A chemist prepares a solution of zinc oxalate (ZnC₂04) by measuring out 3.94 mg of zinc oxalate 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 zinc oxalate solution. Be sure your answer has the correct number of significant digits. x 10 mol/L x10 X

A chemist prepares a solution of zinc oxalate (ZnC₂04) by measuring out 3.94 mg of zinc oxalate 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 zinc oxalate solution. Be sure your answer has the correct number of significant digits. x 10 mol/L x10 X

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter1: Introduction To Chemistry

Section: Chapter Questions

Problem 1.87PAE: 1.87 A solution of ethanol in water has a volume of 54.2 mL and a mass of 49.6 g. what information...

See similar textbooks

Similar questions

A chemist prepares a solution of silver(I) nitrate AgNO3 by measuring out 6.4102 x 10^2 μmol of silver(I) nitrate into a 450.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's silver(I) nitrate solution. Round your answer to 2 significant digits.
A 10.00 mL solution of a certain food dye has a concentration of 1.47 g /L. What is the total mass of food dye in the solution? Report your answer with the correct number of significant figures.
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 sample of 18.11 grams of sodium hydroxide is weighed out on a balance and prepared to a volume of 2.00 x 102 mL in water. What is the molarity of this aqueous solution of NaOH? Express your answer to the correct number of significant figures and include the unit with your answer.
At a certain temperature, an aqueous solution is 16.5% K2CO3 by mass and has a density of 1.149 g/cm3. What is the molarity of the solution?Provide your answer with 3 significant figures.
How many grams of iron ammonium sulfate hexahydrate (Fe(NH4)2(SO4)2*6H20; 392.14 g/mol ) must be dissolved in a 250.0 mL volumetric flask to make a solution that has a Fe2 + concentration of 5.36x10 - 3 M? Be sure to enter you answer with the correct number of significant figures for the precision needed in the concentration.
A chemistry student weighs out 0.152g of phosphoric acid H3PO4 , a triprotic acid, into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits.
A certain solution is 5.84 % by mass in calcium carbonate (CaCO3). If the density of the solution is 1.02 g/mL, what mass (in grams) of calcium carbonate is contained in 46.4 mL of solution? (3 sf)
A chemist must prepare 625.mL of 149.μM aqueous magnesium fluoride MgF2 working solution. He'll do this by pouring out some 0.00179M aqueous magnesium fluoride stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the magnesium fluoride stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits.
A chemist must prepare 300.mL of 2.00M aqueous silver perchlorate AgClO4 working solution. He'll do this by pouring out some 5.62molL aqueous silver perchlorate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the silver perchlorate stock solution that the chemist should pour out. Round your answer to 3 significant digits.
If you made a solution of 1.5 ppm of Pb in 1.25 mL of nitric acid, from 0.25 mL of a stock solution. What is the concentration of the stock solution? Give your answer in ppm. Use the correct number of significant figures.
A chemistry student weighs out 0.379g of citric acid H3C6H5O7, a triprotic acid, into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits.