Concept explainers
a. Calculate the pH of a buffer that is
b. What is the pH of a buffer that is
c. What is the difference between the buffers described in parts a and b?
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Chemistry for Today: General, Organic, and Biochemistry
- A buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL. (a) Which component of the buffer is present in a larger amount? (b) If the concentration of Na3PO4 is 0.400 M, what mass of Na2HPO4 is present? (c) Which component of the buffer must be added to change the pH to 12.25? What mass of that component is required?arrow_forwardLactic acid (CH3CHOHCO2H) is found in sour milk, in sauerkraut, and in muscles after activity. (Ka for lactic acid = 1.4 104.) (a) If 2.75 g of NaCH3CHOHCO2, sodium lactate, is added to 5.00 102 mL of 0.100 M lactic acid, what is the pH of the resulting buffer solution? (b) Is the pH of the buffered solution lower or higher than the pH of the lactic acid solution?arrow_forwardA buffer solution is prepared by dissolving 1.50 g each of benzoic acid, C6H5CO2H, and sodium benzoate, NaC6H5CO2, in 150.0 mL of solution. (a) What is the pH of this buffer solution? (b) Which buffer component must be added, and in what quantity, to change the pH to 4.00? (c) What quantity of 2.0 M NaOH or 2.0 M HCl must be added to the buffer to change the pH to 4.00?arrow_forward
- A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?arrow_forwardConsider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25C. (Ka for HCN = 6.2 1010.) a. Calculate the pH after 0.0 mL of KOH has been added. b. Calculate the pH after 50.0 mL of KOH has been added. c. Calculate the pH after 75.0 mL of KOH has been added. d. Calculate the pH at the equivalence point. e. Calculate the pH after 125 mL of KOH has been added.arrow_forwardYou want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?arrow_forward
- A buffer contains 0.20 mol of propionic acid (C2H5COOH) and 0.18 mol of sodium propionate (C2H5COONa) in 1.20 L. A. What is the pH of this buffer? B. What is the pH of the buffer after the addition of 0.01 mol of NaOH? C. What is the pH of the buffer after the addition of 0.01 mol of HI?arrow_forwardA buffer solution contains 0.120 moles of propionic acid, HC3H50₂, and 0.100 moles of sodium propionate, NaC3H5O₂, in 1.00 L of solution. K₁= 1.32 x 10-5 a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.010 mol of NaOH? c. Beginning with the initial buffer from part a, what the pH of the buffer after the addition of 0.010 mol of HBr?arrow_forwardA buffer solution contains 0.250 mol of propylamine, CH3CH2CH2NH2, and 0.350 mol of propylammonium bromide, CH3CH2CH2NH3Br in 1.00 L of solution. Kb = 5.10 x 10-4. a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.025 mol of NaOH? (assume no volume change upon the addition of the NaOH) c. To the buffer produced in part a, what is the pH of the buffer after the addition of 0.100 mol of HCI? (assume no volume change up the addition of the HCI)arrow_forward
- a. How many grams of dry NH4CI need to be added to 2.40 L of a 0.300 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.89? Kb for ammonia is 1.8×10^-5. b. What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10^−7arrow_forwarda. What is the pH of a buffer made by mixing 1.556 mol methylamine with 1.556 mol methylammonium chloride (CH3NH3+). b. What is the pH of this buffer after the addition of 0.0056mol HCI? c. What is the pH of this buffer after the addition of 0.0056 mol NaOH?arrow_forwardthe reagent potassium phosphate tribasic trihydrate (K3PO4*3H2O) and 1.1M HCl and 1.1 M NaOH. you need to make 1 liter of buffer that has 0.01 molar minimum buffer capacity to resist either 0.01 moles of strong base or strong acid at pH 7.2. a. How many grams of potassium phosphate tribasic trihydrate are theoretically needed? b.how many mL of HCL solution? c. How many mL of NaOH solution? Please answer very soon will give rating surely All questions answers neededarrow_forward
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