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Find the number of cm³, in 2.60 ft.³.
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- mol L A chemist must prepare 850. mL of 2.00 M aqueous silver nitrate (AgNO3) working solution. He'll do this by pouring out some 4.47 aqueous silver nitrate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the silver nitrate stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits.A chemist prepares a solution of potassium chloride (KC1) by measuring out 43. mg of KCl into a 50. mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Canions in the chemist's solution. Be sure your answer is rounded to 2 significant digits. 0 mol L x10 X ŚA chemist adds 0.45 L of a 2.9 × 10 M copper(II) fluoride (CuF,) solution to a reaction flask. Calculate the mass in milligrams of copper(II) fluoride the chemist has added to the flask. Be sure your answer has the correct number of significant digits. O mg
- A chemist wants to make 5.0 L of a 0.280 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use? Express your answer in grams using two significant figures.A chemist wants to make 6.5 L of a 0.290 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use? Express your answer using two significant figures.Methyl benzoate is an oily liquid with a boiling point of 199°C. What volume of methyl benzoate is needed to prepare 5.8 grams of benzoic acid? The density of methyl benzoate is 1.08 g·cm⁻³. Molar masses are given in Figure 4. [Give only the number without the unit. Give the answer in cubic centimetres and round to 1 decimal place. Use a decimal point.] * Your answer
- A sample of an ethanol-water solution has a volume of 54.4 cm^3 and a mass of 49.9 g. What is the percentage of ethanol (by mass) in the solution? (Assume that there is no change in volume when the pure compounds are mixed.) The density of ethanol is 0.789 g/cm^3 and that of water is 0.998 g/cm^3.A) Calculate the molarity 12.21 mg KI in 107.6 mL of solution Express your answer using four significant figures. B) A chemist wants to make 6.0 L of a 0.310 MCaCl2 solution. What mass of CaCl2 (in g) should the chemist use? Express your answer in grams using two significant figures.A 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 + 0
- What is the mass (in kg) of 6.89 × 10^25 molecules of carbon dioxide? Give the answer as a number. The units are understood to be kg.A tablet of Mylanta antacid contains 0.300 g Mg(OH)2 and 0.200 g Al(OH)3. For the blanks in this question: Report here only your numerical answers (without units), if the value is less than zero as a decimal (not in scientific notation), to the correct number of significant figures. Mg(OH)2 (molar mass: 58.32 g/mole) Al(OH)3 (molar mass: 78.00 g/mole) How many moles Mg(OH)2 are present in the tablet? How many moles of Al(OH)3 are present in the tablet? How many moles of HCl are required to neutralize the Mg(OH)2 in the tablet? Start this question by using your rounded answer from #1. How many moles of HCl are required to neutralize the Al(OH)3 in the tablet? Start this question by using your rounded answer from #2. How many moles of HCl acid will be required to neutralize both the Mg(OH)2 and the Al(OH)3 in the tablet? Use your rounded answers from #3 and #4 to answer this question. How many milliliters of 0.200 M HCl can be neutralized by one tablet? Use your rounded…A chemist prepares a solution of potassium dichromate (K, Cr,0,) by measuring out 63.7 umol of potassium dichromate into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's potassium dichromate solution. Be sure your answer has the correct number of significant digits. H mol L