Purchase Solution

pH of Glycine After Addition of Acid/Base

Not what you're looking for?

Ask Custom Question

I need some help answering this questsion:
If I had 1L of a 1.0M solution of glycine at the isoelectric pH (6.02) and I added 0.3 mol of HCL, what would be the new pH? What would be the pH if I added 0.3 mol of NaOH instead of the acid?

Purchase this Solution
Solution Summary

This in-depth solution conducts step-by-step calculation to determine the new pH of the solution and also pH when 0.3 mol of NaOH is added. All formulas and workings are shown for better understanding.

Purchase this Solution
Free BrainMass Quizzes
Biochemistry Basics

A refresher quiz to test your knowledge of basics concepts of biochemistry.

BioChemistry Basics

This Quiz will test your knowledge of the amino acids used in biological systems

Parts of the Brain

This quiz will test your knowledge on different areas of the brain.

BIOLOGY

Basics in biology

Infant Development: Sleep

How much do you know about infant sleep? Test your knowledge with this quiz.

View More Free Quizzes
Related BrainMass Solutions

  • Net Electrical Charge

    We will determine the answer after we calculate the effect of each amino acid. Arginine: This is another base with an ionizable R group whose pKa is 12.48. Clearly, this will be protonated forming the =NH2+ group.

  • Calculate the isoelectric point (pI) of an amino acid

    The isoelectric point (or pI) of an amino acid is the pH at which the amino acid has a net charge of zero. Step one: Consider the ionization of the amino acid. Draw the structures of the +1, 0, and -1 charged states of each amino acid.

  • Use Reaction Equations to Describe Chemical Changes

    Explain how the buffer keeps the pH of the solution at about the same value (a) after the addition of a few drops of a dilute HCl solution and (b) after the addition of a few drops of a dilute NaOH solution.

  • Understanding buffers and weak acids.

    Simply stated, when the pH of a buffer is equal to the pKa of the weak acid, the ratio of weak acid to weak base is 1:1. In addition, the ability of a buffer to resist changes in pH is GREATEST when pH = pKa.

  • PH of a buffer system

    (a) pH=pK_a+log [base]/[acid] =-log⁡(5.75×〖10〗^(-10) )+log ((0.20))/((0.18) ) =9.240332+0.045757 =9.29 (b) Moles of NH4+ = 0.18 M × 0.070 L = 0.0126 moles Moles of NH3 = 0.20 M × 0.070 L = 0.0140 moles Upon addition of 0.10 M × 0.010

  • PH of buffer system

    What is the pH after the addition of 20.0 mL of 0.050 M NaOH to 80.0 mL of the buffer solution? pH of buffer system Calculate the pH of the 0.32 M NH3/0.35 M NH4Cl buffer system.

  • pH calculations for buffers, mixtures of acids and bases

    The ratio of weak acid to weak base was 1 when you started, and 1 after the addition of water.......since the ratio is still one, pH still equals pKa. So, the pH of a buffer doesn't change when it is diluted.

  • Determine the pH of a 1.0 L of the buffer that is 0.50 M in NH3 and 0.20 M in NH4Cl after the addition of 0.010 mol of NaOH.

    492957 Determining the pH of the Buffer Determine the pH of a 1.0 L of the buffer that is 0.50 M in NH3 and 0.20 M in NH4Cl after the addition of 0.010 mol of NaOH. Kb = 1.8 x 10^(-5) for NH3. The calculation should be in two parts.

  • Volume of an acid required to change the pH of a buffer solution

    The molar amount of NH4+ is equal to the moles of HCl added because the stoichiometric ratio of the acid-base reaction is 1:1.

View More Related Solutions