A buffer is prepared by adding 5.00 g sodium acetate (MW = 82.0343 g/mol) and 10.0 mL of 5.00 % acetic acid. The pKa of acetic acid = 4.76. What is the pH of this buffer?
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A buffer is prepared by adding 5.00 g sodium acetate (MW = 82.0343 g/mol) and 10.0 mL of 5.00 % acetic acid. The pKa of acetic acid = 4.76. What is the pH of this buffer?
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- Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.A chemistry graduate student is given 100. mL of a 1.70M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K = 4.9 × 10-10, what mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.78? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 0x10 X ŚConsider the titration of a weak acid that has a pKa = 4.00. Suppose a chemist was going to perform a titration on 50.0 mL of 0.050 0 M of the weak acid using 0.500 M NaOH. (A) What would be the pH of the solution after 0.00 mL of 0.500 M NaOH has been added?(B) What would be the pH halfway to the equivalence point of the titration?(C) What would be the pH at the equivalence point in the titration? (D) What would be the pH of the solution after 6.00 mL of 0.500 M NaOH has been added? Use the following reasoning when solving this problem. Because at the equivalence point the moles of strong base (0.500 M NaOH) added as a titrant equal the moles of weak acid, HA (50.0 ml of 0.050 M) in the solution, we can start by calculating the volume of 0.500 M NaOH needed to reach the equivalence point. To do this we simply equate the moles of HA to moles of NaOH by using the dilution formula. i.e. MaVa = MbVb where a represents HA and b represents NaOH. To calculate volume of NaOH needed to reach…
- What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pKa of the acid is 5.7. How many grams of ammonium sulfate ((NH4 )2SO4 )) would you need to add to 425 mL of 0.28 M ammonia (NH3 ) to obtain a buffer solution with a pH of 9.45. Assume that the volume doesn’t change when you add the salt. Ka for the ammonium ion is 5.8 x 10-10 . (be careful with how the reaction for ammonium is written as well as stoichiometry) A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and 0.550 M formic acid (HCOOH). (Ka of HCOOH is 1.8 x 10-4 ) a. Calculate the initial pH of this buffer. b. What is the pH after the addition of 0.0050 mol HCl? c. How about after the addition of 0.0050 mol NaOH? [For parts b and c, assume that volume doesn’t change in the addition process and that neutralization proceeds to completion]A buffer is made by combining lactic acid (HC3H5O3) and sodium lactate (NaC3H5O3) so that it is 3.25 M HC3H5O3 and 1.68 M NaC3H5O3. The Ka of lactic acid is 1.4×10-4. What is the pH of the buffer solution?A buffer solution contains formic acid and a salt solution containing sodium formate. What is the pH of a solution that is 0.0250 M in formic acid and 0.0625 M in sodium formate? pKa of formic acid is 3.745.
- A buffer contains 0.010 mol of lactic acid (pKa = 3.86) and 0.050 mol of sodium lactate per liter. (a) Calculate the pH of the buffer. (b) Calculate thechange in pH when 5 mL of 0.5 M HCl is added to 1 L of the buffer. (c) What pH change would you expect if you added the same quantity of HCl to 1 L of pure water?A chemistry graduate student is given 100. mL of a 0.90M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K₁=7.4 × 104. f (CH3)2NHCl should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 10.66? mass of You may assume that the volume of the solution doesn't change when the (CH3)2NHC1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0x12 What X S ? EFET ol ArA certain weak acid, HA, with a Ka value of 5.61 x 10-6 is titrated with NaOH (a) A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Express pH numerically to two decimal places. (b) More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 33.0 mL ? Express the pH numerically to two decimal places.
- 2. You wish to prepare a buffer containing acetic acid and sodium acetate with a total acetic acid and acetate concentration of 450 mM and a pH of 5.5 (a) What are the final concentrations of acetic acid and sodium acetate in the buffer? (b) Calculate the number of moles of acetic acid and sodium acetate that you would need to make 1.5 L of the buffer. (c) How many grams of acetic acid and sodium acetate would you need to make 1.5 L of the buffer (molecular weight of acetic acid=60.05 g/mol: molecular weight of sodium acetate =82.03 g/mol)?A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONA) into 100.00 mL of a 0.100 M solution of acetic acid. Then 1.80 mL of a 10.00 M solution of hydrochloric acid is added to the acetic acid/sodium acetate buffer solution. The K, of acetic acid is 1.8 × 10. What is the pH of the solution after adding HCl? pHA buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 2.00 mL of a 1.00 M solution of sodium hydroxide is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 x 10-5. What is the pH of the solution after adding NaOH?