Part AAs a technician in a large pharmaceutical research firm, you need to produce 100. mL of 1.00 mol L potassium phosphate buffer solution of pH = 6.95. The pK, of H,PO, is 7.21.You have the following supplies: 2.00 L of 1.00 mol L- KH2PO4 stock solution, 1.50 L of 1.00 mol L-1 K2HPO4 stock solution, and a carboy of pure distilled H20.How much 1.00 mol L-1 KH,PO4 will you need to make this solution?Express your answer to three significant digits with the appropriate units.• View Available Hint(s)HẢVolume of KH2PO4 needed =ValueUnitsSubmit

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Part A As a technician in a large pharmaceutical research firm, you need to produce 100. mL of 1.00 mol L- potassium phosphate buffer solution of pH= 6.95. The pK, of H2PO, is 7.21. You have the following supplies: 2.00 L of 1.00 mol L KH2PO, stock solution, 1.50 L of 1.00 mol L- K,HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 mol L-1 KH,PO, will you need to make this solution? Express your answer to three significant digits with the appropriate units. > View Available Hint(s) µA ? Volume of KH2P0, needed = Value Units Submit

Part A As a technician in a large pharmaceutical research firm, you need to produce 100. mL of 1.00 mol L- potassium phosphate buffer solution of pH= 6.95. The pK, of H2PO, is 7.21. You have the following supplies: 2.00 L of 1.00 mol L KH2PO, stock solution, 1.50 L of 1.00 mol L- K,HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 mol L-1 KH,PO, will you need to make this solution? Express your answer to three significant digits with the appropriate units. > View Available Hint(s) µA ? Volume of KH2P0, needed = Value Units Submit

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 188IP: Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid...

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What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
A solution consisting of 25.00 g NH4Cl in 178 mL of water is titrated with 0.114 M KOH. (a) How many milliliters of KOH are required to reach the equivalence point? (b) Calculate [Cl-], [K+], [NH3], and [OH-] at the equivalence point. (Assume that volumes are additive.) (c) What is the pH at the equivalence point?
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
Consider a 10.0% (by mass) solution of hypochlorous acid. Assume the density of the solution to be 1.00 g/mL. A 30.0-mL sample of the solution is titrated with 0.419 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 103 HONH2 Kb = 1.1 108 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. a. HCO2H b. HOBr c. KHCO2 d. HONH3NO3 e. (C2H5)2NH f. (C2H5)2NH2Cl g. HONH2 h. NaOBr
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?