Name:……………………………………………………. Date: …………………… Making Salts Worksheet This worksheet accompanies Making Salts Summary and Precipitation Reactions Summary. 1. When an acid reacts with a base, a neutralisation reaction occurs, producing a salt. Using the following equation, name the salts that are produced in the acid-base reactions. acid + base salt a) hydrochloric acid + ammonia → ……………………… b) nitric acid + sodium hydroxide → ……………………… c) phosphoric acid + potassium hydroxide →……………………… 2. There are three other ways of making salts from acids. Complete the following equations to illustrate them. a) acid + metal → salt + ……………………… b) acid + ……………………… → salt + water c) acid + carbonate → salt + ……………………… + water 3. Use the above information to complete the following reactions that form soluble salts using acids. a) iron oxide + sulfuric acid → ……………………… + water b) ……………………… + hydrochloric acid → magnesium chloride + H2O + CO2 c) zinc + ……………………… → zinc nitrate + hydrogen 4. Name two ways in which salt is used by humans in everyday life. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… © Boardworks Ltd 2011 1 Name:……………………………………………………. Date: …………………… 5. A student conducts an experiment to obtain the salt zinc nitrate from zinc oxide powder (ZnO). He adds the powder spoon by spoon into a flask containing 1M of nitric acid (HNO3). a) Describe what happens to the first spoonfuls of powder when he mixes it with the acid. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b) Describe what would happen if the student kept adding zinc oxide to the nitric acid after the reaction between the acid and metal oxide was complete. …………………………………………………………………………………….……………………… …………………………………………………………………………………….……………………… c) Write a word and symbol equation to show the results of this experiment. ……………………………………………………………………………………..……………………… ……………………………………………………………………………………..……………………… 6. Fill in the missing symbols and balance the following equations for making salts. a) 2Na + Cl2 → ………… NaCl b) Al2O3 (s) + 3H2SO4 (aq) → Al2(SO4)3 (……) + 3H2O (l) c) H3PO4 (aq) + ….KOH(s) → K3PO4(aq) + … H2O(I) d) LiOH + HNO3 → LiNO + ………… + H2O e) Ba(OH)2 + H2SO … → BaSO4 + 2H2O f) …………HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O © Boardworks Ltd 2011 2 Name:……………………………………………………. Date: …………………… 7. Most precipitation reactions are very fast reactions that occur between ions. They occur when two solutions of ions react to form an insoluble solid called a precipitate. a) Complete the symbol equation for the precipitation reaction between lead nitrate and potassium iodide that produces the insoluble salt lead iodide. Pb(NO3)2 (aq) + 2Kl(aq) → Pbl2 (s) + ………………… (aq) b) Complete the ionic equation for this reaction. Pb2+ + 2NO3(-)+ 2K+ + 2l- → ………………… 8. Sodium hydroxide was poured into a test tube containing a colourless solution. The metal’s hydroxide precipitate turned the solution blue. a) Identify the metal ion present in the colourless solution. Circle your answer. Fe2+ Cu2+ Fe3+ b) In another experiment, dilute hydrochloric acid was poured into a test tube containing a colourless solution. The acid’s hydrogen ions reacted with the metal ions in the solution and produced the gas sulfur dioxide. Balance the ionic equation for this reaction. SO32- + H+ (aq) → SO2 (g) + H2O (l) c) Write a balanced ionic equation for the reaction between Cu2+ and OH-. …………………………………………………………………………………………………………….. 10. a) Negative ions in salts can be identified in a solution by adding a reagent. Describe an experiment to show that sulfite ions (SO32-) are present in a solution. ………………………………………………………………………………………….…………………. ….……………………………………………………………………………………….……..…………. ……....……………………………………………………………………….…..………….……….…… …………………………………………………………………………………………………………….. ...................................................................................................................................................... b) Write the ionic equation for this reaction. ……………………………………………………………………………………………………………. © Boardworks Ltd 2011 3
