1. Tris(hydroxymethyl)aminomethane abbreviated as Tris or TRIZMA is frequently used to make buffers in biochemistry laboratories. Tris has a Molecular weight 121.1 g/mol and its solution in water is basic with pH = 10.5. Describe in details how to prepare 1L of 0.5 M Tris buffer solution at pH 7.5. %3D

1. Tris(hydroxymethyl)aminomethane abbreviated as Tris or TRIZMA is frequently used to make buffers in biochemistry laboratories. Tris has a Molecular weight 121.1 g/mol and its solution in water is basic with pH = 10.5. Describe in details how to prepare 1L of 0.5 M Tris buffer solution at pH 7.5. %3D

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.128QE

See similar textbooks

Similar questions

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.)
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
A solution prepared by dissolving 2.25 g HA (MW = 51.0) and 4.00 g of NaA in 500 mL of solution has a pH of 6.02 . Calculate the Ka of the acid
1. Calculate the pH of a buffer solution that is 0.20 M in sodium hypobromite (NaBrO) and 0.10 M in hypobromous acid (Ka of HBrO= 2.5 ×10−9) a 4.15 b 4.45 c 8.60 d 8.90 e 8.30 2. A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa). [Ka= 1.8 ×10–5] What is the new concentration of CH3COOH after buffering? a. 0.2437 b. 0.2014 c. 0.1615 d. 0.3213 e. 0.2589 3. A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa). [Ka= 1.8 x 10–5] What is the new concentration of NaOH after dilution? a 0.0273 b 0.0439 c 0.0185 d 0.0267 e 0.0385
A solution of nitric acid, HNO2, at a concentration of 0.495M was found to be 1.83 = pH. A. Calculate the concentration [H3O(aq)+] And the ionization percentage of the nitric acid. ShowCalculations. B. Write the expression for the existing equilibrium in the solution and calculate the value of Ka ofNitric acid. Show calculations. C. Calculate the pH of the resulting solution by adding 0.1 g of NaNO2 to750 ml of HNO2 solution 0.0125M. Show calculations. D. Schematically plot the titration curve of 20.0 mL HNO2 0.0125MWhich is purged with NaOH 0.0125M while specifying the names of the axes. Marked on topThe curve the buffer area and the equivalent point. Detail the calculationsWhich led to the drawing of the curve.
1. a. A 250.0ml of a solution of the strong base, CsOH(MW = 150.0 g/mole) is made. The pH is measured to be 8.90. What mass of cesium hydroxide is present in the solution? b. The surface of Venus is quite inhospitable with an average temperature of 450 ̊C and a pressure of 92 atm (earth). Under these delightful conditions, the pKw of water is estimated to be 24. What is the pH of neutral water on Venus? c. An aqueous acetic acid (HOAc) solution is 1.00 % dissociated. What will the concentration of H3O+ be if 0.82 g of sodium acetate (NaO2C2H3) is added to 100.mL of solution? d. PICTURE ATTACHED Glutaric Acid is a diprotic organic acid with a molecular formula of H2C5H6O4, and a molecular weight of 132.12 g/mol. The stepwise acid dissociation reactions and the Ka values are given below. An aqueous solution is prepared by dissolving 1.02 g of glutaric acid in water to form 500.0 ml of solution. Calculate the pH, [H2C5H6O4], [HC5H6O4–], and[C5H6O42–] after the solution has reached…
3..A 10 mL solution of 0.38 M HA (pKa = 4.40) is mixed with 8.0 mL of 0.38 M KOH. What is the pH of the solution? The tolerance for this question is set to ±0.01.
Phosphorous acid (H3PO3) has the Lewis structure shown at right.(a) Explain why H3PO3 is diprotic and not triprotic. (b) A 25.0-mL sample of an H3PO3 solution titrated with 0.102 M NaOH requires 23.3 mL of NaOH to neutralize both acidic protons. What is the molarityof the H3PO3 solution? (c) The original solution from part (b) has a pH of 1.59. Calculate the percentionization and Ka1 for H3PO3, assuming that Ka1 >> Ka2. (d) How does the osmotic pressure of a 0.050 M solution of HCl compare qualitatively with that of a 0.050 M solution of H3PO3? Explain.
A chemist takes a liter of 1.25M H2SO4 and adds 1.00 mole of solid KOH. The addition of solid does not add appreciably to the solution's volume. What is the pH? (Ka of HSO4- = 0.012)
HZ is a weak acid. An aqueous solution of HZis prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0L of solution. The pH of the solution was 4.93 at 25.0 degree C. The Ka of HZ is?
Carbonate and bicarbonate can be combined to form a buffer system. How many grams of magnesium carbonate would have to be dissolved in 750.0 mL of a 0.1330 M bicarbonate solution to prepare a solution with a pH of 9.33? (Ka of bicarbonate is 4.7 X 10 -11)
A buffer solution was prepared by dissolving 0.04 mol Na2HPO4(s) and 0.02 molNaH2PO4(s) in water and diluted to a total volume of 1.0 L. 1. What are the buffering molecules in this solution? Also state whether they act as acid orbase.2. What will be the concentration of the buffer? Report your calculations.3. Calculate the pH of the buffer solution. (K =5*10-8 ). Show your calculations4. How does the pH in the buffer change when 1 mmol NaOH is added? Show calculations.