a. Calculate [Na] (the molarity of sodium ion) when 15-mL of 0.770 M NaH2PO4 and 82-mL of 0.385 MNa₂HPO4 are mixed and diluted to a total volume of 500.0 mL.M

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Answered: a. Calculate [Na] (the molarity of…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

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Problem 125AP: When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting...

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A 300.0-g sample of a solid is made up of a uniform mixture of NaNO3, MgCl2, and BaCl2. A 100.0-g sample of the mixture is dissolved in water and treated with an excess of KOH. The precipitate from the reaction has a mass of 13.47 g. The remaining 200.0-g sample is also dissolved in water and treated with an aqueous solution of AgNO3. The resulting precipitate has a mass of 195.8 g. What are the masses of NaNO3, MgCl2, and BaCl2 in the 300.0-g sample?
39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.
When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?
You mix 25.0 mL of 0.234-M FeCl3 solution with 42.5 mL of 0.453-M NaOH. Calculate the maximum mass, in grams, of Fe(OH)3 that will precipitate. Determine which reactant is in excess. Calculate the concentration of the excess reactant remaining in solution after the maximum mass of Fe(OH)3 has precipitated.
Saccharin (C7H5NO3S) is sometimes dispensed in tablet form. Ten tablets with a total mass of 0.5894 g were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of BaSO4 obtained was 0.5032 g. What is the average mass of saccharin per tablet? What is the average mass percent of saccharin in the tablets?
Sodium bicarbonate and acetic acid react according to the equation NaHCO3(aq) + CH3CO2H(aq) NaCH3CO2(aq) + CO2(g) + H2O(l) What mass of sodium acetate can be obtained from mixing 15.0 g of NaHCO3 with 125 mL of 0.15 M acetic acid?
A 10.00-mL sample of a 24.00% solution of ammonium bromide (NH4Br) requires 23.41 mL of 1.200 molar silver nitrate (AgNO3) to react with all of the bromide ion present. (a) Calculate the molarity of the ammonium bromide solution. (b) Use the molarity of the solution to find the mass of ammonium bromide in 1.000 L of this solution. (c) From the percentage concentration and the answer to part b, find the mass of 1.000 L ammonium bromide solution. (d) Combine the answer to part c with the volume of 1.000 L to express the density of the ammonium bromide solution (in g/mL).
One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?
Glycerol (C3H8O3) is commonly used as an additive to moisturizers. The amount of glycerol added can be determined by titration with permanganate in basic solution. 14MnO4(aq)+C3H8O3(aq)+20OH(aq)14MnO42(aq)+3CO32(aq)+14H2O How many milliliters of 6.15 M KMnO4 are required to completely react with 7.25 mL of an aqueous solution of glycerol (d=1.144g/mL) that is 51.6% by mass?
A 8.50 g sample of KCl is dissolved in 66.0 mL of water. The resulting solution is then added to 72.0 mL of a 0.280 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution.
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?

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a. Calculate [Na] (the molarity of sodium ion) when 15-mL of 0.770 M NaH2PO4 and 82-mL of 0.385 M Na₂HPO4 are mixed and diluted to a total volume of 500.0 mL. M