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- Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.A chemist prepares a solution of iron(II) bromide (FeBr,) by measuring out 223. umol of iron(II) bromide into a 200. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's iron(II) bromide solution. Be sure your answer has the correct number of significant digits. H mol LA student is measuring the density of soda using a completely-filled flask of known volume. The student performing the experiment uses a sample that contains air bubbles. The student expects that this will artifically increase the calculated density of the solution. Select the answer below that is most appropriate. The student is incorrect. Air bubbles will have no effect on the calculated density of the soda. The student is incorrect. Air bubbles in the sample will cause the calculated density to decrease. The student is correct. Air bubbles in the sample will cause the calculated density to increase. The student is incorrect. Air bubbles will react with the water to form oxygen gas, which will cause the calculated density to increase. The student is incorrect. Air bubbles will react with the water to form carbon dioxide, which will cause the calculated density to increase.
- A chemist prepares a solution of magnesium fluoride (MgF,) by measuring out 0.0152 µumol of magnesium fluoride into a 200. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's magnesium fluoride solution. Be sure your answer has the correct number of significant digits. mol olo L ArA flask weighs 345.8g is filled with 225mL of carbon tetrachloride. The weight of the flask and carbon tetrachloride is found to be 703.55g. From this information,calculate the density if carbon tetrachlorideA chemist prepares a solution of iron(III) bromide (FeBr;) by measuring out 132. umol of iron(III) bromide into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol L of the chemist's iron(III) bromide solution. Round your answer to 3 significant digits. mol a10 L.
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- A chemist must prepare 0.100 L of 1.00 M aqueous barium chloride (BaCl,) working solution. He'll do this by pouring out some mol aqueous barium chloride stock solution into a graduated cylinder and diluting it with distilled water. 1.73 L Calculate the volume in L of the barium chloride stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits.A chemist must dilute 16.6mL of 2.03M aqueous zinc nitrate ZnNO32 solution until the concentration falls to 1.00M. She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits.A chemist must dilute 39.5mL of 664.mM aqueous barium acetate BaC2H3O22 solution until the concentration falls to 434.mM . She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits. mL