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Chapter 5: Problem 6

The following compounds are water-soluble. What ions are produced by each compound in aqueous solution? (a) \(\mathrm{KI}\) (c) \(\mathrm{K}_{2} \mathrm{HPO}_{4}\) (b) \(\mathrm{Mg}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}\) (d) NaCN

Short Answer

Expert verified
(a) K鈦� and I鈦�; (b) Mg虏鈦� and 2 CH鈧僀O鈧傗伝; (c) 2 K鈦� and HPO鈧劼测伝; (d) Na鈦� and CN鈦�.

Step by step solution

01

Analyze Compound KI

Potassium iodide ( KI ) is a simple ionic compound consisting of potassium ions ( K^+ ) and iodide ions ( I^- ). In aqueous solution, it dissociates completely into these ions.
02

Analyze Compound Mg(CH3CO2)2

Magnesium acetate ( Mg(CH_3CO_2)_2 ) is composed of magnesium ions ( Mg^{2+} ) and acetate ions ( CH_3CO_2^- ). When dissolved in water, it dissociates into one magnesium ion and two acetate ions per formula unit.
03

Analyze Compound K2HPO4

Dipotassium hydrogen phosphate ( K_2HPO_4 ) consists of potassium ions ( K^+ ) and hydrogen phosphate ions ( HPO_4^{2-} ). In aqueous solution, it dissociates into two potassium ions and one hydrogen phosphate ion.
04

Analyze Compound NaCN

Sodium cyanide ( NaCN ) is made up of sodium ions ( Na^+ ) and cyanide ions ( CN^- ). When dissolved, it dissociates into these ions in water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Water-Solubility
Water solubility is an important property of ionic compounds because it determines how well a substance dissolves in water. Many ionic compounds are composed of positive and negative ions held together by strong electrostatic forces. When they are introduced to water, these forces are overcome by the polar nature of water molecules.
Water molecules are polar, meaning they have a partial positive charge on one side and a partial negative charge on the other. This allows them to interact with charged ions of an ionic compound, surrounding them and pulling them apart.
  • Water breaks apart the ions in the compounds, allowing the ions to move freely.
  • The ability of a compound to dissolve in water depends on the strength of the forces between its ions compared to the strength of attraction between the ions and water molecules.
  • Potassium iodide and sodium cyanide are examples of highly water-soluble ionic compounds.
Dissociation in Aqueous Solution
Dissociation is the process whereby an ionic compound separates into its individual ions when dissolved in water. This is a crucial aspect for understanding reactions in aqueous solutions as it influences everything from conductive properties to reaction outcomes.
When an ionic compound like potassium iodide or sodium cyanide dissolves, it dissociates into ions. These ions are then free to move around in the solution.
  • For instance, in potassium iodide (KI), it splits into potassium ions ( K^+ ) and iodide ions ( I^- ).
  • Sodium cyanide (NaCN) breaks into sodium ions ( Na^+ ) and cyanide ions ( CN^- ).
  • This dissociation is not just a physical change but plays a fundamental role in chemical reactions that occur in liquid environments.
Potassium Iodide
Potassium iodide ( KI ) is a classic example of a water-soluble ionic compound. Its formula indicates that it contains potassium ions ( K^+ ) and iodide ions ( I^- ). In water, these ions separate completely, showcasing its solubility and the characteristic dissociation.
The complete dissociation means that KI can easily participate in chemical reactions in aqueous environments. It is often used in medical and photographic applications where its ionic characteristics facilitate different processes.
Potassium iodide is:
  • A good conductor of electricity when dissolved due to the free moving ions.
  • Useful in iodine supplementations due to its iodine content.
  • A reagent in various chemical experiments.
Sodium Cyanide
Sodium cyanide ( NaCN ) is another example of an ionic compound that dissociates fully in water. It breaks down into sodium ions ( Na^+ ) and cyanide ions ( CN^- ) when dissolved. This compound is crucial in certain industrial applications, particularly in the extraction of gold and silver where its easy dissociation is utilized.
Due to the cyanide ions, NaCN solutions can be highly reactive and need to be handled with care. The toxic nature of cyanide makes it both a potent reagent and a hazardous substance.
Some key points about sodium cyanide include:
  • It is highly soluble, enabling the free movement of its ions in water.
  • Its dissociation allows for its active use in industrial processes.
  • Caution is necessary due to its potential toxicity and impact on health and the environment.

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Most popular questions from this chapter

A The cancer chemotherapy drug cisplatin, \(\operatorname{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\) can be made by reacting (NH_) \(_{2} \mathrm{PtCl}_{4}\) with ammonia in aqueous solution. Besides cisplatin, the other product is \(\mathrm{NH}_{1} \mathrm{Cl}\) (a) Write a balanced equation for this reaction. (b) To obtain \(12.50 \mathrm{g}\) of cisplatin, what mass of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{PtCl}_{4}\) is required? What volume of \(0.125 \mathrm{M}\) \(\mathrm{NH}_{3}\) is required? (c) Cisplatin can react with the organic compound pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N},\) to form a new compound. $$\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}(\mathrm{aq})+x \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(\mathrm{aq}) \longrightarrow \mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\left(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\right)_{x}(\mathrm{s})$$ Suppose you treat \(0.150 \mathrm{g}\) of cisplatin with what you believe is an excess of liquid pyridine \((1.50 \mathrm{mL}\) \(d=0.979 \mathrm{g} / \mathrm{mL}) .\) When the reaction is complete, you can find out how much pyridine was not used by titrating the solution with standardized HCl. If 37.0 mL. of \(0.475 \mathrm{M} \mathrm{HCl}\) is required to titrate the excess pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) what is the formula of the unknown compound \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\left(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\right)_{x} ?\)

Write a balanced equation for the ionization of nitric acid in water.

Balance the following equations, and then write the net ionic equation. Show states for all reactants and products \((s, \ell, g, a q)\) (a) the reaction of silver nitrate and potassium iodide to give silver iodide and potassium nitrate (b) the reaction of barium hydroxide and nitric acid to give barium nitrate and water (c) the reaction of sodium phosphate and nickel(II) nitrate to give nickel(11) phosphate and sodium nitrate

(a) What is the pH of a 0.105 M HCl solution? (b) What is the hydrogen ion concentration in a solution with a pH of \(2.56 ?\) Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydrogen ion concentration in the solution? Is the solution acidic or basic? (d) \(A 10.0\) -mL. sample of \(2.56 \mathrm{M}\) HCl is diluted with water to \(250 .\) mL. What is the pH of the dilute solution?

What mass of \(\mathrm{Na}_{2} \mathrm{CO}_{3},\) in grams, is required for complete reaction with \(50.0 \mathrm{mL}\) of \(0.125 \mathrm{M} \mathrm{HNO}_{3} ?\) \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})+2 \mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow\) $$2 \mathrm{NaNO}_{3}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$$
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