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# Calculations with Equilibrium

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What copper (II) nitrate is dissolved in dilute hydrochloric acid the following is established.

Cu(H2))6^2+(aq) + 4Cl-(aq) <---> CuCl4^2-(aq) +6H2O(l)

(a) Write the equilibrium constant expression for this system.
(b) Three test tubes are set up, each containing some of the equilibrium mixture. Each of the tubes is treated as described below. In each case state the equilibrium will shift.

*see attached file for chart

Consider the following acid-base equilibrium:
H2S(aq) + H2O(l) <---> HS-(aq) + H3O+(aq)
(a) Identify the conjugate acid-base pairs in this equilibrium.

*see attached file for chart

The value of the equilibrium constant for the above reaction is 5.7 x 10^-8

(b) How will the concentration of H2S compare to the concentration of the HS- ion in any soluation in which this equilibrium occurs?
(c) The hydrogensulfide ion (HS-) produced in the equilibrium above can also react with water in an acid-base reaction. Write the equation for this reaction in the space below.

https://brainmass.com/chemistry/general-chemistry/calculations-with-equilibrium-549039

#### Solution Summary

Copper(II) nitrate dissolved in diluted hydrochloric acid is examined.

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## Calculate equilibrium partial pressure

The heterogeneous equilibrium process
C(s) + CO2(g) f/r 2 CO(g)

At 700 deg. C. the total pressure in this system is 4.71 atem. The equilibrium constant is 1.52, calculate the equilibrium partial pressures of CO2 and CO.

PCO2=? atm
PCO=? atm

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