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Chapter 9: QIE (page 207)

A solution contains 63 different conjugate acid-base pairs.

Among them is acrylic acid and acrylate ion, with the equilibrium ratio [acrylate]/[acrylic acid]5 0.75. What is the pH of the solution?

H2C=CHCO2HpKa=4.25

Short Answer

Expert verified

The pH of the solution using Henderson-Hasselbalch equation and was found to be 4.13

Step by step solution

01

Step 1: Define the term Henderson-Hasselbalch Equation.

Equation of Henderson-Hasselbalch. pH, pKa, and molar concentration (concentration in moles per litre) are all linked by the Henderson-Hasselbalch equation: apH=logA-/HA+pK a The molar concentration of a conjugate base isA-.HA= molar concentration of a weak acid that has not been dissociated (M).

02

Calculate the ph of the solution.

Equilibrium ratio=0.75

pKa=4.25

The pHof the solution can be calculated as,

role="math" localid="1654769713942" pH=pKa+logA-HApH=4.25+log0.75pH=4.13

The pH of the solution=4.13

The pH of the solution using Henderson-Hasselbalch equation and was found to be 4.13.

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Most popular questions from this chapter

Which of the following bases would be most suitable for preparing a buffer of pH9.00?

(i) NH3(ammonia,Kb=1.76脳10-5);

(ii) role="math" localid="1654764490555" C6H5NH2(aniline,role="math" localid="1654764515634" C6H5NH2 );

(iii)H2NNH2(hydrazine,Kb=1.05脳10-6)));

(iv) C6HsNH2(pyridine,Kb=1.58脳10-9) ).

Calculate the pH of a solution prepared by mixing 0.0800mol of chloroacetic acid plus0.0400mol of sodium chloroacetate in1.00L of water.

(a) First do the calculation by assuming that the concentrations of HA andA- equal their formal concentrations.

(b) Then do the calculation, using the real values of and in the solution.

(c) Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of1.00L:0.180molCICHCOO2H,0.020molCICHCHO2Na20.080molHNO3,and0.080molCa(OH)2. Assume thatCa(OH)2 dissociates completely.

(a) Write the chemical reactions whose equilibrium constants areKband Kafor imidazole and imidazole hydrochloride respectively.

(b) Calculate the pH of a solution prepared by mixing 1.00gof imidazole with 1.00gof imidazole hydrochloride and diluting torole="math" localid="1655093511290" 100.0mL .

(c) Calculate the pH of the solution if 2.30mLof 1.07MHCIO4are added.

(d) How many milliliters of1.07MHCIO4should be added to of imidazole to give a pH ofrole="math" localid="1655093364034" 6.993?

Barbituric acid dissociates as follows:

(b)Calculate the pH and fraction of dissociation of 10-10.00 M barbituric acid.

Select a compound from Table 9-2 that you could use to make 250mLof 0.2Mbuffer with a pH of 6.0. Explain how you would make the buffer.
See all solutions

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