Tin(IV) sulfide, SnS,, a yellow pigment, can be produced using the following reaction. SnBr, (aq) + 2 Na,S(aq) → 4 NaBr(aq) + SnS,(s) Suppose a student adds 45.7 mL of a 0.570 M solution of SnBr, to 51.3 mL of a 0.118 M solution of Na, S. Identify the limiting reactant. O SnS, NaBr O Na, S SnBr4 Calculate the theoretical yield of SnS,. theoretical yield: The student recovers 0.304 g of SnS,. Calculate the percent yield of SnS, that the student obtained. percent yield:

In the laboratory, a student dilutes 28.1 mL of a 8.85 M hydrobromic acid solution to a total volume of 250.0 mL. What is the concentration of the diluted solution?

In a titration experiment, a 5.00-mL sample of sulfuric acid, H2SO4, from a car battery is diluted with de-ionized water to 100.0 mL. A 20.00-mL portion of the diluted acid is titrated with 0.2025 M NaOH solution. If 42.00 mL of the NaOH solution is required to neutralize the dilute acid, what is the molar concentration of H2SO4 in the original solution taken from the battery? The acid-base reaction occurs as follows:                 H2SO(aq)  +  2NaOH(aq)   -->  Na2SO4(aq)  +  2H2O(l)          (A) 0.2126 M                             (B) 0.4252 M                             (C) 4.25 M                     (D) 8.50 M

5. A student mixed 20.00 grams of calcium nitrate, 10.00 grams of sodium nitrate, and 50.00 grams of aluminum nitrate in a 5.00 Litre volumetric flask. What is the molarity (M) of the resulting solution relative to the nitrate ion, NO31?