WRITING NET IONIC EQUATIONSWrite a balanced net ionic equation for the reaction that occurs in each of the following cases. Assume that all soluble reactants are added in the form of aqueous solutions. Indicate gases and precipitates that are formed, as well as insoluble solid reactants. If no reaction occurs, then write "NO RXN" and do not write a balanced equation,1.potassium phosphate + magnesium nitrate →2.calcium chloride +. aluminum nitrate →3.sodium hydroxide + oxalic acid →4.calcium + iron (III) sulfate →5.mercury + sulfuric acid →6.calcium carbonate + sulfuric acid →17.ammonia solution + sulfuric acid →8.sodium sulfide + phosphoric acid →9.aluminum + phosphoric acid →10. sodium hydrogen carbonate + nitric acid →11. lead + calcium chloride →12. nitric acid + silver carbonate →13. calcium hydroxide + ammonium chloride →214. hydrochloric acid + sulfuric acid →15. nitric acid + aluminum hydroxide →16. - zinc + copper (II) chloride →17. calcium acetate + nitric acid →18. ammonia solution + acetic acid →19. barium chloride + sulfuric acid →20. sodium sulfite + hydrochloric acid →3ELECTROLYTES:ARE THEY ACIDS OR BASES?For the following compounds; when added to water, will the resulting solution be strongly acidic, weakly acidic, neutral, weakly basic or strongly basic?1. Ca(CN)22. H2SO33. NH4NO34. BaBr25. HCI6. AgOH7. potassium acetate8. rubidium hydroxide9. lithium chlorite10. H2S11. Na2SO4Activity Series of MetalsK → K++ e-Ba → Ba++ 2e-Ca → Ca++ 2e-Na → Na++ e-Mg → Mg++ 2e-Al → A13++ 3e-Zn → Zn3++ 2e-4Cr → Cr3++ 3e-Fe → Fe2++ 2e-Ni → Ni2++ 2e-Pb → Pb2++ 2e-H2→ 2H++ 2e-Cu → Cu2++ 2e-As → As3++ 3e-Ag → Ag++ e-Hg → Hg++ 2e-Au → Au3++ 3e-5Summary of Information about the Solubilities of Electrolytes in Aqueous Solution6Rule Exceptions1. Nitrates (NO3-, acetates (CH3COO-) chlorates (ClO3-) and perchlorates (CIO4-) are generally soluble.1. No common exceptions. Silver acetate, AgOAc, is only slightly soluble.2. Compounds of the alkali metals, and of the ammonium ion, NH4+, are generally soluble2 No common exceptions. KC1O4 is only slightly soluble.3. Chlorides (Cl-), bromides (Br-), and iodides (I-) are generally soluble3. The halides of Ag+, Pb2+, Hg2+ and Cu+ are insoluble except that PbC12 is slightly soluble. HgI2is insoluble4. Sulfates (SO4-) are generally soluble. 4. PbSO4, SrSO4, and BaSO4are insoluble. CaSO4, Ag2SO4, and Hg2SO4 are slightly soluble.5. Carbonates (CO32-), sulfites (SO32-), chromates (CrO42-), and phosphates (PO43-) are generally insoluble.5. Carbonates, sulfites, chromates and phosphates of alkali metals and of NH4+ are soluble. (See Rule 2.) Li3PO4 is only slightly soluble.6. Sulfides (S2-) are generally insoluble. 6. Sulfides of the alkali metals and of NH4+ are soluble. (See Rule 2). Sulfides of the alkaline earths, Cr2S3, and A12S3 are decomposed by H2O.7. Hydroxides are generally insoluble. 7. Hydroxides of the alkali metals and of NH4+ are soluble. (See Rule 2). Hydroxides of Ca2+, Sr2+ and Ba2+ are slightly