4) Use your results from Part 3 to explain what you observed with a balanced che

Question

4) Use your results from Part 3 to explain what you observed with a balanced chemical 5) Use your results from Part 4 to explain what you observed with a balanced chemical equation 6) In Part 5 you should now be able to tell whether CoCl2(H20)2 + 4 HO Co(HO2 CH is an exothermic or endothermic reaction. Rewrite the balanced equilibrium equation to show how the equilibrium responds to changes in temperature (add the word 'heat to the left or right) Explain. 7) Use your results from Part 6 to show how you might increase or decrease the solubility of sodium chloride in water by adding ions or changing temperature. Is the dissolving (dissolution reaction) of NaCl in water exothermic or endothermic? How is the solubility of NaCl affected by the presence of HCi? Write a balanced chemical equation to show what happened 8) Briefy explain how the test performed in tube 3 rules out the formation of Ca(OH)2 in Part 7 Explain, using balanced equilibrium equation(S), what happens in tube 3. What is the identity of the precipitate formed in Step 6? 147

Explanation / Answer

The following is the equilibrium equation :

    Co(H2O)62+ + 4 Cl- <=> CoCl42- + 6 H2O

    The Co(H2O)62+ is pink in color, and the CoCl42- is blue in color.

    The above reaction is endothermic , so adding heat while reaction causes the equilibrium constant to shift to the right. This makes the solution blue.

i.e. Co(H2O)62+ + 4 Cl- + heat <=> CoCl42- + 6 H2O . Equilibrium constant to shift to the right.  

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