3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33.
(a) State two ways to standardize the NaOH used in the titration.
(b) Suggest and explain an indicator that can be used in the above neutralization titration. State the color change of the indicator at the end-point.
(c) Calculate the Ka of the weak acid.
(d) Calculate the percentage mass of HA in the sample, given that the molar mass of HA is 46.025 g/mol.
(e) Sketch and compare the titration curve of a strong acid vs strong base and the titration curve of weak acid vs strong base, given that both titrations contain the same concentration of the acid and base.
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3. 0.7253 g sample containing an unknown weak acid HA was
dissolved in 50 mL water...
It's a weak acid strong base titration Experiment 4: Identification of an unknown acid by titration...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
13. Sketch a titration curve for the titration of a monoprotic weak acid HA with a...
13. Sketch a titration curve for the titration of a monoprotic weak acid HA with a strong base. The titration reaction (neutralization) is: HA + OH + H2O+ A On the curve, clearly label the points that correspond to: i. the equivalence point ii. the region with maximum buffering iii. pH = pka iv. pH depends only on [HA] v. pH depends only on [A-] vi. pH depends only on amount of strong base added.
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.24 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 18.73 3.60 Equivalence point 37.45 8.59 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.18 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 18.77 3.83 Equivalence point 37.54 8.73 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.22 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 18.34 4.06 Equivalence point 36.68 8.84 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
2. A 0.500-gram sample of a weak, nonvolatile monoprotic acid, HA, was dissolved in sufficient water...
2. A 0.500-gram sample of a weak, nonvolatile monoprotic acid, HA, was dissolved in sufficient water to make 50.0 milliliters of solution. The solution was then titrated with a standard NaOH solution. Predict how the calculated molar mass of HA would be affected (too high, too low, or not affected) by the following laboratory procedures. Explain each of your answers. A. (2 points.). After rinsing the buret with distilled water, the buret is filled with the standard NaOH solution; the...
A 0.625-gram sample of an unknown weak acid (call it HA for short) is dissolved in...
A 0.625-gram sample of an unknown weak acid (call it HA for short) is dissolved in enough water to make 25.0 mL of solution. This weak acid solution is then titrated with 0.100 M NaOH and 45.0 mL of the NaOH solution is required to reach the equivalence point. Using a pH meter, the pH of the solution at the equivalence point is found to be 8.25. Determine the pKa value of the unknown acid.
5 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL...
5 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 2.1 . This solution is titrated with a 0.210 M NaOH solution. 60.2 mL of this NaOH solution is needed to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the value of pKa for HA (aq)? (c) What is the pH at the equivalence point? (d) What...
2.77 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL...
2.77 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 1.33. This solution is titrated with a 0.250 M NaOH solution. 40.6 mL of this NaOH solution is needed to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the value of pKa for HA (aq)? (c) What is the pH at the equivalence point? (d) What is...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
13. Sketch a titration curve for the titration of a monoprotic weak acid HA with a strong base. The titration reaction (neutralization) is: HA + OH + H2O+ A On the curve, clearly label the points that correspond to: i. the equivalence point ii. the region with maximum buffering iii. pH = pka iv. pH depends only on [HA] v. pH depends only on [A-] vi. pH depends only on amount of strong base added.
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.24 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 18.73 3.60 Equivalence point 37.45 8.59 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.18 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 18.77 3.83 Equivalence point 37.54 8.73 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
2. A 0.500-gram sample of a weak, nonvolatile monoprotic acid, HA, was dissolved in sufficient water to make 50.0 milliliters of solution. The solution was then titrated with a standard NaOH solution. Predict how the calculated molar mass of HA would be affected (too high, too low, or not affected) by the following laboratory procedures. Explain each of your answers. A. (2 points.). After rinsing the buret with distilled water, the buret is filled with the standard NaOH solution; the...
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