The atomic radii of a divalent cation and a monovalent anion are 0.50 nm and 0.138 nm, respectively. (a) Calculate the force of attraction between these two ions at their equilibrium interionic separation (i.e., when the ions just touch one another). N (b) What is the force of repulsion at this same separation distance? N

The atomic radii of a divalent cation and a monovalent anion are 0.50 nm and 0.138 nm, respectively. (a) Calculate the force of attraction between these two ions at their equilibrium interionic separation (i.e., when the ions just touch one another). N (b) What is the force of repulsion at this same separation distance? N

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter6: Solutions And Colloids

Section: Chapter Questions

Problem 6.66P: 6-66 What gives nanotubes their unique optical and electrical properties?

See similar textbooks

Similar questions

7. Calculate the atomic concentration (in cm-³) and density (in g/cm³) of the following, using their lattice constants, atomic weights, and Avogadro's number: (a) Si (lattice constant = 5.43 Å; atomic weight = 28.1) (b) Ge (lattice constant = 5.66 Å; atomic weight = 72.6) (c) GaAs (lattice const. = 5.65 Å; atomic weightGa = 69.7; atomic weight As = 74.9) (d) InP (lattice constant = 5.87 Å; atomic weightn = 114.8; atomic weightp = 31) %3D %3D %3D %3D
3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBr is -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number.…
Calculate the atomic concentration (in cm¯³) and density (in g/cm³) of the following, using their lattice constants, atomic weights, and Avogadro's number: (a) Si (lattice constant = 5.43 Å; atomic weight = 28.1) (b) Ge (lattice constant = 5.66 Ä; atomic weight = (c) GaAs (lattice const. = 5.65 Å; atomic weightGa = 69.7; atomic weight As = 74.9) 72.6) %3D %3D %3D
Water is a polar solvent while carbon tetrachloride (CCl4) is a nonpolar solvent. Which solvent would you choose to dissolve FeSO4? Justify your choice.
The atomic radii of a divalent cation and a monovalent anion are 0.15 nm and 0.143 nm, respectively. (a) Calculate the force of attraction between these two ions at their equilibrium interionic separation (i.e., when the ions just touch one another). i ! N (b) What is the force of repulsion at this same separation distance? N i
3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBris -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number. (c) Would you expect this compound to be soluble in water? Why/Why not? Calculate anything you need in order to figure this out, and explain your answer.
What is the electrostatic force of repulsion for two protons separated by 75 pm.
(a) What is the molarity of a solution made by dissolving 10 moles of sucrose, C12H22O11, in 10L of water? (b) How much boric acid (H3BO3), in grams, is needed to be dissolves in 300.g of water to make a 1.50m aqueous H3BO3 solution? The molar mass of H3BO3 is 61.83g/mol. (c) How much aluminum sulfate (Al2(SO4)3) in moles, is needed to be dissolved in 500g of water to make a 1.0m aqueous Al2(SO4)3 solution?
12. Two charged spheres 10 cm apart attract each other with a force of 3.0 x 10-6N. What force results from each of the following changes, considered separately? (a) Both charges are doubled and the distance remains the same. F = Kqi9z 1.2x10-5 (b) The separation is increased to 30 cm. 3.3x10-7 pre dissolved in 875 g of H20, what will be the boiling point of
(a) Use the following data to calculate the combined heat ofhydration for the ions in sodium acetate (NaC₂H₃O₂):ΔH(lattice)=763 kJ/mol ΔH(soln)=17.3 kJ/mol(b) Which ion contributes more to the answer to part (a)? Why?
5. (a) The melting point of ammonia (NH3) is higher than that of methane (CH4) and yet these molecules have comparable molecular mass. Why does NH3 have a higher melting point than CH4? Explain in terms of intermolecular forces. (b) Predict the solubility of HF, HCl and Cl2 in water and explain your answer.
State a reason of the following statement: (i) Soap do not work in hard water. (ii) The use of the sweetener aspartame is limited to cold foods and drinks.