A bioengineer preparing cells for cloning bathes a small piece of rat epithelial tissue in a TRIS buffer (pKb36.01, formula is (HOCH2)3CNH2). The buffer is made by dissolving 36.762 g of TRIS in enough of 0.104 M HCI to make 1.32 L of solution. What is the pH of the buffer? Record your answer with 2 decimals.

A bioengineer preparing cells for cloning bathes a small piece of rat epithelial tissue in a TRIS buffer (pKb36.01, formula is (HOCH2)3CNH2). The buffer is made by dissolving 36.762 g of TRIS in enough of 0.104 M HCI to make 1.32 L of solution. What is the pH of the buffer? Record your answer with 2 decimals.

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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A frequently used buffer in biological systems, including IV fluids, is a phosphate buffered saline solution (“PBS”), which contains 8.00 g of NaCl buffered with 1.44 g of Na2HPO4.2H2O and 0.24 g of KH2PO4 and per liter of solution. What is its pH?
A 50.0-mL solution of 0.100 M propanoic acid (HC3H5O2; Ka= 1.34 x 10–5) is titrated with 0.200 M NaOH solution. The net ionic equation for the reaction is as follows: HC3H5O2(aq) + OH–(aq) --> C3H5O2–(aq)+ H2O (a) What is the initial pH of the acid solution? (b) Calculate the pH of the resulting solution after each of the following amount of 0.200 M NaOH has been added, and the limiting reactant is completely reacted. (i) 10.0 mL of 0.200 M NaOH; (ii) 15.0 mL of 0.100 M NaOH; (iii) 20.0 mL of 0.100 M NaOH; (iv) 25.0 mL of 0.100 M NaOH; (v) 30.0 mL of 0.200 M NaOH
Consider a buffer solution that contains 0.40 M C6H4(CO2H)2 and 0.25 M C6H4(CO2H)(CO2K). pKa(C6H4(CO2H)2)=2.95. Calculate its: a)pH, the change in pH if 0.160 g of solid NaOH is added to 200 mL of this solution. b)If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.
If 0.626 g of an unknown monoprotic acid was used to prepare a 25.00 mL weak acid solution and this solution is titrated with 0.489 M NaOH, what is the molar mass (g/mol) of the unknown acid if 17.19 mL of the NaOH solution was required to reach the equivalence point?
A buffer solution is made that is 0.488 M in H2CO3 and 0.488 M in KHCO3. If Ka1 for H2CO3 is 4.20x10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.124 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O^+ instead of H^+) + +
A bioengineer preparing cells for cloning bathes a small piece of rat epithelial tissue in a TRIS buffer . The buffer is made by dissolving 43.0 g of TRIS (pKb= 5.91) in enough 0.095 M HCl to make 1.00 L of solution. What is the molarity of TRIS and the pH of the buffer?
A buffer, consisting of H2PO4 - and HPO4 2 -, helps controlthe pH of physiological fluids. Many carbonated soft drinksalso use this buffer system. What is the pH of a soft drinkin which the major buffer ingredients are 6.5 g of NaH2PO4and 8.0 g of Na2HPO4 per 355 mL of solution?
Human blood contains one buffer system based on phos-phate species and one on carbonate species. Assuming that blood has a normal pH of 7.4, what are the principal phosphateand carbonate species present? What is the ratio of the two phosphate species? (In the presence of the dissolved ions andother species in blood, Kₐ₁of H₃PO4=1.3X10⁻², Kaₐ₂=2.3X10⁻⁷, and Kₐ₃=6X10⁻¹²; Kₐ₁ of H₂CO₃=8X10⁻⁷ and Kₐ₂=1.6X10⁻¹⁰.)
A chemistry graduate student is given 100.mL of a 0.40M trimethylamine ((CH3)3N) solution. Trimethylamine is a weak base with =Kb×7.410−4. What mass of (CH3)3NHCl should the student dissolve in the (CH3)3N solution to turn it into a buffer with pH =10.35? You may assume that the volume of the solution doesn't change when the (CH3)3NHCl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
Consider the 25.0 mL portion of pH=4.45 buffer solution prepared as described in question 4. Calculate the buffering capacity of it for the hydrochloric acid of known concentration (M = 0.123 mol/L). Hint: you are calculating how much of the strong acid (HCl in this case) you can add to the buffer portion before you see a significant pH change, so start with deciding which component of the buffer will be the buffering species against the strong acid. Then calculate how much of that species is present in the 25.0 mL portion of this buffer. For the sake of these calculations, consider the buffering capacity to be the maximum volume of the strong acid that can be added to the portion of your buffer before the buffering species in it is completely used up, and the buffer is ‘overwhelmed’. Provide the answer in millilitres, mL. Don't include units.
2.50 g of sodium acetate, CH3COONa was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was added into the above salt solution. Calculate the pH of the mixed solution. [pKa of CH3COOH = 4.75, Molar mass of CH3COONa = 82.0 g mol-1 ]
Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. a.State whether the solution at the equivalence point of the titration is acidic, basic, or neutral. Explain your reasoning. b.How many mL of 0.25 M NaOH need to be added in order to make the ideal buffer solution?