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.
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A portion of a crushed antacid tablet is analyzed by a
back-titration. First 50.00 mL of...
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...
(1) A student is given an antacid tablet that weighs 5.4320 g. The tablet is crushed...
(1) A student is given an antacid tablet that weighs 5.4320 g. The tablet is crushed and 4.1220 g of the antacid is added to 200. mL of simulated stomach acid. It is allowed to react and then filtered. It is found that 25.00 mL of this partially neutralized stomach acid required 14.4 mL of a NaOH solution to titrate it to a methyl red end point. It takes 27.8 mL of this NaOH solution to neutralize 25.00 mL of...
A student is given an antacid tablet that weighed 5.6832 g. The tablet was crushed and...
A student is given an antacid tablet that weighed 5.6832 g. The tablet was crushed and 4.3628 g of he antacid was added to 200 mL fo simulated stomah acid. This was allowed to react and the filtered. It was found that 25 mL fo this partially neutralized stomach acid required 8.5 mL of a NaOH solution to titrate it to a methyl red endpoint. If it took 25.5 mL of this NaOH solution to neutralize 25 mL of the...
2. A student is given an antacid tablet that weighed 5.6832 g. The tablet was crushed...
2. A student is given an antacid tablet that weighed 5.6832 g. The tablet was crushed and 4.3628 g of the antacid was added to 200 mL of simulated stomach acid. This was allowed to react and then filtered. It was found that 25.00 mL of this partially neutralized stomach acid required 8.50 mL of a NaOH solution to titrate it to a methyl red endpoint. It took 21.54 mL of this NaOH solution to neutralize 25.00 mL of 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...
need calculation for this experiment EXPERIMENT 11 LABORATORY REPORT Brand of Antacid Cost of antacid —...
need calculation for this experiment
EXPERIMENT 11 LABORATORY REPORT Brand of Antacid Cost of antacid — Rugby 4. 5 € per tablet Average mass of tablet_1-30129_per tablet Concentration of HCl solution (M) 0.0979 Concentration of NaOH solution (M) 2.1006 Data Trial 1 Trial 2 Mass of sample (g) 0.116 49.1 Initial volume of HCI (mL 0-104 46.1 24-1 Final volume of HCI (mL) 21.) Initial volume of NaOH (mL 49.6 49.1 Final volume of NaOH (mL) 34.2 344 31-1 140...
Suppose a student adds 25.00 mL of 0.989 M HCl to a 1.54 g antacid tablet....
Suppose a student adds 25.00 mL of 0.989 M HCl to a 1.54 g antacid tablet. The student uses 21.1 mL of 0.543 M NaOH to titrate the solution. Calculate the moles of acid neutralized per grams of tablet. __________mol/g
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?
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.
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...
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...
2. A student is given an antacid tablet that weighed 5.6832 g. The tablet was crushed and 4.3628 g of the antacid was added to 200 mL of simulated stomach acid. This was allowed to react and then filtered. It was found that 25.00 mL of this partially neutralized stomach acid required 8.50 mL of a NaOH solution to titrate it to a methyl red endpoint. It took 21.54 mL of this NaOH solution to neutralize 25.00 mL of the...
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...
need calculation for this experiment
EXPERIMENT 11 LABORATORY REPORT Brand of Antacid Cost of antacid — Rugby 4. 5 € per tablet Average mass of tablet_1-30129_per tablet Concentration of HCl solution (M) 0.0979 Concentration of NaOH solution (M) 2.1006 Data Trial 1 Trial 2 Mass of sample (g) 0.116 49.1 Initial volume of HCI (mL 0-104 46.1 24-1 Final volume of HCI (mL) 21.) Initial volume of NaOH (mL 49.6 49.1 Final volume of NaOH (mL) 34.2 344 31-1 140...
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