As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.80. The pKa of H₂PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 M KH₂PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. ► View Available Hint(s) Volume of KH₂PO4 needed = μÅ Value Units ?

As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.80. The pKa of H₂PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 M KH₂PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. ► View Available Hint(s) Volume of KH₂PO4 needed = μÅ Value Units ?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 54QAP: Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a...

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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.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
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
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
Part A As a technician in a large pharmaceutical research firm, you need to produce 150. mL of 1.00 mol L-1 potassium phosphate buffer solution of pH = 7.10. The pKa of H₂PO4¯ is 7.21. You have the following supplies: 2.00 L of 1.00 mol L-¹ KH₂PO4 stock solution, 1.50 L of 1.00 mol L-¹ K₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 mol L-¹ KH₂PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. ► View Available Hint(s) Volume of KH₂PO4 needed = Submit 0 μÅ Review | Constants I Periodic Table Value Units
As a technician in a large pharmaceutical research firm, you need to produce 400. mL of 1.00 M potassium phosphate buffer solution of pH = 7.05. The pKa of H2PO4− is 7.21.You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O.How much 1.00 M KH2PO4 will you need to make this solution?
3. A solution was prepared by adding 4.95 g sodium acetate (NaC;H;O2) to 250.0 mL of 0.150 M acetic acid (K = 1.75 x 10). Assume negligible volume change. a) What is the pH of the resulting solution? PH: pk2 + log CH3 02) moles saium 4.959 0.06 mol %3D 2cent %3D 82gmu H: -log (1.73x 10) + log 0.24 moles 2cete 250 x 0.15 IL :00375 1000me PH : 4 1.96 O.06 (N2 G Hs0): 0.24m 0.230 L O.0375 : CCHS COOH): 0 15 m Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to it. What is the pH of this new mixture? b)
From the following choose the most appropriate weak base (when added to its conjugate acid) for making a buffer with pH = 4.50 O (CH3)3N (K, = 6.4 x 105) %3D O CgH5NH2 (K = 3.9 x 1010) O C2H5NH2 (Kg = 5.6 x 104) O HONH2 (K, = 1.1x 108) %3D O NH3 (K5 - 1.8 x 10 5)
(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
What is the ratio of lactic acid to sodium lactate in a solution with pH = 4.00? How many grams of sodium lactate (Formula NaC3H5O3) need to be added to 1.00 L of 0.150 M Lactic acid (C3H6O3) to form a buffer with pH=4.00? pKa lactic acid = 3.86.
Calculate the pH and pOH of 440 mL of a phosphate buffer that is composed of 0.336 MHPO2 and 0.464 M PO³ at 25°C. The K₂ of HPO is 4.50 × 10-1³. 4 4 4 Report your answer to 3 sig figs. pH = 0.4785 pOH = 0.3279 РОН X X