Which is the correct net ionic equation for the following reaction: 3 (NH4)2CO3 (aq) NH4NO3 (aq) + 2 Al(NO3)3 (aq) 6 + Al2(CO3)3 (s) > Al2(CO3)3(s) O 2 A13+(aq) + 3 CO32 (aq) O 6 NH4+ (aq) + 3 CO32 (aq) + 2 A13+(aq) + 6 NO3(aq) Al2(CO3)3(s) + 6 NH4+(aq) + 6 NO3(aq) NH4+ (aq)+ NO3 (aq) →→ NH4NO3(s) O Al(NO3)3(s) Al3+(aq)+ 3NO3(aq)

An unknown solid acid is either citric acid or tartaric acid. To determine which acid you have, you titrate a sample of the solid with aqueous NaOH and from this determine the molar mass of the unknown acid. The appropriate equations are as follows. Citric acid: H3C6H5O7(aq) + 3 NaOH(aq) 3 H2O(l) + Na3C6H5O7(aq) Tartaric acid: H2C4H4O6(aq)+ 2 NaOH(aq) 2 H2O(l) + Na2C4H4O6(aq) A 0.956-g sample requires 29.1 mL of 0.513 M NaOH to consume the acid completely. What is The unknown acid?

Vitamin C, ascorbic acid (C6HgO6)(molar mass 176.1 g/mol), is a reducing agent. One way to determine the ascorbic acid content of a sample is to mix the acid with an excess of iodine, C6HgO6(aq) + I2(aq) + H2O(l) C6HgO6(aq) + 2 H3O+(aq) + 2 I(aq) and then titrate the iodine that did not react with the ascorbic acid with sodium thiosulfate. The balanced, net ionic equation for the reaction occurring in this titration is I2(aq) + 2 S2O32(aq)2 I(aq) + S4O62(aq) Suppose 50.00 mL of 0.0520 M I2 was added to the sample containing ascorbic acid. After the ascorbic acid/I2, reaction was complete, the I2 not used in this reaction required 20.30 mL of 0.196 M Na2S2O3 for titration to the equivalence point. Calculate the mass of ascorbic acid in the unknown sample.

Balance each of the following equations, and then write the net ionic equation. Show states for all reactants and products (s, . g, aq). (a) the reaction of sodium hydroxide and iron(II) chloride to give iron(II) hydroxide and sodium chloride (b) the reaction of barium chloride with sodium carbonate to give barium carbonate and sodium chloride (c) the reaction of ammonia with phosphoric acid