One of the most common buffers used in protein chemistry is a weak base called TRIS (the nitrogen atom of the amino group is the basic portion of the molecule): Но. -NH2 (HOCH2);CNH2 = TRIS HO A biochemist prepares a buffer solution by adding enough TRIS and 12 M HCI to give 1.0 L of a buffer solution that has concentrations [TRIS] = 0.34 M and [TRISH*] = 0.71 M. (pKµ of TRIS is 5.91.) (a) Calculate the pH of the buffer solution.

15

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4-  + H2O ⇌  HPO42-  + H+  pKa= 7.21  (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)

A buffer solution is made that is 0.368 M in HCN and 0.368 M in KCN. If Ka for HCN is 4.00 × 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +

A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 6.44) with 20.00 mL of 0.100 M NaOH.  This buffer is then divided into 4 equal 15.00 mL parts. If 0.15 mL of a 1.0 M solution of sodium hydroxide is added to one of these 15.00 mL portions of the buffer, what is the pH of the resulting solution?

A buffer solution is made that is 0.327 M in H2 CO3 and 0.327 M in NaHCO3. If Ka for H2CO3 is 4.20 x 10, what is the pH of the buffer solution? 7 PH3D6,38 Write the net ionic equation for the reaction that occurs when 0.070 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3 0 instead of Ht) +.

A second titration is performed using the same 0.250 M NaOH in a buret. This time 25.0mL of an H2SO4 soln is titrated. At the endpoint 47.8 mL of NaOH has been added to theH2SO4 soln. What is the molarity of the H2SO4?