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IDENTIFICATION OF AN UNKNOWN AMMONIUM SALT PURPOSE In this lab you will: 1. gain experience in the use of the concept of equivalent mass in acid - base calculations, 2. determine the equivalent mass and thus the identity of an unknown crystalline solid which has the general formula (NH4)aX, and METHOD For an acid, the equivalent mass is defined as the mass in grams that provides one mole of protons in a neutralization reaction. Ammonium salts react with strong bases, such as sodium hydroxide, as shown below. EXPERIMENT 2 heat NH4+(aq) + OH- (aq) NH3 (aq) + H₂O(1) (1) In this experiment we will add a large excess of NaOH to react with the ammonium salt. The ammonia formed will be driven out of solution by heating. NH3(aq) NH3(g) (2) Note that the addition of heat drives equilibrium (2) to the right. This removes ammonia from the solution and gradually drives equilibrium (1) to completion. unknown ammonium salt 0.2 M standard NaOH 0.2 M standard HCl bromthymol blue indicator - The remaining unreacted excess NaOH will be backtitrated with standard acid. The amount of NaOH which reacted with the NH4+ can be calculated by subtracting the amount of NaOH left from the amount of NaOH originally added. CHEMICALS EQUIPMENT 125 mL Erlenmeyer flasks 1-50 mL buret, clamp, ring stand 1-50mL volumetric pipet Red litmus paper Boiling chips/stones SAFETY The dilute acid and base used here are relatively safe. Clean up any spills. Wear your goggles during the heating to remove ammonia. Do the heating in the hood to avoid ammonia fumes in the room.

IDENTIFICATION OF AN UNKNOWN AMMONIUM SALT PURPOSE In this lab you will: 1. gain experience in the use of the concept of equivalent mass in acid - base calculations, 2. determine the equivalent mass and thus the identity of an unknown crystalline solid which has the general formula (NH4)aX, and METHOD For an acid, the equivalent mass is defined as the mass in grams that provides one mole of protons in a neutralization reaction. Ammonium salts react with strong bases, such as sodium hydroxide, as shown below. EXPERIMENT 2 heat NH4+(aq) + OH- (aq) NH3 (aq) + H₂O(1) (1) In this experiment we will add a large excess of NaOH to react with the ammonium salt. The ammonia formed will be driven out of solution by heating. NH3(aq) NH3(g) (2) Note that the addition of heat drives equilibrium (2) to the right. This removes ammonia from the solution and gradually drives equilibrium (1) to completion. unknown ammonium salt 0.2 M standard NaOH 0.2 M standard HCl bromthymol blue indicator - The remaining unreacted excess NaOH will be backtitrated with standard acid. The amount of NaOH which reacted with the NH4+ can be calculated by subtracting the amount of NaOH left from the amount of NaOH originally added. CHEMICALS EQUIPMENT 125 mL Erlenmeyer flasks 1-50 mL buret, clamp, ring stand 1-50mL volumetric pipet Red litmus paper Boiling chips/stones SAFETY The dilute acid and base used here are relatively safe. Clean up any spills. Wear your goggles during the heating to remove ammonia. Do the heating in the hood to avoid ammonia fumes in the room.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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IDENTIFICATION OF AN UNKNOWN AMMONIUM SALT EXPERIMENT 2 PURPOSE In this lab you will: 1. gain experience in the use of the concept of equivalent mass in acid - base calculations, 2. determine the equivalent mass and thus the identity of an unknown crystalline solid which has the general formula (NH4)aX, and METHOD For an acid, the equivalent mass is defined as the mass in grams that provides one mole of protons in a neutralization reaction. Ammonium salts react with strong bases, such as sodium hydroxide, as shown below. heat NH4+ (aq) + OH- (aq) NH3 (aq) + H₂O(1) (1) In this experiment we will add a large excess of NaOH to react with the ammonium salt. The ammonia formed will be driven out of solution by heating. NH3(aq) NH3(g) (2) Note that the addition of heat drives equilibrium (2) to the right. This removes ammonia from the solution and gradually drives equilibrium (1) to completion. unknown ammonium salt 0.2 M standard NaOH 0.2 M standard HCl bromthymol blue indicator The remaining unreacted excess NaOH will be backtitrated with standard acid. The amount of NaOH which reacted with the NH4+ can be calculated by subtracting the amount of NaOH left from the amount of NaOH originally added. CHEMICALS EQUIPMENT 125 mL Erlenmeyer flasks 1-50 mL buret, clamp, ring stand 1-50mL volumetric pipet Red litmus paper Boiling chips/stones SAFETY The dilute acid and base used here are relatively safe. Clean up any spills. Wear your goggles during the heating to remove ammonia. Do the heating in the hood to avoid ammonia fumes in the room.
Transcribed Image Text:IDENTIFICATION OF AN UNKNOWN AMMONIUM SALT EXPERIMENT 2 PURPOSE In this lab you will: 1. gain experience in the use of the concept of equivalent mass in acid - base calculations, 2. determine the equivalent mass and thus the identity of an unknown crystalline solid which has the general formula (NH4)aX, and METHOD For an acid, the equivalent mass is defined as the mass in grams that provides one mole of protons in a neutralization reaction. Ammonium salts react with strong bases, such as sodium hydroxide, as shown below. heat NH4+ (aq) + OH- (aq) NH3 (aq) + H₂O(1) (1) In this experiment we will add a large excess of NaOH to react with the ammonium salt. The ammonia formed will be driven out of solution by heating. NH3(aq) NH3(g) (2) Note that the addition of heat drives equilibrium (2) to the right. This removes ammonia from the solution and gradually drives equilibrium (1) to completion. unknown ammonium salt 0.2 M standard NaOH 0.2 M standard HCl bromthymol blue indicator The remaining unreacted excess NaOH will be backtitrated with standard acid. The amount of NaOH which reacted with the NH4+ can be calculated by subtracting the amount of NaOH left from the amount of NaOH originally added. CHEMICALS EQUIPMENT 125 mL Erlenmeyer flasks 1-50 mL buret, clamp, ring stand 1-50mL volumetric pipet Red litmus paper Boiling chips/stones SAFETY The dilute acid and base used here are relatively safe. Clean up any spills. Wear your goggles during the heating to remove ammonia. Do the heating in the hood to avoid ammonia fumes in the room.
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