ZuoTi.Pro
Question

6). TrisHCl is an organic buffering compound that forms an equilibrium with its conjugate base (TrisCl-) according to th...

6). TrisHCl is an organic buffering compound that forms an equilibrium with its conjugate base (TrisCl-) according to the following equilibrium.
TrisHCl TrisCl- + H+ pKa= 8.1 -

  1. (i) In a solution which has a pH=8 what are molar ratios of TrisCl of TrisHCl l?

  2. (ii) If the above solution which has a total Tris concentration ([TrisHCl] + [TrisCl-] =

    1 mol L-1) of 1 mol L-1 what are the concentrations of TrisHCl and TrisCl?

  3. (iii) What masses of TrisHCl and TrisCl are required to make a 1L solution with these

    calculated concentrations?

Molecular weight of TrisHCl= 157.6 g mol-1

Molecular weight of TrisCl- = 121.14 g mol-1

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Lo T A Lo 、ヲ la) lina 7つ 21 /y 0.4し

0 0
Add a comment
Know the answer?
Add Answer to:
6). TrisHCl is an organic buffering compound that forms an equilibrium with its conjugate base (TrisCl-) according to th...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • 1) Solution Components A 1 mL 100 mM NaH2PO4 + 9 mL 100 mM Na2HPO4 B...

    1) Solution Components A 1 mL 100 mM NaH2PO4 + 9 mL 100 mM Na2HPO4 B 5 mL 100 mM NaH2PO4 + 5 mL 100 mM Na2HPO4 C 9 mL 100 mM NaH2PO4 + 1 mL 100 mM Na2HPO4 D 10 mL 100 mM NaH2PO4 stock solution E 10 mL 100 mM Na2HPO4 stock solution F 10 mL distilled water pKa of phosphate: 6.8 How would you calculate the pH of each equation using the Henderson Hasselbalch equations? 2) Tris...

  • A cyclohexane (c-hex) solution is prepared by fully dissolving 9.11g of a newly synthesized organic compound...

    A cyclohexane (c-hex) solution is prepared by fully dissolving 9.11g of a newly synthesized organic compound in 100.g cyclohexane. The freezing point of the solution is depressed by -5.80 oC from the normal freezing point of 6.55 oC for pure cyclohexane ( Kf,c-hex= 20.0 oC kg/mol , MWc-hex = 84.0 g/mol). (a) What is the molecular weight (molar mass) of the organic compound? (b) What is the vapor pressure of the cyclohexane for this solution at 298K?

  • 1. Identify the Brönsted acid and base in the following reaction, and identify the conjugate base...

    1. Identify the Brönsted acid and base in the following reaction, and identify the conjugate base and acid formed. HSO3-(aq) + CH3NH3(aq) ------ H2SO3(aq) + CH3NH2(aq) 2. Write the formulae for the conjugate acids of: 1. a) C2042: the oxalate ion. 2.b) C6H5NH2, aniline. 3.c)NH2OH, hydroxylamine. (Use above question as a guide for where to put the H.) 3. Calculate the molarity of OH' in solutions with the following concentrations of H30*: a) 0.020 mol LP b) 1.0 x 10-5...

  • 1. in run 1, you mix 8.1 mL of the 43 g/L MO solution (MO molar...

    1. in run 1, you mix 8.1 mL of the 43 g/L MO solution (MO molar mass is 327.33 g/mol), 2.89 mL of the 0.040 M SnCl22 in 2 M HCl solution, 5.46 mL of 2.0M HCl solution, and 3.47 mL of 2.0M NaCl solution. What is the [MO]? a. In run 1, you mix 8.1 mL of the 43 g/L MO solution (MO molar mass is 327.33 g/mol), 2.89 mL of the 0.040 M SnCl22 in 2.0 M HCl...

  • p-dichlorobenzene is an organic molecular (covalent) compound with i = 1 and Kf = 7.10 oC/m...

    p-dichlorobenzene is an organic molecular (covalent) compound with i = 1 and Kf = 7.10 oC/m A student weighed 11.20 mL of p-dichlorobenzene and recorded mass of it as 10.820 g. The freezing point of the pure p-dichlorobenzene liquid was determined as 53.1 oC. 1.118 g of an unknown solid compound was added and completely dissolved in the previous sample of pure p-dichlorobenzene liquid. The freezing point determination procedure was conducted for the solution and the freezing point of this...

  • 1. Calculate the masses of the conjugate acid and base needed to prepare each of t...

    1. Calculate the masses of the conjugate acid and base needed to prepare each of t listed in the table on the left. (pKa of H,PO 6.70) Assume the availability of the phosphate salf listed in the table on the right. Fill out the worksheet below. Show all work on separate pages for full credit. кн-РО,/К, НРО, mol NaH,PO/Na2HPO Molar mass (g Salt (0.25 M, 100 mL) (0.25 M, 100 mL) 136.09 кн, РО, K2HPO NaH,PO H2O Na,HPO 7 H2O...

  • An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume...

    An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. What is the effect of adding 0.50 mol CH3CO2–(aq) to this solution? 1. The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2. Some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2–(aq) and increasing the concentration of H+. 3. Some CH3CO2–(aq) will react with H+, increasing the concentration of...

  • 5. The equilibrium constant, KcKc, is calculated using molar concentrations. For gaseous reactions another form of...

    5. The equilibrium constant, KcKc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, KpKp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol)R=0.08206 L⋅atm/(K⋅mol), TT is the absolute temperature, and ΔnΔn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2 For the reaction 3A(g)+2B(g)⇌C(g) KcKc...

  • The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...

    The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)?n where R=0.08206 L?atm/(K?mol), T is the absolute temperature, and ?n is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)?2NH3(g) for which ?n=2?(1+3)=?2. Part A For the reaction 3A(g)+3B(g)?C(g) Kc...

  • The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...

    The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. A) For the reaction 3A(g)+3B(g)⇌C(g) Kc =...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT