Question

In: Chemistry

How many mL pf 1.07 M HClO4 should be added to 1.00 g of imidazole (C3H4N2;...

How many mL pf 1.07 M HClO4 should be added to 1.00 g of imidazole (C3H4N2; MW= 68.077 g/mol), a weak organic base (pKb= 6.95), to give a pH of 7.993?

Solutions

Expert Solution

Number of moles of imidazole(C3H4N2) in 1g can be calculated as follows:

Moles of C3H4N2 = 1.00 g C3H4N2 x (1 mole C3H4N2 / 68.077 g C3H4N2) = 0.0147 moles C3H4N2.

--------------------------------------------------------------------------------------------------------------------------------------------------

Addition of strong acid HClO4 to weak bases imidazole (C3H4N2) creates a buffer. The moles of protonated imidazole(C3H4N2H+) formed in the buffer by addition of HClO4 can be calculated by using Henderson-Hasselbalch’s equation as follows:

pH = pKa + log (moles C3H4N2 / moles C3H4N2H+)

pH = (14 – pKb) + log (moles C3H4N2 / moles C3H4N2H+)

7.993 = (14 – 6.95) + log (moles C3H4N2 / moles C3H4N2H+)

7.993 = 7.05 + log (moles C3H4N2 / moles C3H4N2H+)

7.993 – 7.05 = log (moles C3H4N2 / moles C3H4N2H+)

0.943 = log (moles C3H4N2 / moles C3H4N2H+)

10^0.943 = (moles C3H4N2 / moles C3H4N2H+)

8.770 = (moles C3H4N2 / moles C3H4N2H+)

moles C3H4N2 = 8.770 (moles C3H4N2H+)-----------------(1)

Since, initial amount of (C3H4N2) = 0.0147 = (moles C3H4N2) + (moles C3H4N2H+)

Therefore, (moles C3H4N2H+) = 0.0147 - (moles C3H4N2)

Substitute eq 1 in above equation

(moles C3H4N2H+) = 0.0147 - (8.770 (moles C3H4N2H+))

(moles C3H4N2H+) + (8.770 (moles C3H4N2H+))= 0.0147

9.770 (moles C3H4N2H+) = 0.0147

(moles C3H4N2H+) = 0.0147 / 9.770 = 0.00150

--------------------------------------------------------------------------------------------------------------------------------------------------------

Since, moles of C3H4N2H+ are formed by addition of HClO4.

Moles of HClO4 = moles of C3H4N2H+ = 0.00150

Molarity of HClO4 is 1.07M, hence, volume of HClO4 can be calculated as follows:

Volume of HClO4(L) = moles of HClO4 / molarity of HClO4

Volume of HClO4(L) = 0.00150 / 1.07

Volume of HClO4(L) = 0.00140 L = 1.4mL

Hence, 1.4 mL of 1.07 M HClO4 should be added to 1.00 g of imidazole to get a pH of 7.993


Related Solutions

How many milliliters of 1.00 M KOH should be added to 4.90 g of phosphoric acid...
How many milliliters of 1.00 M KOH should be added to 4.90 g of phosphoric acid (MM= 98.0g/mol) to give a pH of 11.00 when diluted to 1000 ml? (Ka1=7.11 x10-3, Ka2=6.32x10-8, Ka3=4.5x10-13)
how many ml of 1.0 M NaOH should be added to 500 ml 0.1 M acetic...
how many ml of 1.0 M NaOH should be added to 500 ml 0.1 M acetic acid in order to make a buffer of pH 5.5?
1.How many mL of 0.500 M HCl should be added to 155 mL of 0.0500 M...
1.How many mL of 0.500 M HCl should be added to 155 mL of 0.0500 M benzylamine to form a buffer with pH = 8.52? C7H7NH2 pKb = 4.35 C7H7NH2 (aq) + H+ (aq)  C7H7NH3 + (aq) This structure of benzylamine has a carbon at the junction of each line with 1 hydrogen on each 3-bonded ring C and 2 hydrogens on the C in the side chain attached to the ring carbon. Note that the N atom has...
How many mL (to the nearest mL) of 0.225-M KF solution should be added to 370....
How many mL (to the nearest mL) of 0.225-M KF solution should be added to 370. mL of 0.246-M HF to prepare a pH = 3.90 solution? Please show work, thank you in advance.
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of 1.00 M...
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of 1.00 M NaCl solution at 25.0 ° C in a calorimeter, a white precipitate of AgCl forms and the temperature of the aqueous mixture increases to 32.6 ° C. Assuming that the specific heat of the aqueous mixture is 4.18 J/(g °C), the density of the mixture is 1.00 g/mL, and the calorimeter itself absorbs a negligible amount of heat, what is ΔH in kJ/mol AgCl...
How many milliliters of 1.27 M KOH should be added to 100. mL of solution containing...
How many milliliters of 1.27 M KOH should be added to 100. mL of solution containing 10.0 g of histidine hydrochloride (His·HCl, FM 191.62) to get a pH of 9.30?
How many milliliters of 0.500 M KOH should be added to 2.38 g of oxalic acid...
How many milliliters of 0.500 M KOH should be added to 2.38 g of oxalic acid (molecular weight: 90.03, pKa1=1.46; pKa2=4.40) to give a pH of 4.50 when diluted to 250 mL?
a) How many grams of solid potassium cyanide should be added to 1.00 L of a...
a) How many grams of solid potassium cyanide should be added to 1.00 L of a 0.158 M hydrocyanic acid solution to prepare a buffer with a pH of 8.688 ? b) How many grams of solid ammonium chloride should be added to 2.00 L of a 0.171 M ammonia solution to prepare a buffer with a pH of 9.940 ?   c) Design a buffer that has a pH of 7.98 using one of the weak acid/conjugate base systems shown...
A) How many grams of solid sodium fluoride should be added to 1.00 L of a...
A) How many grams of solid sodium fluoride should be added to 1.00 L of a 0.218 M hydrofluoric acid solution to prepare a buffer with a pH of 3.847 ? grams sodium fluoride =  g. B)How many grams of solid sodium hypochlorite should be added to 0.500 L of a 0.297 M hypochlorous acid solution to prepare a buffer with a pH of6.803 ? grams sodium hypochlorite =  g. C)How many grams of solid ammonium chloride should be added to 1.50...
When 28.5 mL of 0.500 M H2SO4 is added to 28.5 mL of 1.00 M KOH...
When 28.5 mL of 0.500 M H2SO4 is added to 28.5 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.)
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT