The sidechain thiol of the amino acid cysteine has a pKa value of 8.37. Ka=4.26E-9 Give...
The sidechain thiol of the amino acid cysteine has a pKa value of 8.37.
Ka=4.26E-9
Give the standard free energy change for the sidechain acting as an acid at 30 degrees C.
If the pH of the solution is 7.6, what is the [H3O+] in solution?
If the pH of the solution is 9.8000000000, what fraction of deprotonated to protonated cysteine sidechains will exist in solution?
What is the concentration of protonated cysteine sidechains if the pH of the solution is 6.2000000000 and the solution contains 10.0000000000 mM of total cysteine?
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The sidechain thiol of the amino acid cysteine has a pKa value
of 8.37.
Ka=4.26E-9
Give...
20. Properties of a Buffer The amino acid glycine is often used as the main ingredient...
20. Properties of a Buffer The amino acid glycine is often used as the main ingredient of a buffer in biochemical experi- ments. The amino group of glycine, which has a pKa of 9.6, can exist either in the protonated form (-NH3 or as the free base (-NH2), because of the reversible equilibrium (a) In what pH range can glycine be used as an effective buffer due to its amino group? (b) In a 0.1 M solution of glycine at...
Alanine (H2NCH(CH3) is a common amino acid that has a basic amino group. A) Write an...
Alanine (H2NCH(CH3) is a common amino acid that has a basic amino group. A) Write an equilibrium for the reaction of alanine acting as a Bronsted base with a water molecule. (Ka of protonated amino group = 1.349 x 10 -10 B) Calculate the Kb of the amino group C) Calculate the pOH of a 0.025M solution of alanine in water D) Calculate the pH value of a 0.025M solution of alanine in water E) Describe how the equilibrium would...
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O โ H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) โ 2 HI(g)
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Acetic Acid (CH3COOH) has a Ka value of 8 x 1-5. If I have a 0.15 M acetic acid solution, what are the following values? pH pOH [H3O+] [OH-] If I add 0..15 M sodium acetate to the solution what is the pH value here? Remember that pH = pKa + log [A-]/[HA].
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20. Properties of a Buffer The amino acid glycine is often used as the main ingredient of a buffer in biochemical experi- ments. The amino group of glycine, which has a pKa of 9.6, can exist either in the protonated form (-NH3 or as the free base (-NH2), because of the reversible equilibrium (a) In what pH range can glycine be used as an effective buffer due to its amino group? (b) In a 0.1 M solution of glycine at...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O โ H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) โ 2 HI(g)
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