To mimic physiological conditions in the laboratory, a phosphate buffer solution is often used. It consists of a mixture of NaH₂PO4 and Na₂HPO4 to create a 10mM phosphate buffer at pH 7.4. How many grams of each must be dissolved in 1000.0mL of water to create such a buffer? (pK₂ of NaH₂PO4 is 7.1)

To mimic physiological conditions in the laboratory, a phosphate buffer solution is often used. It consists of a mixture of NaH₂PO4 and Na₂HPO4 to create a 10mM phosphate buffer at pH 7.4. How many grams of each must be dissolved in 1000.0mL of water to create such a buffer? (pK₂ of NaH₂PO4 is 7.1)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06. (pKa = 4.76)
The pK₂ value for H₂S is 7.00. What mole ratio of KHS to H₂S is needed to prepare a buffer with a pH of 7.27? [HS] [H₂S]
Both the reactant Na2CO3 and the product NaCl are white solids. What chemical tests other than placing drops of HCl, can you use to determine Na2CO3 from NaCl and reactions will you get from each?
The pK₂ value for HCN is 9.40. Would a buffer prepared from HCN and NaCN with a pH of 7.60 be considered to be an effective buffer? A buffer in which the mole ratio of NaCN to HCN is 2.0 has a pH of 9.71. Would this buffer solution have a greater capacity for added acid ( H3O+) or added base (OH)?
The pKa of lactic acid is 3.86. What is the pH of a buffer in which the lactic acid concentration is 0.200 M and the sodium lactate concentration is 2.00 M?
A compound has an ionisable groups with a pKa of 2.6. A 200 mL volume of a 0.15 M solution of this compound had an initial pH 2.4. The concentration of the conjugate acid in the initial buffer was 0.092 M. The concentration of the conjugate base in the initial buffer was 0.058 M. What is the final pH of the buffer AFTER you added 5 mL of 1 M NaOH?
A buffer solution contains 0.89 mol of hypoiodous acid (HIO) and 0.57 mol of sodium hypoiodite (NaIO) in 3.40 L.The Ka of hypoiodous acid (HIO) is Ka = 2.3e-11.(a) What is the pH of this buffer?pH = (b) What is the pH of the buffer after the addition of 0.17 mol of NaOH? (assume no volume change)pH = (c) What is the pH of the original buffer after the addition of 0.24 mol of HI? (assume no volume change)pH =
A chemistry graduate student is given 100. mL of a 1.70M diethylamine ((C2H5)2NH): NH solution. Diethylamine is a weak base with K = 1.3 × 10³. What mass of (C₂Hs)2NH2Br should the student dissolve in the (C2H3)2NH solution to turn it into a buffer with pH = 11.12? You may assume that the volume of the solution doesn't change when the (C2H5)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10
A student wishes to make a buffer that has a pH of 4.65. The student has HNO2 and NaNO2. Nitrous Acid (HNO2) has a pKa of 3.40 What would the pH of the buffer be if the Molarity of the acid and conjugate base in the solution was equal.
A formic acid buffer solution contains 0.18 M HCOOHHCOOH and 0.13 M HCOO−HCOO− . The pKa of formic acid is 3.75. What is the pH of the buffer?
3. A buffer is prepared by adding 0.50 mol of acetic acid (HC₂H3O₂) and 0.75 mol of sodium acetate (NaC₂H302) to enough water to form 2.00L solution. (pKa for acetic acid is 4.74) Calculate the pH of the buffer.
Kk.314.