Question

5. An aqueous solution containing 10.0 g sodium hydroxide is added to an aqueous solution containing 10.0 g phosphoric acid. a. (4) Write and balance the complete chemical reaction. b. (4) Write the ionic acid the net ionic equations for the reaction. C. (4) Determine which reagent is limiting in the reaction. d. (1) Will the solution be acidic or basic after the reaction is complete?

Answer 1

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6 sodium hydroxide @ 3 NaOH cags & Sodium hydroxide (NOK) ; phosphosie acid (H3PO4). NaOH cags + H₂PO4 (aq) Na3PO4 (aq) + B ocus lonte equation write down all possible ionic and non- donic species - 3 Nat Cart 301 (aq) + 31 Tags & Pola 3 Natragst poze Cars + 3 H₂0 (1) Net lonce equation & cancell the spectator ions which are common on both sides 800 (ar) + At cag) - 8H₂0 (1) Oh cag) + + (aq) Ha (1) © NaOH]:- Mass = (0.09 ; molar maxs - 39.99 glmol no. of moles - mars (2) – 10.09 molar Mass (g/mol) H3PO4 - Mass - 10.og molar mass = 97.99 g/mol no.of moles = 10.09 39.99 almoy = 0.25 mars = 0.1020 mot from ou 97.99g/mol Nos 3 mol naoh reacts with a mol H₂PO4 2 0.25 mol xlmol so 0.25 ml NaOH reacts with - mol Haloy 3 moj = 0.0833 mol But there is ..1020 mol of H₂PO4, which is more than enough (in excess), in Nooh is limiting reactant which will be consumed completely Here, NaOH completefy reacts with H₂PO₂ 10.0833 mol). Then the remaining H₂PO2 (0.1020 mol-0.0833 mol = 0.0186 will be left over. So the solution is acidic (:: Hapon is an acid). (0.25 mol