In Experiment 1, a student determined the aspirin content of a tablet by a back titration procedure. The weight of the s...
In Experiment 1, a student determined the aspirin content of a tablet by a back titration procedure. The weight of the student’s tablet was 1.5500 g. After crushing and dissolving the tablet, the student added 54.00 mL of 0.1000 M NaOH. The back titration of the excess NaOH required 18.00 mL of 0.2000 M HCl. How many moles of aspirin were in the tablet?
Homework Answers
Request Answer!
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Add Answer to:
In Experiment 1, a student determined the aspirin content of a tablet by a back titration procedure. The weight of the s...
In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and...
In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and the excess was then back titrated with HCl. Suppose a 0.4567 g sample of aspirin was reacted with 18.12 mL of 0.1345 M NaOH and back titrated with 12.15 mL of 0.1124 M HCl to reach the endpoint. Calculate the weight of aspirin (Asp) in the sample.
A portion of a crushed antacid tablet is analyzed by a back-titration. First 50.00 mL of...
A portion of a crushed antacid tablet is analyzed by a back-titration. First 50.00 mL of 0.1250 M HCl is added to the tablet; then 12.51 mL of 0.1234 M NaOH is added to titrate the excess acid and reach the endpoint. Calculate the number of moles of HCl that reacted with the antacid.
9. In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin...
9. In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and the excess was then back titrated with HCl. Suppose a 0.4567 g sample of aspirin was reacted with 18.12 ml/of 0.1345 M NaOH and back titrated with 12.15 mL of 0.1124 M HCl to reach the endpoint. Calculate the weight percent of aspirin (Asp) in the sample. 8.457% 37.90% 21.14% 42.28% none of the above
The amount of aspirin (C_9H_7O_4H, molar mass = 180.15 g/mole) in a commercial tablet was determined...
The amount of aspirin (C_9H_7O_4H, molar mass = 180.15 g/mole) in a commercial tablet was determined by titration with sodium hydroxide. What mass of aspirin was in a tablet if 15.00 mL of 0.2000 M NaOH solution were needed to titrate the tablet dissolved in 30 mL of water? Show all calculations. Would more or less of NaOH titrant in problem 6 be required if the amount of water initially added to the Erlenmeyer flask with the product to be...
1. A student carries out a back titration to determine the concentration of ammonium chloride in a solution. The student...
1. A student carries out a back titration to determine the concentration of ammonium chloride in a solution. The student collects 10.80 mL of the original NH4Cl solution and dilutes it to 250.0 mL (we will refer to this as the dilute NH4Cl solution). Then 25.00 mL of the dilute NH4Cl solution are transferred to an Erlenmeyer flask and 25.00 mL of 0.1963 M NaOH are added. Calculate the moles of NaOH added to this Erlenmeyer flask. 2. In the...
A Tums tablet weighed 1.319 g. Using the procedure of this experiment, the tablet was dissolved...
A Tums tablet weighed 1.319 g. Using the procedure of this experiment, the tablet was dissolved in, and reacted with, an excess amount of HCl (125.00 mL of 0.101 M HCl). The excess unreacted HCl was titrated with NaOH; 18.75 mL of 0.101 M NaOH was used to reach the endpoint. Calculate the moles of HCl that did not react with the antacid. Calculate the moles of HCl that did react with the antacid. Calculate the mass of HCl that...
4. A student analyzed an antacid tablet from a bottle of 48 tablets purchased at a...
4. A student analyzed an antacid tablet from a bottle of 48 tablets purchased at a discount store for $1.00. The mass of the tablet was 1.462g. After adding 25.00mL of 0.8000/M HCl solution to the tablet, the student back-titrated the excess HCI with 3.52 mL of 1.019M NaOH solution. (a) Calculate the number of moles of HCI added to the tablet (b) Calculate the number of moles of NaOH required for the back-titration (c) Calculate the number of moles...
Question 5 (10 points) If a student determined that 0.02351 moles of HCl was initial added...
Question 5 (10 points) If a student determined that 0.02351 moles of HCl was initial added to the beaker and 0.008952 moles of NaOH was calculated for the back titration. How many moles of HCl were neutralized by the antacid tablet (Note: the molar ratio of the reaction is 1:1 ; so there are 1 mole of HCI-to-1 mole of NaOH)? 0.014558 0.0014560 -0.014558 -0.01456 0.01456 RA
b) In this experiment an aspirin tablet mark with deionized water. Using a pipette into a...
b) In this experiment an aspirin tablet mark with deionized water. Using a pipette into a 100-mL volumetric flask and diluted to t make a 'diluted aspirin solution'. an aspirin tablet was placed in a 250-ml volumetric flask o dissolved in 10 mL of 1.0M NaOH solution, the flask was then 1.0M NaOH solution, the flask was then filled to the nized water. Using a pipette, 5.0 mL of this solution was added mL volumetric flask and diluted to the...
1. A particular brand of antacid contains 500 mg of CaCO3 per 2.0 g tablet according...
1. A particular brand of antacid contains 500 mg of CaCO3 per 2.0 g tablet according to the label. How many mol of CaCO3 are contained in one tablet? nCaCO3 = ___ mol Ans. 0.005mol 2. The reaction by which the antacid neutralizes HCl is 2 HCl(aq) + CaCO3(s) à CaCl2(aq) + CO2(g) + H2O(l) How many moles of HCl can be neutralized by one tablet? nHCl = 0.010 mol 3. 50.0 mL of 0.300 M HCl are used to...
9. In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and the excess was then back titrated with HCl. Suppose a 0.4567 g sample of aspirin was reacted with 18.12 ml/of 0.1345 M NaOH and back titrated with 12.15 mL of 0.1124 M HCl to reach the endpoint. Calculate the weight percent of aspirin (Asp) in the sample. 8.457% 37.90% 21.14% 42.28% none of the above
The amount of aspirin (C_9H_7O_4H, molar mass = 180.15 g/mole) in a commercial tablet was determined by titration with sodium hydroxide. What mass of aspirin was in a tablet if 15.00 mL of 0.2000 M NaOH solution were needed to titrate the tablet dissolved in 30 mL of water? Show all calculations. Would more or less of NaOH titrant in problem 6 be required if the amount of water initially added to the Erlenmeyer flask with the product to be...
A Tums tablet weighed 1.319 g. Using the procedure of this experiment, the tablet was dissolved in, and reacted with, an excess amount of HCl (125.00 mL of 0.101 M HCl). The excess unreacted HCl was titrated with NaOH; 18.75 mL of 0.101 M NaOH was used to reach the endpoint. Calculate the moles of HCl that did not react with the antacid. Calculate the moles of HCl that did react with the antacid. Calculate the mass of HCl that...
4. A student analyzed an antacid tablet from a bottle of 48 tablets purchased at a discount store for $1.00. The mass of the tablet was 1.462g. After adding 25.00mL of 0.8000/M HCl solution to the tablet, the student back-titrated the excess HCI with 3.52 mL of 1.019M NaOH solution. (a) Calculate the number of moles of HCI added to the tablet (b) Calculate the number of moles of NaOH required for the back-titration (c) Calculate the number of moles...
Question 5 (10 points) If a student determined that 0.02351 moles of HCl was initial added to the beaker and 0.008952 moles of NaOH was calculated for the back titration. How many moles of HCl were neutralized by the antacid tablet (Note: the molar ratio of the reaction is 1:1 ; so there are 1 mole of HCI-to-1 mole of NaOH)? 0.014558 0.0014560 -0.014558 -0.01456 0.01456 RA
b) In this experiment an aspirin tablet mark with deionized water. Using a pipette into a 100-mL volumetric flask and diluted to t make a 'diluted aspirin solution'. an aspirin tablet was placed in a 250-ml volumetric flask o dissolved in 10 mL of 1.0M NaOH solution, the flask was then 1.0M NaOH solution, the flask was then filled to the nized water. Using a pipette, 5.0 mL of this solution was added mL volumetric flask and diluted to the...
Most questions answered within 3 hours.
-
An important news announcement is transmitted by radio waves to
people who are 65 km away,...
asked 10 minutes ago -
On June 30, 2021, Rosetta Granite purchased equipment for
$130,000. The estimated useful life of the...
asked 9 minutes ago -
. If you were the CEO of Agricole, would you pursue an
acquisition target in the...
asked 10 minutes ago -
(a) We define standard Gibbs energy change, G0 =
H0 – TS0, what is the relationship...
asked 10 minutes ago -
If the barometric pressure is 107.4 kPa, what is the pressure in
kPa of the gas...
asked 31 minutes ago -
A resonance tube can be used to measure the speed of sound in
air. A tuning...
asked 24 minutes ago -
Lourdes LLC. keeps a $100 change fund in its cash register. At
the end of the...
asked 29 minutes ago -
State the operation or control mechanism of TRIAC, DIAC, UJT, PUT,
GTO and IGBT.
asked 32 minutes ago -
Generator An AC generator supplies an rms voltage of 220 V at
50.0 Hz. It is...
asked 35 minutes ago -
Cars enter a car wash at a mean rate of 2 cars per half an hour....
asked 46 minutes ago -
Write SQL queries to answer the following question: A. Which
students are enrolled in Database and...
asked 1 hour ago -
Required:
How was Dell computer working capital policy as a competitive
advantage? Write at least 200...
asked 42 minutes ago