One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with copper(II) chloride, which would react with silver nitrate solution like this: CuCl,(aq) + 2 AgNO,(aq) → 2 AgCl(s) + The chemist adds 24.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 6.9 mg of silver chloride. Calculate the concentration of copper(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits.

A chemist prepares a solution of copper(II) sulfate (CuSO,) by measuring out 12. g of copper(II) sulfate into a 300. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's copper(II) sulfate solution. Round your answer to 2 significant digits. mol/L

5 ( An analytical chemist weighs out 0.118 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1100 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 12.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. g x10 mol 3 ? Explanation 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility Check X

How many moles of sodium hydroxide, NaOH, are present in 1.73 L of a 0.157 M sodium hydroxide solution? Place your answer in the box. Express your answer using only a number without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.

A chemist prepares a solution of barium acetate  BaC2H3O22  by measuring out  105.g  of barium acetate into a  250.mL  volumetric flask and filling the flask to the mark with water.   Calculate the concentration in  /molL  of the chemist's barium acetate solution. Round your answer to  3  significant digits.

A student prepares a 0.70 mM aqueous solution of butanoic acid (C,H,CO2H). Calculate the fraction of butanoic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. ① % X 나

How many liters of 0.250 M NaOH solution can be prepared from 10.0 g of NaOH? Place your answer in the box. Express your answer using only a number without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.

An analytical chemist weighs out 0.181 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0900M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 34.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. x10 mol

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A chemist must prepare 725.mL of 793.μM aqueous magnesium fluoride (MgF2) working solution. He'll do this by pouring out some 0.00148M 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. Round your answer to 3 significant digits.