For the synthesis of boric acid; 7.94 g of anhydrous borax was taken and 15 mL of water was added and the mixture was heated until it dissolved. After the addition of 5 mL of HCl, 5.830 g of crystals were obtained from the mixture which was cooled in an ice bath. What is the percentage yield of the reaction? (Na: 23; B: 11; O: 16; H: 1; Cl: 35.5 g / mol) (d: 1.19g / mL for 37% HCl, dH2O = 1 g / mL)

refer to the following balanced equation

For the experiment " limiting reactant " and after filtering the precipitate, you checked the filtrate (supernatant) to identify the limiting reactant. 2Na3PO4 + 3BaCl2 – Ba;(PO4)2 (s) + 6NACI If you added BaCl, to the filtrate (supernatant) and a white precipitate was formed, this means that a. Both BaCl2 and Na3PO4 are limiting reactants O b. NazPO4 is the limiting reactant O c. BaCl, is the limiting reactant Od. BaCl, is an excess O e. None of the mentioned

Consider the reaction:3A+4B -> 3C  What is the limiting reactant if 1 moleof A is allowed to react with 1 mole B?

(b) In the reaction with 50.0 g of magnesium and 50.0 g of copper(II) nitrate how many grams of the precipitate will you produce? Is magnesium or copper(II) nitrate the limiting reactant?  (c) Which is undergoing oxidation? (d) Which is undergoing reduction?

19. A product weighing 12.11 g was isolated/obtained in the laboratory. The maximum amount of obtainable product was calculated to be 20.51g. What is the percentage (%) yield of this reaction?

The nitrogen in sodium nitrate and in ammonium sulfate is available to plants as fertilizer. Which is the more economical source of nitrogen, a fertilizer containing 30.0% sodium nitrate by weight and costing $9.00 per 100 lb or one containing 20.0% ammonium sulfate by weight and costing $8.10 per100 lb?

for the following reaction 28.3 grams of disphosphorus pentoxide are allowed to react with 15.0 grams of water. What is the maximum amount of phosphoric acid that can be formed?

Balance the following chemical equations (type corresponding coefficients (1, 2, 3, ...) in blanks). NaOH + H3PO4 → NazPO4 + H20

3. A student followed the procedure of this experiment to determine the percent NaOCl in a commercial bleaching solution that was found in the basement of an abandoned house. The student diluted 50.00 mL of the commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mL aliquot of the diluted bleaching solution. The titration required 35.46 mL of 0.1052M Na,5203 solution. A faded price label on the gallon bottle read S0.79. The density of the bleaching solution was 1.10 g mL-? h. Calculate the mass of one gallon of the commercial bleaching solution. i. Calculate the cost of 100 g of the commercial bleaching solution. j. Determine the cost of the amount of commercial bleaching solution required to supply 100 g of NaOCl.