Please clear answer and if you can avoid hand writing. Thanks ahead. An unknown triprotic acid...
Please clear answer and if you can avoid hand writing. Thanks ahead.
An unknown triprotic acid (so “n” = 3) sample of mass 0.225 g required 38.22 mL of 0.09767 M NaOH to neutralize where 2.14 mL of 0.1015 M HCl was used to back titrate, find the molar mass of the unknown solid acid in grams per mole.
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An unknown triprotic acid...
11. What is the molar mass of an unknown triprotic acid if 0.251 g of the...
11. What is the molar mass of an unknown triprotic acid if 0.251 g of the unknown acid requires 25.08 mL of 0.142 M NaOH to titrate it? 12. Describe how to prepare a 250mL 0.350M of oxalic acid solution using oxalic acid dihydrate solids (H2C204.2H20, molar mass = 126.06g/mol) You need to describe appropriate glassware in your preparation. 13. Describe how you would prepare 500. mL of 0.10M of HCl solution from 3.0M of HCI stock solution. You need...
6. 0.122 grams of an unknown triprotic acid was neutralized with 37.2 mL of a 0.125...
6. 0.122 grams of an unknown triprotic acid was neutralized with 37.2 mL of a 0.125 M NaOH solution. What is the Molar Mass of the unknown acid? Report the answer to three sig figs and there is no need to put in the unit label.
An analytical chemist weighs out 0.026 g of an unknown triprotic acid into a 250 mL...
An analytical chemist weighs out 0.026 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0800 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 9.9 mL of NaOH solution Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol
6. a) If the titration of 2.729 g of an unknown triprotic acid requires 48.15 mL...
6. a) If the titration of 2.729 g of an unknown triprotic acid requires 48.15 mL of 0.4012 M NaOH to reach the third equivalence point, what is the molar mass of this unknown acid? Show your work with units and correct significant figures. 7. If the second equivalence point in the titration of a diprotic acid is at 39.48 mL of strong base titrant added, at what volume is the? First half-equivalence point? Second half-equivalence point? 39.48 ml Second...
The student dissolved 2.050 grams of acid in 50 mL of distilled water. He then titrated...
The student dissolved 2.050 grams of acid in 50 mL of distilled water. He then titrated the unknown acid with a standardized NaOH solution. Unfortunately, the student over shot the end point and had to back titrate the solution with 2.17 mL of 0.98861 M HCl. Once the final end point was determined, the student had added a total of 29.15 mL of a 1.0324 M NaOH solution. A) How many moles of OH- were used to reach the end...
The student dissolved 2.050 grams of acid in 50 mL of distilled water. He then titrated...
The student dissolved 2.050 grams of acid in 50 mL of distilled water. He then titrated the unknown acid with a standardized NaOH solution. Unfortunately, the student over shot the end point and had to back titrate the solution with 2.17 mL of 0.98861 M HCl. Once the final end point was determined, the student had added a total of 29.15 mL of a 1.0324 M NaOH solution. A) How many moles of OH- were used to reach the end...
how do we determine the mass of acid/mole of sodium hydroxide of the unknown acid? i...
how do we determine the mass of acid/mole of sodium hydroxide of
the unknown acid?
i
am just looking for the formula to solve it
D. Determination of the mass of an unknown acid required to neutralize one mole of hydroxide ion. Obtain a clean, dry capped shell vial containing an unknown acid. Record your unknown's number and label the vial. Keep this vial in your locker until your graded lab report has been returned to you. 1. Note: the...
3. A 0.7026 g sample of an unknown acid requires 40.96 mL of 0.1158 M NaOH...
3. A 0.7026 g sample of an unknown acid requires 40.96 mL of 0.1158 M NaOH for neutralization to a phenolphthalein end point. There are 1.22 mL of 0.1036 M HCl used for back-titration. a. How many moles of OH are used? How many moles of Ht from HCI? moles OH moles H+ b. How many moles of Ht are there in the solid acid? (Use Eq. 5.) moles H+ in solid c. What is the molar mass of the...
1. In a 0.200 M solution of an unknown acid, the pH is 5.004. Calculate the...
1. In a 0.200 M solution of an unknown acid, the pH is 5.004. Calculate the Ka for this monoprotic acid 2. A 500.0 mL solution of HCl has a pH of 4.50. How many grams of HCl are there in this solution? The molar mass of HCl is 36.5g/mol. 3. Calculate the pOH of a 0.20 molar solution of NaOH.
Unknown acid 2 6. Complete the following table. Trial 1 Trial 2 Trial 3 Mass of...
Unknown acid 2 6. Complete the following table. Trial 1 Trial 2 Trial 3 Mass of unknown (8) 0.175 0.120 0.122 Initial buret reading (mL) 0.00 22.37 0.00 Final buret reading (mL) 22.37 44.85 22.83 Volume of NaOH added (mL) 22.37 22.48 22.83 We will assume that the data collected for the first trial is not accurate. 7. What is the average mass of unknown acid for Trials 2 and 3? (Must show calculations) 8. What is the average volume...
11. What is the molar mass of an unknown triprotic acid if 0.251 g of the unknown acid requires 25.08 mL of 0.142 M NaOH to titrate it? 12. Describe how to prepare a 250mL 0.350M of oxalic acid solution using oxalic acid dihydrate solids (H2C204.2H20, molar mass = 126.06g/mol) You need to describe appropriate glassware in your preparation. 13. Describe how you would prepare 500. mL of 0.10M of HCl solution from 3.0M of HCI stock solution. You need...
An analytical chemist weighs out 0.026 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0800 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 9.9 mL of NaOH solution Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol
6. a) If the titration of 2.729 g of an unknown triprotic acid requires 48.15 mL of 0.4012 M NaOH to reach the third equivalence point, what is the molar mass of this unknown acid? Show your work with units and correct significant figures. 7. If the second equivalence point in the titration of a diprotic acid is at 39.48 mL of strong base titrant added, at what volume is the? First half-equivalence point? Second half-equivalence point? 39.48 ml Second...
how do we determine the mass of acid/mole of sodium hydroxide of
the unknown acid?
i
am just looking for the formula to solve it
D. Determination of the mass of an unknown acid required to neutralize one mole of hydroxide ion. Obtain a clean, dry capped shell vial containing an unknown acid. Record your unknown's number and label the vial. Keep this vial in your locker until your graded lab report has been returned to you. 1. Note: the...
3. A 0.7026 g sample of an unknown acid requires 40.96 mL of 0.1158 M NaOH for neutralization to a phenolphthalein end point. There are 1.22 mL of 0.1036 M HCl used for back-titration. a. How many moles of OH are used? How many moles of Ht from HCI? moles OH moles H+ b. How many moles of Ht are there in the solid acid? (Use Eq. 5.) moles H+ in solid c. What is the molar mass of the...
Unknown acid 2 6. Complete the following table. Trial 1 Trial 2 Trial 3 Mass of unknown (8) 0.175 0.120 0.122 Initial buret reading (mL) 0.00 22.37 0.00 Final buret reading (mL) 22.37 44.85 22.83 Volume of NaOH added (mL) 22.37 22.48 22.83 We will assume that the data collected for the first trial is not accurate. 7. What is the average mass of unknown acid for Trials 2 and 3? (Must show calculations) 8. What is the average volume...
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