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Unformatted text preview: L of a 1.00 M
aqueous solution of NH4Cl (molar mass 53.5 g mol−1). Include specific amounts and equipment where
Distilled water 50 mL buret
100 mL beaker 100 mL graduated cylinder
100 mL volumetric flask 100 mL pipet
Balance mass of NH4Cl = (0.100 L)(1.00 mol L−1)(53.5 g mol−1) = 5.35 g NH4Cl
1. Measure out 5.35 g NH4Cl using the balance. One point is
earned for the mass. 2. Use the 100 mL graduated cylinder to transfer approximately 25 mL of
distilled water to the 100 mL volumetric flask.
3. Transfer the 5.35 g NH4Cl to the 100 mL volumetric flask. One point is
earned for using a
volumetric flask. 4. Continue to add distilled water to the volumetric flask while swirling the flask
to dissolve the NH4Cl and remove all NH4Cl particles adhered to the walls. One point is
earned for diluting
to the mark. 5. Carefully add distilled water to the 100 mL volumetric flask until the bottom
of the meniscus of the solution reaches the etched mark on the flask. © 2007 The College Board. All rights reserved.
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This note was uploaded on 10/01/2009 for the course OC 9876 taught by Professor Dq during the Spring '09 term at UC Merced.
- Spring '09