Consider the titration of TRIS, a weak base, as you carried out in lab. The conjugate acid of TRIS, TRISH has a pKa-8.06. What is the pKb of TRIS? What is the pH of a solution with 0.00300 moles of TRIS with dissolved in 50.00 mls of water? Calculate the pH upon addition of 15, 30 and 35 mls of 0.100 M HCI.

Consider the titration of TRIS, a weak base, as you carried out in lab. The conjugate acid of TRIS, TRISH has a pKa-8.06. What is the pKb of TRIS? What is the pH of a solution with 0.00300 moles of TRIS with dissolved in 50.00 mls of water? Calculate the pH upon addition of 15, 30 and 35 mls of 0.100 M HCI.

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

A 28.3 mL sample of 0.130 M formic acid (HCHO2) is titrated with 0.130 M NAOH, Calculate the pH after the addition of 28.3 mL of NaOH. (For HCHO2; Ka = 1.76 × 10–4) Hint: Determine the equivalence point so you know where you are in the titration. 6. Report your answer with 2 places past the decimal point. Type your answer...
Nitesh
A 100.0 mL solution containing 0.923 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.306 M KOH. Calculate the pH of the solution after the addition of 52.0 mL of the KOH solution. Maleic acid has pK₂ values of 1.92 and 6.27. pH = At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H₂M, HM¯, and M²-, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. [M²-] = [HM-] = [H₂M] = X- M M M
Given the following: citric acid pKa1 = 3.12, oxalic acid pKa1=1.25. Which of the following is true? a.Both acids can be used to buffer a solution at pH 4.0. b.The conjugate base of citric acid can be used as buffer at pH 8 c.Oxalic acid is a weaker acid than citric acid; d.The conjugate base of citric acid is more basic than the conjugate base of oxalic acid.
1.Why is more than one accurate titration carried out? 2.Explain why hydrochloric acid is not used as a primary standard. 3.Can any of the following be used as primary standards: NaOH, H2SO4, HNO3? Explain your answer.
MOPS is a weak acid that ionizes according the the reversibile chemical equaiton HMOPS 2 MOPS¯ + H". MOPS has a pka of 7.28. What is the resulting pH when 25mL of 2.5M HCl is added to 500mL of a 0.5M MOPS buffer at pH 7.40?
Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?
1. biology. The reagent of CHES is N-cyclohexyl-2-aminoethanesulfonic acid, a monoprotic acid, with a formula of CSH17NO:S. It has a useful pH range between 8.6 to 10. It is made by reacting with NaOH in situ. How many grams of solid CHES should be added to 100.0 mL of 0.500 M NaOH to make a buffer of pH = 9.54? Ka for CHES is 5.0 × 1010. Please note NaOH is used to make the CHES salt, and not part of HH equation. CHES buffer is a commonly used buffer system in biochemistry and molecular
HCl is a: strong acid strong base weak acid weak base NaOH is a: strong acid strong base weak acid weak base What should be the equivalence point pH be for this experiment? a. less than 7 b.equal to 7 c. greater than 7 Assume it takes 2.80 mL of 0.1100 M NaOH to titrate 5.00 mL of HCl. Calculate the concentration of HCl using this data (and show your work!)
Can someone show me how to solve this using mole and not millimoles Ka=9.12x10-5 (asorbic acid)
Please don't provide handwritten solution
[attached is the given data] Questions: 1. What is the pH of arterial blood plasma? * Do not round off the pKa. Use the complete value of the pKa in solving for the pH.