Calculate the volume (in mL) of a 0.370 M KOH solution that should be added to 4.000 g of HEPES (MW=238.306 g/mol, pKa...
Homework Answers
The Henderson-Hassebalch equation is used to determine the pH of a buffer and the concentration of an acid and base.
Using this equation, the initial volume of the acid or base can be found with the given information
The Henderson-Hassebalch equation is as follows:
![pH = pK, +log 3
where,
TA] = molar concentration of conjugate base
[HA] = molar concentration of a undissociated weak acid
PK](http://img.homeworklib.com/questions/3f672e40-12ab-11ea-a624-358d4f1baefa.png?x-oss-process=image/resize,w_560)
Related formulae:
The volume of KOH in mL = 16.57mL
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Calculate the volume (in mL) of a 0.370 M KOH solution that should be added to 4.000 g of HEPES (MW=238.306 g/mol, pKa...
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Assignment Score: 681/3200 Resources int Check Answer Question 14 of 32 > Calculate the volume, in milliliters, of a 0.380 M KOH solution that should be added to 4.750g of HEPES (MW - 238.306 g/mol, pk, = 7.56) to give a pH of 7.46. KOH volume =
A 100.0 mL solution containing 0.852 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.277 M KOH. Calculate the pH of the solution after the addition of 53.0 mL of the KOH solution. Maleic acid has pK, values of 1.92 and 6.27. pH = -.57 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 H, M, HMⓇ, and M2-, which...
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A 100.0 mL solution containing 0.956 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.350 M KOH. Calculate the pH of the solution after the addition of 47.0 mL of the KOH solution. Maleic acid has pKa 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 H,M, HM, and M2, which represent the fully...
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