Phenylacetic acid (C6H5CH2CO2H) is a weak monoprotic acid with Ka=4.90x10-5. what is the pH that results by mixing 2.56 g of phenylacetic acid with 1.59 g of potassium phenylacetate and diluting to 250.0 mL?

A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2 (ethylamine), the burette is filled with 0.20 M HCl as titrant.   Kb of C2H3NH2 = 6.5 ´ 10-4          What is the initial pH of above sample solution before titration starts?

Consider the titration of 100.0 mL of 0.100 M acetic acid (Ka = 1.8 x 105). When 50.00 mL of 0.100 M NaOH is added to the acetic acid solution, calculate the pH of the resulting mixture. Use the simultaneous equations method, showing the derivation of the final equation you used to calculate pH and justify any assumptions made in your derivation.

How many mL of 1.0 M NaOH must be added to 100. mL of 0.050 M HC2H3O2 to make a buffer with a pH = 5.00? Ka = 1.8 x 10-5 for acetic acid.

We are looking for the molar mass and the pKa value of a weak monoprotonic acid. Two experimentswere carried out with the solid, anhydrous sodium salt of this acid:1st experiment: 10.00 g of the salt was dissolved in 1.000 L of water. Then 10.00 mL of hydrochloric acidwith a concentration of 3.000 mol/L was added. The resulting solution had a pH value of pH = 4.7903.2nd experiment: 10.00 g of the salt was dissolved in 1.000 L of water. Then 15.00 mL of hydrochloric acidwith a concentration of 3.000 mol/L was added. The resulting solution had a pH value of pH = 4.4246.

Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid (HPr), and we slowly add 0.1000 M NaOH. What is the pH at 0.00 mL and 30.00 mL?

Similar to acetic acid, benzoic acid is a weak acid (HA) and is a commonly used as antimicrobial preservative in food and beverages, especially in carbonated beverages Suppose 10.00-mL of 0.5000 M benzoic acid (C6H5COOH) is titrated with 0.2000M NaOH. Ka for benzoic acid is 6.3 x 10-5 . What is the pH after addition of 35.00 mL of NaOH to the benzoic acid solution?

An undergraduate research student wishes to create a system that mimics human blood (pH = 7.4). The student chose as the model system to use a buffer solution of sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4, Ka = 4.2 × 10-13). A)  Which of the components of the buffer solution is the acid?  B)  Using the Henderson Hasselbalch equation, calculate the mole ratio of Na2HPO4/NaH2PO4 the student needs to use. C)  To approximate the human condition of blood alkalosis (where the pH of blood rises to 7.6, which is usually lethal), how much base will the student need to add to the buffer?

End Points in Strong-Base Titration of Mixed Strong Monoprotic and Weak Polyprotic Acids 1.39×10-2; ka2 = 6.73×10−8) is titrated A mixed aqueous solution of HCl and sulfurous acid (H₂SO3; Kal with 0.1000-M NaOH. The first end point (ethyl orange indicator) is reached after 38.91 mL of NaOH has been added. The second end point (thymolphthalein indicator) is reached after a total of 54.79 mL of NaOH has been added. What quantity of HCI (units of mol or mmol) was present in the initial mixture? 2.303 mol Submit Answer Incorrect. Tries 2/5 Previous Tries What quantity of sulfurous acid (units of mol or mmol) was present in the initial mixture? 1.59 mol

Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid (HPr), and we slowly add 0.1000 M NaOH. What is the pH at 40.00 mL and 50.00 mL?