Question

in the table below, predict which of the following reactant combinations will produce precipitates and write all the products that form (including states of matters- l, s, aq, g; write "ss" if it is slightly soluble). Useful information is also below.

TABLE 4.1 | Simple Rules for the Solubility of Salts in Water 1. Most nitrate (NO3-) salts are soluble. 2. Most salts containing the alkali metal ions (Li+, Na+, K+, Cst, Rb+) and the ammonium ion (NH4+) are soluble. 3. Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag+, Pb2+, and Hg22+. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, Hg2SO4, and CaSO4- 5. Most hydroxides are only slightly soluble. The important soluble hydroxides are NaOH and KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble. 6. Most sulfide (52-), carbonate (CO32-), chromate (CrO2-), and phosphate (PO43-) salts are only slightly soluble, except for those containing the cations in Rule 2.

Answer 1

The balanced reactions are as follows -

1. Na2SO4 (aq) + H2SO4 (aq) → 2 NaHSO4 (aq)

2. 2 NaHSO3 (aq) + H2SO4 (aq) → 2 H2SO3 (aq) + Na2SO4(aq)

3. H2SO4 (aq) + Na2CO3 (aq) → Na2SO4 (aq) + H2O (l) + CO2 (g)

4. 2 NaNO3 (aq) + H2SO4 (aq) → 2 HNO3 (aq) + Na2SO4 (aq)

5. 3 H2SO4 (aq) + 2 Na3PO4 (aq) → 3 Na2SO4 (aq) + 2 H3PO4 (aq)

6. 2 NaCl (aq) + H2SO4 (aq) → 2 HCl (aq) + Na2SO4 (aq)

7. 2 NaBr (aq) + 2 H2SO4 (aq) → Na2SO4 (aq) + Br2 (aq) + SO2 (g) + 2 H2O (l)

8. 2 NaI (aq) + H2SO4 (aq) → I2 (s) + Na2SO3 (aq) +  H2S (g) + H2O (l)

There are no precipitates formed as the products are salts of sodium that are water soluble.