In the first column (pH), predict whether an aqueous solution of the compound would be acidic (a), basic (b) or neutral (n).
In the numbered boxes,
Use the solubility rules to predict the result of mixing the two solutions that intersect to form each box. For example, box #1 represents the mixing of aqueous solutions of HCl and KOH.
IF . . .
-ï a reaction occurs and a precipitate (ppt) forms, write the balanced molecular equation for the reaction. Indicate the formation of a precipitate by using the appropriate state of matter in the equation and by indicating the color of the precipitate. Write the color of the precipitate in the appropriate box in the table. (See #2.)
-ï a reaction occurs and a gas is produced in the reaction, write the balanced molecular equation for the reaction. Indicate the formation of a gas by using the appropriate state of matter in the equation. Write âbubblesâ in the appropriate box in the table.
-ï a reaction occurs but no precipitate forms, write the balanced molecular equation for the reaction. Write NP in the appropriate box in the table. (See #1.)
-ï no reaction occurs, write NR in the appropriate box in the table. (See #72.)
How Can We Use Chemical Interactions to Characterize Compounds? (CH 5) CHM 11500, Fall 2017 Prelab Assignment As part of your individual preparation for lab, read the experiment and answer the following questions in your lab notebook. The copy of your answers on the duplicate (pink) pages is due at the beginning of the lab period Reagents Unknowns pHKOH AgNO3 BaCl2 NaCl NH3(aq) Na2S Na2SO4 H2SO4 HCI HNO3 H2SO4 KOH NH3** Na2S NaCl CuCl2 BaCl2 AgNO3n NP white 12 15 16 20 24 25 28 29 30 32 35 37 38 39 42 43 45 47 48 49 52 54 56 58 63 67 70 72 73 NR 74 75 76 78 79 Cu(NO3)2 a 83 84 87 89 Fe(NO3)3 92 93 95 97 Nal Na2S04n Na2CO3 98 100 102 103 104 105 106 107 108 109 112 These may measure as slightly acidic in the lab because the water may have some carbon dioxide from the air dissolved in it (CO2 + HsO ê·¼ H2CO3 H+ + HCO3 pH ~5-6) **Hint: in water, NH3 produces NH4 and OH-, so you must consider the possible reaction of these ions with the reagents. NH3 (aq) + H2O(l) â NH4"(aq) + OH-(aq). Page 1 of 3
