(Ba(C₂H,O2)2)1 solution until the concentration falls to 1.00 M. She'll doA chemist must dilute 26.4 mL of 1.50 M aqueous barium acetate (Ba(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.☐ mLx10

Dilution is the process of adding a solvent to a solution to reduce its concentration. In this…

Answered: (Ba(C₂H,O2)2)1 solution until the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter2: Chemical Compounds

Section: Chapter Questions

Problem 143QRT: The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry...

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What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of KIO3 that can be used.
A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
I||| O O CHEMICAL REACTIONS Calculating ion molarity using solute mass A chemist prepares a solution of magnesium chloride (MgCl₂) by measuring out 64. mg of MgCl₂ into a 100. mL volumetric flask and filling to the mark with distilled water, Calculate the molarity of CI anions in the chemist's solution. Be sure your answer is rounded to the correct number of significant digits. Microsoft O W Microsoft Microsoft 6.52.210... esc mol L Explanation 1 C Check 0,207 2 W # 3 103 E On NOV 6 X $ 4 R 15 % tv T 2 MacBook Pro 6 Y & 7 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. * 0 U 66 C 8 A Terms of Use | Privacy Center | Accessibility W 0 9 T 0 O P DI { 5 dla M 2 lab h Englis }
1597 59 S ||| 2 O CHEMICAL REACTIONS Calculating ion molarity using solute mass A chemist prepares a solution of magnesium bromide (MgBr₂) by measuring out 2.1 g of MgBr, into a 300. mL volumetric flask and filling to the mark with distilled water. V Calculate the molarity of Br anions in the chemist's solution. Be sure your answer is rounded to the correct number of significant digits. Microsoft O W Microsoft Microsoft 6.52.210... esc mol L Explanation 18 ! 1 Check 9,206 2 # 3 103 NOV 6 X $ 4 O 67 5⁰ % 5 stv 6 Y 2 & 7 © 2022 McGraw Hill LLC. All Rights Reserved. U * CO 66 8 A 9 I 1 Terms of Use | Privacy Center | Accessibility W 0 0 P { [ do F }
A chemist prepares a solution of barium acetate (Ba(CH,CO2),) by measuring out 1.3 x 10² µumol of barium acetate into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's barium acetate solution, Be sure your answer has the correct number of significant digits. mmol
Calculate the molarity of the solution that results when 8.5 ml of CH3OH (methyl alcohol or methanol) is dissolved in 7.5 ml of water (CH3OH; density 0.792 g/mL) C = 12.01 H = 1.008 O = 16.00 Write this answer with one digit past the decimal point. (Important - Trailing zeroes count as digits - (e.g. 12.0 counts as one digit past the decimal point). The molarity is ______________________M
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 wants to make 5.0 LL of a 0.330 MCaCl2MCaCl2 solution. What mass of CaCl2CaCl2 (in gg) should the chemist use? Express your answer in grams using two significant figures.
A chemistry student weighs out 0.133 g of citric acid (H,C,H;0,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1000M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. mL

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