Question

In: Chemistry

1.) Explain the following observations in terms of shifting equilibria by Le Chatelier's Principle. Write the...

1.) Explain the following observations in terms of shifting equilibria by Le Chatelier's Principle. Write the equation for the equilibrium involved in each case.

a.) barium chromate, BaCrO4, is insoluble in basic solution but dissolves readily in acidic solution.

b.) The addition of NaOH to the iron (III)- thiocyanate equilibrium causes the red color to disappear and a rust colored precipitate to form.

c.) The solubility of lead chloride, PbCl2, in 0.10 M HCl is much lower than in pure water.

d.) Limestone, CaCO3, is an insoluble salt but will dissolve in acid.

e.) For part C, how does the rate of the reaction vary as the temperature is increased? Explain.

Solutions

Expert Solution

(a) BaCrO4 + H2SO4 BaSO4 + H2CrO4 (chromic acid)

Here a stable product chromic acid is formed therefore it is not in equilibrium condition,it is a irreversible reaction

(b) [Fe(SCN)(H2O)5]+2 + NaOH   Fe+3(aq) + NaSCN (colourless) + H2O

In this equation Fe+3(aq) slowly converted into Fe2O3 that is known as rust and the red colour disappear

(c) PbCl2 + HCl(aq) PbCl2 + Cl- + H+

     PbCl2 + H2O 2HCl + Pb+2(aq)

The solubility of PbCl2 is very low in HCl because no further chemical species formed in this reaction and only the concentration of chloride ions increases but in case of water a third chemical species HCl is formed that increase the solubility.

(d) CaCO3 + H2SO4 CaSO4 + H2O + CO2

It dissolve in H2SO4 completely to form CaSO4 & evolve CO2 gas.

(e) There is no effect of temperature on the reaction (c) because there is no further chemical formed in this reaction.


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