5. When substances form solutions with water, they always dissolve, but sometimes they also dissociate. (i) Explain thedifference between the terms dissolve and dissociate. Then, (ii) explain why ionic substances must dissociate todissolve in water while covalent substances do not have to dissociate to dissolve in water.

Interpretation: We have to explain the difference between dissolve and dissociate.

Answered: 5. When substances form solutions with…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 20CR

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Similar questions

When substances form solutions with water, they always dissolve, but sometimes they also dissociate. (i) Explain the difference between the terms dissolve and dissociate. Then, (ii) explain why ionic substances must dissociate to dissolve in water while covalent substances DO NOT have to dissociate to dissolve in water.
Explain the difference between the terms dissolve and dissociate. Then, (ii) explain why ionic substances must dissociate to dissolve in water while covalent substances do not have to dissociate to dissolve in water.
(b) (i) Draw the Lewis structure of methanol, CH3OH(ℓ). (ii) Show with a simple diagram how methanol dissolves in water. Explain.
Ammonium chloride, NH4Cl, is a very soluble salt in water.(a) Draw the Lewis structures of the ammonium and chlorideions. (b) Is there an N—Cl bond in solid ammonium chloride?(c) If you dissolve 14 g of ammonium chloride in 500.0 mLof water, what is the molar concentration of the solution?(d) How many grams of silver nitrate do you need to add tothe solution in part (c) to precipitate all of the chloride as silverchloride?
A solution is formed from dissolving 1 mole of Al(NO3)3 into enough water to have a total volume of 1 liter. The heat of the solution from this dissolution process was found to be 175 kJ/mol. if the lattice energy for the aluminum nitrate is 5960 kJ/mol in the heat of the hydration for the aluminum (III) cation is -4606 kJ/mol What is the heat of hydration for the nitrate ion in kJ/mol?
Under the concepts of bond polarity and solubility, why is it that ethanol (rubbing alcohol) and water are miscible, but oil and water are immiscible?
Why are most solid ionic compounds electrically nonconductive, whereas aqueous solutions of ionic compounds are good conductors? Would you expect a liquid (molten) ionic compound to be electrically conductive or nonconductive?
100-g of MgSO4*7H2O is dissolved in 900 g of water. If the density of the solution is 1.047 g/mL, what is the formality of MgSO4 in the solution?
a) What mass of strontium nitrate (Sr(NO3)2) would be required to prepare 2.000 L of a 0.0180 M aqueous solution of this salt? (b) Calculate the mass percent of Sr(NO3)2 in this solution, assuming the density of the solution is 1.000 kg/L. c.) A 15.0 g sample of anhydrous sodium sulfate, Na2SO4, is dissolved in 4.83 L of water. The molar mass of sodium sulfate is 142.1 g/mol. Use the equation given to calculate the molality (m) of the solution, in mol/kg.For this situation, assume the density of water is 1.00 g/mL.
Describe how you could separate and purify compound A from a mixture of two neutral compounds (A and B) when A comprises 95% of the total and B the other 5% of the total. Assume that A and B have similar polarities.
Which statement about the properties of barium chloric and mercury(II) chloride is correct? (A) BaCl₂ has a higher melting point than HgCl₂. (B) BaCl₂ has a higher solubility in nonpolar solvents than HgCl₂. (C) BaCl₂ has a higher vapor pressure than HgCl₂. (D) Molten BaCl₂ has a lower electrical conductivity than molten HgCl2.
Calculate the molarity of the following solution: 0.800 g NaOH (s) dissolved in distilled water, to give 500.0 mL of solution. Calculate the molarity of the following solution: 10.00 mL of 0.500 M NaOH (aq), diluted to 250.0 mL of solution with distilled water.

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