Assume you have successfully made a buffer solution, such that you have 0.250 M phosphate buffer...

Assume you have successfully made a buffer solution, such
that you have 0.250 M phosphate buffer at pH 7.2. You dissolve in this solution sufficient
histidine (side chain pKa = 6.0), such that the final histidine concentration is 5 mM, all at 25°C.
Therefore, the pH of the solution is controlled by the phosphate buffer. In this solution, what is
the percent of histidine with a protonated side chain? What is the total charge on molecules in
this fraction? Explain.

Expert Solution

queen_honey_blossom answered 2 years ago

A 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium...

A 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium acetate. For acetic acid, Ka=1.8×10−5. Part A) What is the initial pH of this solution? Part B) What is the pH after addition of 0.0150 mol of HCl? Part C) What is the pH after addition of 0.0150 mol of NaOH?

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate...

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.

Assume that you have a solution of 0.1 M glucose 6-phosphate. To this solution, you add...

Assume that you have a solution of 0.1 M glucose 6-phosphate. To this solution, you add the enzyme Phosphoglucomutase, which catalyzes the following reaction: The ΔG0’ for the reaction is +1.8 kcal mol-1. (a) Does the reaction proceed as written? If so, what are the final concentrations of glucose 6-phosphate and glucose 1-phosphate?

Part A. Calculate the pH of a buffer solution that is 0.250 M in HCN and...

Part A. Calculate the pH of a buffer solution that is 0.250 M in HCN and 0.168 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.240 M in HC2H3O2 and 0.190 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of...

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride,...

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a) Calculate the pH of the initial buffer solution. b) Calculate the pH of the new solution after the addition of acid. c) What becomes the pH if another 20.00 mL of the same acid solution is added?

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride,...

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a) Calculate the pH of the initial buffer solution. b) Calculate the pH of the new solution after the addition of acid. c) What becomes the pH if another 20.00 mL of the same acid solution is added? Pkb= 4.75

A 200.0 mL buffer solution is 0.360 M NH3 and 0.250 M NH4Br. What mass of...

A 200.0 mL buffer solution is 0.360 M NH3 and 0.250 M NH4Br. What mass of HCl does this buffer neutralize before pH falls below 8.80?

A). A buffer solution is made that is 0.337 M in H2CO3 and 0.337 M in...

A). A buffer solution is made that is 0.337 M in H2CO3 and 0.337 M in KHCO3. (1) If Ka for H2CO3 is 4.20×10-7, what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.075 mol NaOH is added to 1.00 L of the buffer solution B). A buffer solution is made that is 0.317 M in H2C2O4 and 0.317 M in KHC2O4. (1) If Ka for H2C2O4 is 5.90×10-2, what is the pH of the...

A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate...

A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate (NaCH3COO). The Ka of acetic acid is 1.8 • 10-5 at 25 o C. Calculate the pH of the resulting buffer solution when 10.00 mL of a 0.500 M aqueous HCl solution is added to this mixture.

A buffer solution is made that is 0.363 M in HClO and 0.363 M in NaClO...

A buffer solution is made that is 0.363 M in HClO and 0.363 M in NaClO . (1) If Ka for HClO is 3.50×10-8 , what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.082 mol HCl is added to 1.00 L of the buffer solution. Use H3O+ instead of H+ . A buffer solution is made that is 0.388 M in HCN and 0.388 M in NaCN. (1)...

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Assume you have successfully made a buffer solution, such that you have 0.250 M phosphate buffer...

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