A chemist needs to create a series of standard Cu²+ (aq) solutions for an absorbance experiment. For the first standard, he uses a pipet to transfer 10.00 mL of a 2.07 M Cu²+ (aq) stock solution to a 500.0 mL volumetric flask, and he adds enough water to dilute to the mark. He then uses a second pipet to transfer 5.00 mL of the second solution to a 100.0 mL volumetric flask, and he adds enough water to dilute to the mark. Calculate the concentration of the Cu²+ (aq) solution in the 100.0 mL volumetric flask. concentration: M

A chemist needs to create a series of standard Cu²+ (aq) solutions for an absorbance experiment. For the first standard, he uses a pipet to transfer 10.00 mL of a 2.07 M Cu²+ (aq) stock solution to a 500.0 mL volumetric flask, and he adds enough water to dilute to the mark. He then uses a second pipet to transfer 5.00 mL of the second solution to a 100.0 mL volumetric flask, and he adds enough water to dilute to the mark. Calculate the concentration of the Cu²+ (aq) solution in the 100.0 mL volumetric flask. concentration: M

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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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.
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?
Andrew dissolved 10.00 grams of an iron ore sample in 5.00 L of acid to produce a stock solution. Josh ran a trial of the analytical procedure on the stock solution, but found the solution was too concentrated to be used. So Josh prepared a 1:250 dilution of the sample solution, and, after running the analytical procedure successfully, found the solution contained 1.62 x 10-5 mol/L Fe2+ (aq). What is the mass of iron in the meteorite sample?
A 1.6 g sample of a compound is transfered to a 100 mL volumetric flask, filled to the mark with distilled water, and thoroughly mixed. Twenty five milliters of this solution is drawn from the flask using a volumetric pipet, transfered to another 100 mL volumetric flask, and filled to the mark and mixed. The grams of compound in the second volumetric flask is: A. 1.6 B. 1.2 C. 0.80 D. 0.40
Potassium permanganate in acidic solution is used to titrate a solution of copper(I) ions, with which it reacts according to MnO4-(aq) + 5Cu+(aq)+8H3O+(aq)Mn2+(aq) + 5Cu2+(aq)+12H2O(l) A potassium permanganate solution is prepared by dissolving 23.14 g of KMnO4 in water and diluting to a total volume of 1.000 L. A total of 15.61 mL of this solution is required to reach the endpoint in a titration of a 200.0-mL sample containing Cu+(aq). Determine the concentration of Cu+ in the original solution.
Come up with a dilution scheme for a test solution starting from 1000 μg/mL Mn stock solution so that the concentration of permanganate in the solution just prior to measurement is approx. 20 μg/mL MnO4-. Carefully read the units!
Tartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of apple wine. Emma was tasked to find out the acid content in a 50.0 mL wine sample by titrating it with a standardized solution of NaOH. She was able to establish the working concentration of the NaOH solution by using 17.61 mL of NaOH to titrate a primary standard of KHP that weighed 1.501 g. The grams and %w/w of Tartaric acid present in the 50.0 mL wine sample were then determined by titrating a 12.50 mL aliquot using 21.78 mL of the standardized NaOH solution. H2C4H4O6 (aq) + 2NaOH (aq) ↔ Na2C4H4O6 (aq) + 2H2O (l) Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol What is the molar concentration of the prepared NaOH solution?…
You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Molarity H2C2O4 standard solution is 0.48 M how many Moles of NaOH are there in each trial?
For the analysis of unknown soda and vinegar samples, 25.0 mL soda and 1.0 mL vinegar samples were diluted to 50.0 mL in separate Erlenmeyer flasks. KHP, 0.85 g, (Purity = 99.98%; Molar mass = 204.22 g/mol) was titrated with 11.5 mL of NaOH. After the standardization step, it required 0.0143 L of NaOH to reach the endpoint with the soda sample while it took 0.00885 L with the vinegar sample. Phenolphthalein was used as the indicator for the experiment. Express all final answers in 2 significant figures. a. Determine the concentration of the titrant (NaOH) b. Determine the concentration of the unknown vinegar sample. c. Determine the concentration of the unknown soda sample.
A chemistry student weighs out 0.157g of lactic acid HC3H5O3 into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1800M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits.
Gold can be determined in solutions containing high concentrations of diverse ions by ICP. Aliquots of 50.0 mL of the sample solution were transferred to each of four 100.0 mL volumetric flasks. A solution was prepared containing 10.0 mg/L Au in 20% H2SO4, and quantities of this solutions were added to the sample solution to give 0, 2.5, 5 and 10 mg/L added Au in each of the flask. The solutions were made up to a total volume of 100.0 mL, mixed and analyzed by ICP. The resulting data are presented in the following table: Added Au (mg/L) Emission Intensity (Counts) 0.0 12568 2.5 19324 5.0 26622 10.0 40021 a) Attach an excel graph for the determination showing the X intercept. b) Calculate the concentration of gold in the sample, report with its uncertainty. c) The known concentration of gold in the sample is 8.51 mg/L. Test the hypothesis that your result is equal to this value at the 95% confidence level. l