Many thanks! You're dealing with a double replacement reaction in which two soluble ionic compounds react to form an insoluble solid that precipitates out of the aqueous solution. Now, notice that you need 2 moles of sodium hydroxide for every 1 mole of copper II nitrate that takes part in the reaction. To get the complete ionic equation , rewrite the soluble ionic compounds as cations and anions. Now, in order to get the net ionic equation , you must eliminate spectator ions , i.
Stefan V. Mar 22, Explanation: You're dealing with a double replacement reaction in which two soluble ionic compounds react to form an insoluble solid that precipitates out of the aqueous solution. Related questions Question fee Question c5c Question 19eb9. Explain the steps and write the corresponding chemical equation for reaction two. The beaker now contains copper nitrate Cu NO3 2. Sodium nitrate NaNO3 was also yielded from the reaction.
Explain the steps and write down the corresponding chemical reaction for reaction three. The heat from this process will dehydrate the gelatinous copper hydroxide Cu OH 2 form Black flakes of copper oxide, CuO. Use the warm water H2O to perform many washes of the copper oxide CuO.
Explain the steps and write down the corresponding chemical reaction for reaction four. After the washing and decantation of the copper oxide, at about 8 mL of sulfuric acid H2SO4 to dissolve the copper oxide. Stir the solution until it becomes clear blue. Explain the steps and write down the corresponding chemical reaction for reaction five.
Weigh out approximately 2 g of zinc metal and added it in very small portions as needed, to recover the Copper metal. Aqueous Zinc sulfate ZnSO4 it's also yielded from the reaction. Occasionally swirl the solution until it colorless. Then, decant the remaining supernactant ZnSO4. Now that we have restored the Copper metal, we need to get rid of the remaining zinc. Go to the exhaust vent and add about 3 mL of distilled water and stir. Then, carefully add about 5 mL of HCl to oxidize any remaining zinc.
The small amount of gas H2 Will be released, leaving the remainder of zinc chloride ZnCl2, which will be decanted. Upon completion of reaction five, what do you do with the restored copper to finish the experiment? After the copper has been restored, wash the copper with distilled water several times, and then watch the copper with isopropyl alcohol at least three times. On the final washing, transfer the copper into an evaporating dish and decant remaining isopropyl alcohol.
Then, transfer the copper into the different pre-weighed evaporating dish. Warm the evaporating dish on a hotplate Warm to the touch. Too much heat will cause a oxidation back to copper oxide, which would be irreversible. Two little heat will cause the sample to retain isopropyl alcohol, both scenarios resulting in a high recovery error.
After cooling, reweigh the evaporating dish and recovered copper until the final mass of copper is below and within. When you are heating the newly restored copper on the hot plate to evaporate the remaining isopropyl alcohol, what do you risk happening if the heat is too high? What if it is too low? If is too high, the copper will oxidize back to copper oxide, which is irreversible.
To Llover temperature will cause the isopropyl alcohol to remain in the Copper. Both scenarios would cause an exceedingly high percent recovery. Write a complete, balanced chemical equation for the following reaction: Solid nickel reacts with aqueous copper II chloride. Write a complete, balanced chemical equation for the following reaction: Aqueous sodium carbonate reacts with aqueous hydrobromic acid. Write a complete, balanced chemical equation for when tin metal reacts with aqueous HCl to produce tin II chloride and hydrogen gas.
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