3. You are asked to determine the percentage of the components of a mixture containing sodium iodide Nal, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82 g. First you extracted the Nal from the mixture with water and filtered insoluble Mg(OH)2 and Baso from the solution, containing the Nal. After evaporating and drying the filtrate, you find that you have recovered 0.95 g of Nal When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCI, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04 g of BasO4 Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering the solution and drying the precipitate, you recovered 1.21 g of Mg(OH)2. a) Calculate the percent Nal in the original sample mixture b) Calculate the percent Mg(OH)2 in the original sample mixture c) Calculate the percent BaSO, in the original sample mixture. DELL F11 F12 F10 F7 F8 F5 F6 F3 F4 8 7 8 4 5 3 ㄒ

Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 3.7 g of iron are to be dissolved in 2.0 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?

H2. Titrations are performed by a scientist in the laboratory as follows: a solution of deuterated hydrochloric acid contains 1.08 g DCl in 750 ml of deionised, distilled water. An average amount of 14.95 ml of the DCl(aq) solution is titrated with 25.0 ml of Ca(OH)2 to produce an endpoint (as determined by an appropriate indicator). What is the molarity of the Ca(OH)2 solution? You must include all of your calculations    Please give typed answer

A 2.50 g sample of a group 3A metal chloride, MCl3, is mixed with excess AgNO3. The mass of the AgCl precipitate is 3.46 g.  What is the identity of the group 3A metal?