Question

In: Chemistry

If pH of 1 liter of a 1.0mM carbonate buffer is 7.0, what is actual number...

If pH of 1 liter of a 1.0mM carbonate buffer is 7.0, what is actual number of moles of H2CO3 and HCO3? (pk=6.37)

Solutions

Expert Solution

pH ofacidic buffer = pka + log(salt/acid)

    7 = 6.37 + log(HCO3^-/H2CO3)

HCO3^-/H2CO3 = 4.266

salt = HCO3^-

Acid = H2CO3

HCO3^-/H2CO3 = 4.266

TOtal no of mol of buffer = 1*1 = 1*10^-3 mol

No of mol of acid(H2CO3) = x

TOtal no of mol of buffer = H2CO3 + HCO3^-

                                          = x+4.266x = 10^-3

                           x = 0.00019 mol

No of mol of acid(H2CO3) = x = 0.00019 mol

No of mol of salt(HCO3^-) = (10^-3)-x

                            = (10^-3) - (0.00019)

                            = 0.00081 mol


Related Solutions

Buffer 1) 100 mL of 0.50 M sodium phosphate buffer, pH 7.0 MW; 137.99
Buffer 1) 100 mL of 0.50 M sodium phosphate buffer, pH 7.0 MW; 137.99
The solubility of magnesium carbonate is highest in a buffer solution with a pH of :...
The solubility of magnesium carbonate is highest in a buffer solution with a pH of : a)3.5 b)8.5 c)6.5 d)10.5 Please explain how you come to the conclusion.
A carbonic acid/carbonate buffer is used. Explain the action of said buffer in resisting pH changes...
A carbonic acid/carbonate buffer is used. Explain the action of said buffer in resisting pH changes after the addition of NaOH using relevant chemical equations and Le Chateliers Principle. Thank you.
A liter of 0.050M pH 7.10 potassium phosphate buffer is needed for a certain experiment.
1)         A liter of 0.050M pH 7.10 potassium phosphate buffer is needed for a certain experiment.             The following four methods were proposed for the preparation of the buffer. Using the pKa             value given in your textbook, which of these methods should be used and what is wrong             with the other proposals? Letter of method which should be used: __________________________ (A)      A 0.050M sample of K2HPO4 was dissolved in about 800.0mL of water, and the pH was                         adjusted to 7.10 using...
A liter of 0.050M pH 7.10 potassium phosphate buffer is needed for a certain experiment. The...
A liter of 0.050M pH 7.10 potassium phosphate buffer is needed for a certain experiment. The following four methods were proposed for the preparation of the buffer. Using the pKa value given in your textbook, which of these methods should be used and what is wrong with the other proposals? Letter of method which should be used: __________________________ (2 points) (A) A 0.050M sample of K2HPO4 was dissolved in about 800.0mL of water, and the pH was adjusted to 7.10...
One liter of a 0.1M Tris buffer (pKa=8.3) is adjusted to a pH of 2.0. A)...
One liter of a 0.1M Tris buffer (pKa=8.3) is adjusted to a pH of 2.0. A) What are the concentrations of the conjugate base and weak acid at this pH? B) What is the pH when 1.5mL of 3.0M HCl is added to this buffer? Is Tris a good buffer at this pH? Why? C) What is the pH when 1.5mL of 3.0M NaOH is added to this buffer?
A) Consider how best to prepare one liter of a buffer solution with pH = 4.94...
A) Consider how best to prepare one liter of a buffer solution with pH = 4.94 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L...
A liter of pH 7.20 phosphate buffer is needed for a certain experiment. The Henderson-Hasselbach equation...
A liter of pH 7.20 phosphate buffer is needed for a certain experiment. The Henderson-Hasselbach equation will be sufficiently accurate for your determination of pH. The pK’s for possibly relevant phosphate species are: H3PO4 ↔ H2PO4- + H+ pK = 2.15 H2PO4- ↔ HPO4-2 + H+ pK = 7.20 HPO4-2 ↔ PO4-3 + H+ pK = 12.4 0.100 Moles of H3PO4 were dissolved in about 800 mL of water, and the pH was adjusted to 7.20 using a standardized pH...
Dissolve 1 mole of Succinic Acid into 1 Liter of water. What is the pH of...
Dissolve 1 mole of Succinic Acid into 1 Liter of water. What is the pH of the solution? What is the molarity of the protonated and depronated forms of Succinic Acid?
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH=7.0, 9.8, 11.8. Assume...
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH=7.0, 9.8, 11.8. Assume that buffer capacity is not exhausted.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT