Assume the following process is at equilibrium. NaCl(s) <----->Na+(aq) + Cl–(aq) deltaH0> 0 How will the following changes influence this equilibrium? Indicate whether each change will cause additional NaCl to dissolve, will cause NaCl to precipitate, or will have no influence on the equilibrium. __________ (a) The temperature is increased. __________ (b) The pH is decreased. __________ (c) MgCl2 is added to the reaction vessel.
Assume the following process is at equilibrium. NaCl(s) <----->Na+(aq) + Cl–(aq) deltaH0> 0 How will the following changes influence this equilibrium? Indicate whether each change will cause additional NaCl to dissolve, will cause NaCl to precipitate, or will have no influence on the equilibrium. __________ (a) The temperature is increased. __________ (b) The pH is decreased. __________ (c) MgCl2 is added to the reaction vessel.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.11PAE
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Assume the following process is at equilibrium.
NaCl(s) <----->Na+(aq) + Cl–(aq) deltaH0> 0
How will the following changes influence this equilibrium? Indicate whether each change will cause additional NaCl to dissolve, will cause NaCl to precipitate, or will have no influence on the equilibrium.
__________ (a) The temperature is increased.
__________ (b) The pH is decreased.
__________ (c) MgCl2 is added to the reaction vessel.
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