made by dissolving 50.000 \(\mathrm{mL}\) glycerol at \(15^{\circ} \mathrm{C}\) in enough water to make 250.00 \(\mathrm{mL}\) of solution.

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) \(\mathrm{NaCH}_{3} \mathrm{COO}\) and \(\mathrm{HCl},\) (b) \(\mathrm{KOH}\) and \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2},(\mathbf{c}) \mathrm{Na}_{2} \mathrm{S}\) and \(\mathrm{CdSO}_{4}\) .

A solution of 100.0 \(\mathrm{mL}\) of 0.200 \(\mathrm{M} \mathrm{KOH}\) is mixed with a solution of 200.0 \(\mathrm{mL}\) of 0.150 \(\mathrm{M} \mathrm{MiSO}_{4}\) . (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?
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