Concept explainers
The (aq) designation listed after a solute indicates the process of hydration. Using KBr(aq) and C2H5OH(aq) as your examples, explain the process of hydration for soluble ionic compounds and for soluble covalent compounds.
Interpretation: The process of hydration for soluble ionic compounds and soluble covalent compounds with
Concept Introduction: When an ionic compound is dissolved in water, the positive ends of the water molecules are attracted to the negative charged ions and that negative ends are attracted to the positive charged ions. This process is called as hydration.
Answer to Problem 1RQ
Answer
Soluble ionic compounds have to tendency to breakup into their positive and negatively charged ions when they are dissolved into solution.
In
In the hydration process for ions, the partial negative end of the polar water molecules surrounds and stabilizes the cations in the solution. The water molecules present here would align themselves in such a way that the oxygen end of water aligns with the
In the case of
This is assumption when an aqueous solution (aq) is placed after an ionic compound.
Soluble covalent compounds are that compound that doesn’t have to tendency to break into ions when they are dissolved in solution.
Consider,
The hydration process for polar covalent solutes takes place when the covalent solutes and solvents align themselves such that their opposite charged parts attract each other.
The partial negative end of
This is the hydration process for polar covalent compounds. This is assumption when an aqueous solution (aq) is placed after an ionic compound.
It is difficult to predict the partial negative ends and partial positive ends of polar covalent compounds.
Explanation of Solution
Explanation
To explain the process of hydration in soluble ionic compounds
The process of hydration can be defined as dissolution of ionic compound in water, where
the positive ends of the water molecules are attracted to the negative charged ions and that negative ends are attracted to the positive charged ions.
When an ionic compound that is soluble in water can break apart into their ions upon dissolution such ionic compounds are called as soluble ionic compounds.
Taking the example of
The dissolution of
The equation can be given as,
In the hydration process for ions, the partial negative end of the polar water molecules surrounds and stabilizes the cations in the solution. The water molecules present here would align themselves in such a way that the oxygen end of water aligns with the
In the case of
This is assumption when an aqueous solution (aq) is placed after an ionic compound.
The separation of ions that are placed in solution is surrounded by the water that is permitable. There is an enthalpy change. The enthalpy change for this process is called as hydration enthalpy.
When a compound is made to get soluble in water, there is no break apart into their ions upon dissolution such ionic compounds are called as soluble covalent compounds.
To explain the process of hydration in soluble covalent compound
Soluble covalent compounds are that compound that doesn’t have to tendency to break into ions when they are dissolved in solution.
Consider,
The hydration process for polar covalent solutes takes place when the covalent solutes and solvents align themselves such that their opposite charged parts attract each other.
The partial negative end of
This is the hydration process for polar covalent compounds. This is assumption when an aqueous solution (aq) is placed after an ionic compound.
It is difficult to predict the partial negative ends and partial positive ends of polar covalent compounds.
The concept of hydration of soluble ionic and covalent compounds were explained with
Want to see more full solutions like this?
Chapter 4 Solutions
Chemistry with Access Code, Hybrid Edition
- The emission data in cps displayed in Table 1 is reported to two decimal places by the chemist. However, the instrument output is shown in Table 2. Table 2. Iron emission from ICP-AES Sample Blank Standard Emission, cps 579.503252562 9308340.13122 Unknown Sample 343.232365741 Did the chemist make the correct choice in how they choose to display the data up in Table 1? Choose the best explanation from the choices below. No. Since the instrument calculates 12 digits for all values, they should all be kept and not truncated. Doing so would eliminate significant information. No. Since the instrument calculates 5 decimal places for the standard, all of the values should be limited to the same number. The other decimal places are not significant for the blank and unknown sample. Yes. The way Saman made the standards was limited by the 250-mL volumetric flask. This glassware can report values to 2 decimal places, and this establishes our number of significant figures. Yes. Instrumental data…arrow_forwardSteps and explanation pleasearrow_forwardSteps and explanation to undertand concepts.arrow_forward
- Nonearrow_forward7. Draw a curved arrow mechanism for the following reaction. HO cat. HCI OH in dioxane with 4A molecular sievesarrow_forwardTry: Convert the given 3D perspective structure to Newman projection about C2 - C3 bond (C2 carbon in the front). Also, show Newman projection of other possible staggered conformers and circle the most stable conformation. Use the template shown. F H3C Br Harrow_forward
- Nonearrow_forward16. Consider the probability distribution p(x) = ax", 0 ≤ x ≤ 1 for a positive integer n. A. Derive an expression for the constant a, to normalize p(x). B. Compute the average (x) as a function of n. C. Compute σ2 = (x²) - (x)², the variance of x, as a function of n.arrow_forward451. Use the diffusion model from lecture that showed the likelihood of mixing occurring in a lattice model with eight lattice sites: Case Left Right A B C Permeable Barrier → and show that with 2V lattice sites on each side of the permeable barrier and a total of 2V white particles and 2V black particles, that perfect de-mixing (all one color on each side of the barrier) becomes increasingly unlikely as V increases.arrow_forward
- 46. Consider an ideal gas that occupies 2.50 dm³ at a pressure of 3.00 bar. If the gas is compressed isothermally at a constant external pressure so that the final volume is 0.500 dm³, calculate the smallest value Rest can have. Calculate the work involved using this value of Rext.arrow_forwardNonearrow_forward2010. Suppose that a 10 kg mass of iron at 20 C is dropped from a heigh of 100 meters. What is the kinetics energy of the mass just before it hits the ground, assuming no air resistance? What is its speed? What would be the final temperature of the mass if all the kinetic energy at impact is transformed into internal energy? The molar heat capacity of iron is Cpp = 25.1J mol-¹ K-1 and the gravitational acceleration constant is 9.8 m s¯² |arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning