9.20 Characterize the following compounds as soluble or...

9.20 Characterize the following compounds as soluble or insoluble in water: (a) CaCO3, (b) ZnSO4, (c) Hg(NO3)2, (d) HgSO4, (e) NH4ClO4. 9.21 Characterize the following compounds as soluble or insoluble in water: (a) Ca3(PO4)2, (b) Mn(OH)2, (c) AgClO3, (d) K2S, (e) Pb3(PO4)2. 9.22 Write ionic and net ionic equations for the following reactions: (a) Na2S(aq) + ZnCl2(aq) ? (b) K3PO4(aq) + 3Sr(NO3)2(aq) ? (c) Mg(NO3)2(aq) + 2NaOH(aq) ?

Transcript

00:01 All right so where to characterize the compounds and indicate whether they are strong acids or sorry they're soluble or insoluble so we have the first one calcium carbonate following the solubility rule this is insoluble because all carbonates are insoluble right except those are one metals and ammonia so this is insoluble this is insoluble right then if you look at the next one zinc sulfate zinc sulfate all sulfates are soluble the exceptions are your all sulfates are soluble except calcium barium lead silver and sodium so zinc is this is soluble this is soluble if you look at the next one um we have mercury 2 nitrate ag hg no3 bracket 2 this is soluble all nitrates are soluble and if you look at the next one um mercury sulfate mercury sulfate is also right it's also going to be soluble it's soluble because it's not part of the exception and then and select the last one um ammonium chlorate or ammonium perchlorate nh4 clo4 right all sorts are soluble so this is soluble the next set um for calcium phosphate calcium phosphate is insoluble right all phosphates are insoluble it's insoluble um my manganese hydroxide all the hydroxide of transition metals are insoluble this is insoluble manganese hydroxide is insoluble silver chlorate silver perchlorate next one um ag clo4 that is soluble very soluble it's actually really soluble perchlorate and potassium sulfide potassium sulfide that is soluble because it's a group one right if it don't sulfides are insoluble but potassium sulfide will be soluble and then lead 2 phosphate is insoluble right pb3 po4 bracket 2 this is insoluble right all phosphates are insoluble okay so the final part of the question we're to write the ionic equation the net ionic equation for the um reactions so we have sodium sodium sulfide plus zinc 2 chloride we have na2s plus zncl2 and of course you would have zns plus sodium chloride 2 but the net ionic equation um is going to be s2 minus plus zn2 plus and you're gonna have zns solid right the spectator ions are your sodium and your chloride ions the next one you have k3 po4 that's potassium phosphate plus strontium nitrate and the product should be um six moles so this is going to be two moles actually so that that that would be balanced and you would have six moles of potassium nitrate and you should have um you should have potassium phosphate one mole of that right and the net ionic equation the spectator ions will be the potassium and the nitrogen will be po4 3 minus plus that's 2 po4 3 minus plus 3 sr2 plus and then you will have sr3 po4 bracket 2 that's the ionic equation and then magnesium nitrate plus sodium hydroxide magnesium nitrate plus two moles of sodium hydroxide plus two moles of sodium hydroxide and then you will have magnesium hydroxide which is insoluble and sodium nitrate that's the molecular equation the ionic equation would be the reaction between magnesium ions and two moles of hydroxide ions and you have magnesium hydroxide...

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