A chemist needs 1.28 g of sodium hypochlorite, NaOCl(s), for an experiment, but she only has sodium hypochlorite pentahydrate, NaOCl•5H2O(s). How many grams of the hydrate should she use?

Precipitates used in the gravimetric determination of uranium include Na2U2O7 (634.0g/mol), (UO2)2P2O7 (714.0 g/mol), and V2O5 · 2UO3 (753.9 g/ mol). Which of these weighing forms provides the greatest mass of precipitate from a given quantity of uranium?

Sodium hypochlorite is the active ingredient in most household bleach products. One method of preparing this compound is as follows: Cl2(g) + 2N2OH(aq) → NaOCI (aq) + NaCl(aq) + H2O(1) In a certain experiment, 50.0 g chlorine was reacted with 50.0 g sodium hydroxide to yield 37.8 g sodium hypochlorite. (a) Calculate the theoretical yield (b) Calculate the percent yield.

Mg(OH)2(s)+2HNO3(aq)→   the balanced chemical formula?

The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of phosphorus trichloride that can be formed from 226.0 grams of chlorine gas based on the balanced chemical equation?

A chemical reaction calls for 0.125 moles of sodium acetate, NaC2H3O2. What mass, in grams, of sodium acetate would you need to prepare?

Balance the following chemical equation (if necessary): C5H₁0(g) + O₂(g) → H₂O(g) + CO₂(g)

3cucl, (aq) + 2Fe(s) 2Fecl,(aq) • + 3Cu(s) If you had a solution of copper(II) chloride that contained 33.1 g of CuCl, and then added 11.15 g of iron, how much solid copper would you get (assume 10% yield)?

00 S Nazza .01608 ·018302 3. (part a). You are given 0.104 g of a sample of KwFex(C₂O4)y(H₂O)z. In the laboratory, you titrate this sample with 0.00940 M KMnO4 and you need 10.1 mL of the KMnO4 solution to reach the stoichiometric point. Calculate the mass and moles of [C₂04]²- in the sample. Please show all of your detailed calculations.

Iodine is prepared both in the laboratory and commercially by adding Cl, (g) to an aqueous solution containing sodium iodide. 2 Nal(aq) + Cl, (g) - L(s) + 2 NaCl(aq) How many grams of sodium iodide, Nal, must be used to produce 89.4 g of iodine, I,? mass: g Nal Enter numeric value