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Chapter 4: Q4.5P (page 140)

What occurs on the molecular level when an ionic compound dissolves in water?

Short Answer

Expert verified

When an ionic compound dissolves in water it becomes dissociated polar part gets attracted toward the water molecule.

Step by step solution

01

Step 1: Identification of the dissociation of ionic compounds

When ionic compounds dissolve in water, it dissociates into ions by breaking their ionic bond when the strong electrostatic force of attraction generates by the molecules of water and ionic compound since both the ionic and water molecules are polar in nature and the attraction between the ions and water molecules is much stronger than a compound itself.

02

Determine the solubility of ionic compounds in water molecules

Now the molecules of water surround the ions of the ionic compounds to stabilize the ion in such a way that the negative charge of water surrounds positive ions and the negative part surrounds the positive ions as shown in fig given below:

This states that the ionic compound dissolve in the water molecules.

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Most popular questions from this chapter

Mixtures of CaCl₂ and NaCl are used to melt ice on roads. A dissolved 1.9348-g sample of such a mixture was analyzed by using excess Na₂C₂O₄ to precipitate the Ca²⁺ as CaC₂O₄. The CaC₂O₄ was dissolved in sulfuric acid, and the resulting H₂C₂O₄ was titrated with 37.68mL of 0.1019M KMnO₄ solution.

(a) Write the balanced net ionic equation for the precipitation reaction.

(b) Write the balanced net ionic equation for the titration reaction. (See Sample Problem 4.11.)

(c) What is the oxidizing agent?

(d) What is the reducing agent?

(e) Calculate the mass percent of CaCl₂ in the original sample.

Iron reacts rapidly with chlorine gas to form a reddish brown, ionic compound (A), which contains iron in the higher of its two common oxidation states. Strong heating decomposes compound A to compound B, another ionic compound, which contains iron in the lower of its two oxidation states. When compound A is formed by the reaction of 50.6 g of Fe and 83.8 g of Cl₂ and then heated, how much compound B forms?

Question: How many moles ofions are present in the following aqueous solutions?

(a) 1.4 mL of 0.75 M hydrobromic acid

(b) 2.47 mL of 1.98 M hydriodic acid

(c) 395 mL of 0.270 M nitric acid

There are various methods for finding the composition of an alloy (a metal-like mixture). Show that calculating the mass % of Mg in a magnesium-aluminum alloy (d = 2.40 g/cm³) gives the same answer (within rounding) using each of these methods:

(a) $a 0.263 - gsample of alloy (d of Mg = 1.74 g / {cm}^{3}; dofAl = 2.70 g / {cm}^{3});$

(b) an identical sample reacting with excess aqueous HCl forms $1.38 x 10^{- 2} mol of H_{2};$

(c) an identical sample reacting with excess O₂forms 0.483 g of oxide.

Question: Over time, as their free fatty acid (FFA) content increases, edible fats and oils become rancid. To measure rancidity, the fat or oil is dissolved in ethanol, and any FFA present is titrated with KOH dissolved in ethanol. In a series of tests on olive oil, a stock solution of 0.050 M ethanolic KOH was prepared at 25⁰C , stored at 0^oC, and then placed in a 100-mL buret to titrate any oleic acid $[{CH}_{3} {({CH}_{2})}_{7} CH = CH {({CH}_{2})}_{7} COOH]$ present in the oil. Each of four 10.00-g samples of oil took several minutes to titrate: the first required 19.60 mL, the second 19.80 mL, and the third and fourth 20.00 mL of the ethanolic KOH.

(a) What is the apparent acidity of each sample, in terms of mass % of oleic acid? (Note: As the ethanolic KOH warms in the buret, its volume increases by a factor of .)

(b) Is the variation in acidity a random or systematic error? Explain.

(c) What is the actual acidity? How would you demonstrate this?

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