Calculate the volume of liquid in the tank sketched below. Give your answer in liters, and round to the nearest 0.01 L. 6.4 cm 0.135 m 7.8 cm 0₁ X
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- 1.87 A solution of ethanol in water has a volume of 54.2 mL and a mass of 49.6 g. what information would you need to look up and how would you determine the percentage of ethanol in this solution?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 LCalculate the volume of liquid in the round flask sketched below. Give your answer in liters, and round to the nearest 0.01 L. I Don't Know Submit 9.0 cm L X
- How much water, in mL, needs to be added to 29.7 mL of 11.2 M HNO3 to make a 6.05 M solution with the same amount of moles of HNO3? Record 3 significant digits in your answer. Don't type units in. Round your answer to 3 significant figures.mol stock solution of silver A chemist makes 590. mL of silver perchlorate (AgCIO,) working solution by adding distilled water to 180. mL of a 19.0 perchlorate in water. Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits. mol x10 L.A chemist prepares a solution of iron(II) bromide (FeBr₂) by measuring out 491. g of iron(II) bromide into a 500. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's iron (II) bromide solution. Be sure your answer has the correct number of significant digits. ? mol/L x10 X Ś 00. 18 Ar
- 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. mLA chemist must prepare 925. mL of 435. mM aqueous aluminum sulfate (Al₂(SO4)3) working solution. She'll do this by pouring out some 0.596 L mol aqueous aluminum sulfate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the aluminum sulfate stock solution that the chemist should pour out. Round your answer to 3 significant digits. 0mL 0 S ? Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DII DD J () FB F9 F12 esc Explanation F1 ! 1 @ 2 x x Check F2 #3 80 F3 DS 4 F4 % 5 F5 MacBook Air S ^ 6 F6 & 7 aa F7 * 00 8 ( 9 ) 0 F10 F11 + 0A 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.
- Calculate the volume of liquid in the round flask sketched below. Give your answer in milliliters, and round to the nearest 0.1mLA chemist must prepare 275.mL of 25.0mM aqueous barium chlorate BaClO32 working solution. He'll do this by pouring out some 54.9mM aqueous barium chlorate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the barium chlorate stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits.A chemist makes 260. mL of iron(III) bromide (FeBr,) working solution by adding distilled water to 160. mL of a 1.88 mol stock solution of iron(III) bromide in water. Calculate the concentration the chemist's working solution. Be sure your answer has the correct number of significant digits. mol x10 L