Chapter 4: Q4.29P (page 179)
Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:
Short Answer
Precipitation of ions depends upon the charge of ions present in a given solution.
Chapter 4: Q4.29P (page 179)
Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:
Precipitation of ions depends upon the charge of ions present in a given solution.
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Get started for freeIn the process of pickling, rust is removed from newly produced steel by washing the steel in hydrochloric acid:
During the process, some iron is lost as well:
(a) Which reaction, if either, is a redox process? (b) If reaction 2 did not occur and all the HCl were used, how many grams of Fe2O3 could be removed and FeCl3 produced in a 2.50x103-L bath of 3.00 MHCl? (c) If reaction 1 did not occur and all the HCl were used, how many grams of Fe could be lost and FeCl2 produced in a 2.50x103-L bath of 3.00 MHCl? (d) If 0.280 g of Fe is lost per gram of Fe2O3 removed, what is the mass ratio of FeCl2to FeCl3?
With ions shown as spheres and solvent molecules omitted for clarity, the circle (right) illustrates the solid formed when a solution containing is mixed with one containing
(a) Identify the solid.
(b) Write a balanced net ionic equation for the reaction.
(c) If each sphere represents of ion, what mass of product forms?
Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:
(a) Cesium hydroxide(aq) + nitric acid(aq)
(b) Calcium hydroxide(aq) + acetic acid(aq)
A mixture of bases can sometimes be the active ingredient in antacid tablets. If 0.4826 g of a mixture of and is neutralized with 17.30 mL of 1.000 M what is the mass % ofin the mixture?
Question: Zinc hydroxide is insoluble in water but dissolves when a nitric acid solution is added. Why? Write balanced total ionic and net ionic equations, showing nitric acid as it actually exists in water and the reaction as a proton-transfer process.
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