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56. The fluids within cells are buffered by H2PO4 and HPO42- a. Calculate the ratio of HPO42-to H2PO4 required to main- tain a pH of 7.1 within a cell. b. Could a buffer system employing H3PO4 as the weak acid and H2PO4 as the weak base be used as a buffer system within cells? Explain.

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Related questions

Calculate the pH of 0.150 M solution of Na­­2HPO4 .

Know that it can act as both an acid or a base.

Am told to pick the largest Ka.

Calculated pH is 10.19.

How do I solve and get the pH of 10.19?

Also, cant use 1/2 [pkw +pka +log c ]

Acid

Ka

H3PO4

7.1 x 10-3

H2PO4-

6.3 x 10-8

HPO42-

4.5 x 10-13
  1. We want to make 250 mL of a 0.1 M phosphate buffer at pH 7.4.
    1. Given that the relevant pKa for phosphate is 7.2, useHenderson-Hasselbalch to calculate the ratio[HPO42?]/[H2PO4?].
    2. The total concentration of the buffer is the sum of the twocomponents, such that

  2. [phosphate buffer] = [HPO42?] +[H2PO4?]

    Since we want to prepare a 0.1M buffersolution. If we rearrange the above expression to solve for theconcentration of the acid and plug this into the ratio solved forin problem #1, we can solve for the concentration of the base. Whatis the concentration of the base required in our buffer to get ourdesired pH?

  3. What is the concentration of the acid required in our buffer toget our desired pH?
  4. If we want to prepare this buffer by mixing already preparedsolutions of 0.1M Na2HPO4 and 0.1MNaH2PO4, determine the volumes of each bufferrequired to make 250 mL of our 0.1M phosphate buffer of 7.4.(realize that if you mix these two solutions, and the concentrationof the buffer is equal to the sum of the acid + base, you willSTILL have a 0.1 M solution of buffer!)
1. Calculate the pH of a buffer solution made by adding 5.0g ofanhydrous sodium acetate (NaC2H3O2) to 50mL of 0.100 M acedticacid. Assume there is no change in volume on adding the salt to theacid. pKa for acetic acid is 4.7.

Buffer capacity refers to the amount of acid or base a buffer canabsorb without a significant pH change. A 0.5M buffer can absorb 5xas much acid or base as a 0.1M buffer for a given pH chnage.

You are given 60mL of 0.50M phosphate buffer, pH= 6.83. Thestarting composition of the buffer, both in terms of concentrationand molar quantity of two major phosphate species is:
Concentration of HPO4^2-= 0.304M
Concentration of H2PO4-= 0.196M
Molar quantity of HPO4^2-= 18.2 mmol
Molar quantity of H2PO4-= 11.8 mmol

a) You add 1.7 mL of 1.00 M HCL to the buffer. Calculate the molarquantity of H30+ added as HCL and the final molar quantity ofHPO4^2- and H2PO4- at equilibrium?

b) What is the new HPO4^2-/H2PO4- ratio and new pH of solution? ThepKa of H2PO4- is 6.64. Use henderson-hasselbach.

C) Now take a fresh 60mL of the 0.50M pH of 6.83 buffer and add3.7mL of 1.00M NaOH. Caclulate the new pH of the solution.

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