A mixture is prepared using 27.00 mL of a 0.0774 M weak base (pKa = 4.635),...

A mixture is prepared using 27.00 mL of a 0.0774 M weak base (pKa = 4.635), 27.00 mL of a 0.0581 M weak acid (pKa = 3.189) and 1.00 mL of 0.000116 M HIn and then diluting to 100.0 mL, where HIn is the protonated indicator. The absorbance measured at 550 nm in a 5.000 cm cell was 0.1123. The molar absorptivity (ε) values for HIn and its deprotonated form In– at 550 nm are 2.26 × 104 M–1cm–1 and 1.53 × 104 M–1cm–1, respectively. 1.) What is the pH of the solution? 2.)What are the concentrations of In– and HIn? respectively 3.)What is the pKa for HIn?

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A mixture is prepared using 26.00 mL of a 0.0706 M weak base (pKa = 4.591),...

A mixture is prepared using 26.00 mL of a 0.0706 M weak base (pKa = 4.591), 26.00 mL of a 0.0530 M weak acid (pKa = 3.259) and 1.00 mL of 0.000114 M HIn and then diluting to 100.0 mL, where HIn is the protonated indicator. The absorbance measured at 550 nm in a 5.000 cm cell was 0.1227. The molar absorptivity (ε) values for HIn and its deprotonated form In– at 550 nm are 2.26 × 104 M–1cm–1 and...

Weak acid with strong base: 25 mL of 0.1 M HCOOH with 0.1 M NaOH (pka...

Weak acid with strong base: 25 mL of 0.1 M HCOOH with 0.1 M NaOH (pka = 3.74) pH after adding following amounts of NaOH 18) 0 mL of NaOH 19) at half equivalence point 20) after adding 25 mL NaOH

For the titration of 25 ml of a 0.025 M weak acid solution (pKa = 4.615)...

For the titration of 25 ml of a 0.025 M weak acid solution (pKa = 4.615) with 0.050 M NaOH. What will be the pH and pOH at the Equivlance point?

Formic acid is a weak acid with pKa = 3.75. How many mL of 0.10 M...

Formic acid is a weak acid with pKa = 3.75. How many mL of 0.10 M NaOH solution should be added to 100.0 mL of 0.10 M formic acid solution to make a buffer solution with pH = 3.27 A) 0 B) 25 C) 50 D) 75 E) 100

Given: 50 ml of 0.2 M weak acid is titrated with 0.2M NaOH. The pka of...

Given: 50 ml of 0.2 M weak acid is titrated with 0.2M NaOH. The pka of the acid is 4.7 1. What is the pH at the equivalence point? 2. What is the ph when 60ml of NaOH is added? (Total Amt of NaOH is 60ml) 3. What is the pH when 10ml of NaOH is added? 4. What would be the approximate ph of a 0.1 M NaCl solution?

A mixture is prepared by combining 3.0 mL of 0.0050 M NaSCN solution with 4.0 mL...

A mixture is prepared by combining 3.0 mL of 0.0050 M NaSCN solution with 4.0 mL of 0.0030 M Fe(NO3)3 solution, and 3.0 mL of 0.10 M HNO3 a). if Keq = 405, determine the equilibrium concentration of FeSCN2+ in the solution. (keep 4 decimal places) b). if Keq=282, determine the equilibrium concentration of Fe3+ in the solution. (keep 4 decimal places) c). if Keq = 343, determine the equilibrium concentration of SCN-- in the solution. (keep 4 decimal places)

The ratio for ( ionized /unionized ) for weak base (Pka = 10.4 ) in blood...

The ratio for ( ionized /unionized ) for weak base (Pka = 10.4 ) in blood (ph = 7.4) Will be ??

You have 25.00 mL of a 0.22 M of a weak base, anline C6H5NH2 with a...

You have 25.00 mL of a 0.22 M of a weak base, anline C6H5NH2 with a Kb= 3.94 x 10 ^-10.it is to be titrated with 0.20 M HCl. What is the resulting solution after the following additions? a) intial pH b) after 10.05mL HCl have been added. c) 1/2 way to the equivalence point. d) At the equvalence point. e) 5.0mL after the equivalence point f) what indicator would you use to signal the endpoint and why?

Calculate the pH for 200. mL of a 0.750 M solution of the weak base, ethanolamine...

Calculate the pH for 200. mL of a 0.750 M solution of the weak base, ethanolamine (HOCH2CH3NH2), Kb=3.20x10-5 ) being titrated with 0.750 M HCl at the following positions in the titration. a) The initial pH (before any HCl has been added). a. 2.300 b. 3.542 c. 8.945 d. 11.690 e. 13.976 b) The pH of the solution after 75.0 mL of 0.750 M HCl has been added. a. 0.769 b. 9.727 c. 3.564 d. 8.654 e. 13.230 c)The pH...

A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate...

A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). a) pH = 4.56 b) pH= 5.28 c) pH= 4.74

Subjects