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12. Using the Henderson-Hasselbalch equation, prove (mathematically and chemically) why pH equals pkat half-way to the...
Using the Henderson-Hasselbalch equation, calculate the pH when 0.5 mole of sodium hydroxide is added to 1 mole of acetic acid. (pKa of acetic acid is 4.76).
Use the Henderson-Hasselbalch equation to calculate the mass of solid sodium acetate required to mix with 50.0 mL of 0.10 M acetic acid to prepare a pH 4 buffer. Ka for acetic acid is 1.8 times 10^-5. Use the Henderson-Hasselbalch equation to calculate the mass of solid ammonium chloride required to mix with 50.0 mL of 0.10 M ammonia to prepare a pH 10 buffer. The Kb for ammonia is 1.8 times 10^-5. The purpose of this experiment is to...
using your pH at half equivalence for acetic acid and ammonia and considering the Henderson-Hasselbalch equation, calculate their Ka and Kb values. Compare with the accepted values and explain sources of error.
1. Calculation: Using the Henderson-Hasselbalch equation, explain mathematically why a solution is at a pH below the pKa for an acid that more than 50% of the molecules have the proton on (not off). 2. Calculation: If you have a pH of 5.5 for a weak acid with a pKa of 4.76, then is there more A- or more HA in the solution? Explain why in words using your knowledge of positive or negative log numbers.
A buffer is prepared by adding 23.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.160 M acetic acid (CH3COOH) solution. Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added to the buffer. Express your answer as a chemical equation. Identify all of the phases...
A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of a 0.140 M acetic acid (CH3COOH) solution. 1) Determine the pH of the buffer. 2) Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (Express your answer as a chemical equation. Identify all of the phases in your answer.) 3) Write the complete ionic equation for the reaction that occurs when...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page 119 for appropriate K and K, values. Complete these calculations on your Report Sheet for complete credit. I. pH of Strong and Weak Acids 1. Calculate the pH of a 0.10 M hydrochloric acid solution, HCl(aq). 2. Calculate the pH of a solution prepared by diluting 5.00 mL of 0.10 M hydrochloric acid, HCl (aq), in enough water to make a 50.0 mL solution....
A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 480 mL of a 0.160 M acetic acid(CH3COOH) solution. 1. Determine the pHpH of the buffer. 2. Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.Identify all of the phases in your answer. 3. Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added...
Part A, B, C please Constants Periodic Tabl Part A A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of a 0.145 M acetic acid (CH3COOH) solution. Determine the pH of the buffer. Express your answer using two decimal places. IVO AQ R O D ? pH = Submit Request Answer Part B Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the...
Use the Henderson-Hasselbalch Equation to calculate the pH of a buffer solution that 10 0.050 Min benzoic acid (HC,1,0,) and 0.150 Min sodium benzoate ac or benzoic acid, K, - 6.5 * 10. (25 points) 2. Consider the combustion of propane gas: (25 points) CH, (g) + 5 0,(9) -- 3 CO2(g) + 4 H20 (g) ; AHU - -2044 kJ (a) Calculate the entropy change in the surroundings when this reaction occurs at 25 °C. (b) Determine the sign...