Measuring the Densities of Aqueous Glasses at Cryogenic Temperatures

CAUTION: Please consult all relevant material safety data sheets (MSDS) before use. Please use all appropriate safety practices when using compressed gases, including appropriate calibrated gas handling regulators and valves, and approved gas tubing. Contact with liquid cryogens can cause  severe frostbite and necrosis. Use appropriate personal protective equipment (face shield, gloves, lab coat, full length pants, closed-toe shoes), all of which must be impermeable to liquid nitrogen. Remain standing and ensure an unobstructed exit path from the apparatus when using liquid cryogens. Be aware of asphyxiation hazards when using compressed gases and liquid cryogens, and work in a well-ventilated area with adequate make-up air (a fume hood or a high air turnover rate room.)

1. Preparation of Aqueous Solutions for Density Measurements

NOTE: Because weights are more easily measured to a high accuracy than volumes, solution concentrations are measured in w/w units. All densities and melting or boiling temperatures assume an atmospheric pressure of ~100 kPa. The following steps describe the preparation of a 35% w/w glycerol solution. The same procedure can be used for other concentrations and solutes.

1. For each solute type and concentration of interest, roughly estimate the required solute mass to obtain the desired final concentration (e.g., between 25% w/w and 100% w/w) for a total solution volume, V_tot = 10 mL solution volume. For example, for a 35% w/w glycerol solution (ρ_s = 1.26 g/mL), the solute mass, m_s is:
   
   where x is the solute mass fraction (0.35) and ρ_w= 1 g/mL is the density of water.
2. Place a 15 mL centrifuge tube (or other volume-calibrated water-impermeable container) on the pan of an analytical microbalance. Dispense the desired mass of solute/cryoprotectant (e.g., 3.77 g glycerol for a 35% w/w solution) into the tube, and record the actual solute mass.
3. Add high purity (>18 MΩ) deionized water to bring the total mass up to 10.0 g
4. Vortex the container for 30 s (for liquid solutes) or 5 min (for solid solutes), until the solution is optically homogeneous.
5. Measure and record the final mass of the solution. Seal the container with an airtight cap and store at constant temperature (293-298 K).

2. Preparation of the Sample Cooling Chamber

1. Place the experimental apparatus described below in an enclosure and flow dry air (>5% relative humidity (r.h.)) into the enclosure.
   NOTE: The enclosure may be a simple metal frame with its top and three sides sealed with clear plastic sheet and with experiment access via a fourth side covered with flexible plastic sheet. Wear face shields and full body covering to minimize moisture introduced by the experimenter. Moisture condensation and ice formation can interfere with cryogenic temperature density measurements in several ways, and so it must be minimized.
2. Place a disk of neoprene rubber on the bottom of a 4.5 L glass Dewar flask, to protect the Dewar flask from damage.
3. Carefully insert a high thermal conductivity copper chamber (a hollow cylinder with a sealed bottom) into the flask until it rests on the rubber disk. Adjust struts projecting outward from the chamber to the Dewar walls so that the chamber is centered and has no tendency to rock.
   NOTE: The Dewar flask will hold liquid nitrogen, and the much smaller volume copper chamber will hold a liquid N₂-Ar mixture. The liquid nitrogen provides a thermal bath that maintains the copper chamber and its contents at a constant temperature of 77 K and reduces boiling and evaporative losses in the chamber. The chamber's small diameter suppresses surface waves that can interfere with buoyancy measurements, and helps isolate the liquid within the chamber from frost and ice formed elsewhere in the apparatus.
4. Insert the outlet of a gas tube with dry N₂ gas flowing at ~2 L/min down to the bottom of the copper chamber, and purge the chamber of moist air.
5. Slowly pour liquid nitrogen into the Dewar flask, outside the copper chamber, allowing time for nitrogen boil-off.
   NOTE: The final fill level, after boiling has ceased, should be within approximately 4 cm of the top of the copper chamber.
6. Cover the outer portion of the Dewar flask with an annular foam insulating lid. Remove the dry N₂ gas purge tube from the copper chamber and insert into a matching opening in the lid.
   NOTE: The combination of N₂ gas from boil-off in the Dewar flask and from the purge flow expels any moist air and prevents it from condensing and crystalizing on cold surfaces.
7. Slowly pour liquid nitrogen into the copper chamber. The final fill level, after boiling has ceased, should be within approximately 4 cm of the top of the copper chamber.
8. Place a thin, optically transparent plastic sheet over the central opening or vent in the lid, and reduce the N₂ gas flow rate to ~0.2 L/min, leaving a slight overpressure of N₂ gas within the gas spaces above the cryogenic liquids.
   NOTE: As long as cryogenic liquids are present in the Dewar and chamber, continue adjusting the N₂ gas flow as needed to maintain this overpressure and prevent moisture from entering into the Dewar and forming ice.

3. Determination of the Volume and Density of the Test Mass at T = 298 K and T = 77 K

1. Determine the apparent mass of a ~1 g, ~0.4 mL PTFE test mass (Table of Materials) in air at T= 298 K by placing it on the pan of a calibrated analytical microbalance.
2. Determine the volume V(298 K) of the test mass at T = 298 K using a gas pycnometer, or by dimensional measurements using calipers. If using dimensional measurements, the test mass must have a simple, precise shape (no tapers or rounded corners) and the volume of the through-hole (for the suspending line) should be determined.
3. Calculate the mass m of the test mass by correcting the measured apparent mass for the buoyant force exerted by air according to the following:
   
   where ρ_air = 1.23 g/L (~0.1% correction).
4. Place the microbalance on a stable platform roughly 10 cm above the Dewar flask and verify its calibration. Suspend the test mass using a 2 mil (50 μm) monofilament line strung from the hook on the underside of the microbalance (designed for hanging mass measurements) and through a hole in the test mass. Determine the apparent mass in air, and compare with the measurement in step 3.3, correcting as needed for the mass of the line.
5. Determine the volume V(77 K) of the test mass at T = 77 K by measuring its apparent mass in pure liquid nitrogen, m_{app in LN2}. Lower the test mass into the liquid nitrogen within the copper chamber until it is fully submerged. When boiling has ceased, measure the apparent mass.
   NOTE: If the liquid nitrogen in the copper chamber is quiescent and air currents between the microbalance and the liquid surface are minimal, this mass can be measured to greater than ± 0.0002 g accuracy.
6. Estimate the buoyant force on the submerged portion of the line, and verify that it is small compared with measurement errors.
7. Calculate the volume and density of the test mass at 77 K using its known mass m and the measured apparent mass in LN2 at 77 K, m_{app in LN2}, according to the following:
   
   where ρ_LN2((77 K)=0.807 g/mL.

4. Preparation of the Initial Liquid N₂-Ar Mixture

1. Flow Ar gas at a flow rate of ~2 L/min through a coiled tube to its outlet. Place the coiled tube on top of the upper struts that stabilize the position of the copper chamber, just above the liquid nitrogen level and below the top surface of the Dewar. Cold N₂ and Ar gas will build up above the cryogenic liquids, and thermal conduction, convection, and radiation will cool the tubing and the Ar gas within.
2. After allowing the coiled tube to cool for 5 min, place the outlet of the tube in the copper chamber, at least 10 cm below the surface of the liquid nitrogen. Then cover the Dewar with the annular lid and transparent sheet.
3. Adjust the Ar flow rate until Ar bubbles rise from the tube outlet to the top surface of the liquid nitrogen. Then reduce the flow rate until the bubbles form at the outlet but dissolve or liquefy just before breaking the liquid nitrogen surface.
   NOTE: As the Ar concentration in the copper chamber increases, periodically adjust the Ar flow rate as needed to maintain bubble formation. If the Ar flow rate is too low, the Ar may freeze inside the tube and block the flow.
4. Add liquid nitrogen as needed to maintain its level in the surrounding Dewar. Remove ice as it accumulates on cold surfaces.
5. Periodically mix the liquid by inserting a thin (e.g., 35 micron), circular sheet of copper foil attached to a thin insulating rod into the copper chamber, and slowly moving it up and down like a piston. This will reduce concentration gradients and the tendency for Ar to crystallize out of the solution.

5. Measuring and Adjusting the Density of the Initial N₂-Ar Mixture

1. Calculate the target density for the N₂-Ar mixture by estimating the T =77 K density of the sample to be measured, e.g., measurements at higher concentrations of the sample's non-aqueous component.
2. Attach the test mass using the monofilament line to the hook on the underside of the microbalance measuring pan, measure its apparent mass in air, and confirm agreement with the measurement in step 3.1.
3. Mix the N₂-Ar solution to eliminate concentration and density gradients as in step 4.5.
4. Precool the test mass to T = 77 K by lowering it into the liquid nitrogen outside the copper chamber. Raise the test mass into the cold layer of nitrogen gas above the liquid nitrogen, wait for residual liquid nitrogen to evaporate off the test mass, and then lower the cold, dry test mass into the N₂-Ar mixture until it is fully submerged and within 2 cm of the liquid surface.
5. After any boiling and surface waves have disappeared, measure the apparent mass of the test mass. Calculate the solution density using its true mass m and T = 77 K volume V(77K) from step 3.7 according to the following:
   
6. Increase the solution density by flowing additional Ar until the desired initial density is obtained. Sample drops that sink can easily be lost, so the initial density should be at least a few percent higher than the expected sample density. The sample will then float, making it easier to keep track of it, and the N₂-Ar mixture density will then only need to be adjusted downward by adding liquid N₂.
7. Remove the Ar precooling coiled tube and allow to warm and dry before next use.

6. Cooling Drops of Sample Solution

1. Immediately prior to drop dispensing and cooling, repeat step 1.5 to mix the nitrogen/argon cryogenic liquid. Be careful not to introduce any bubbles.
2. Remove the sample tube's airtight cap. Using a clean 1 mL syringe, extract up to 1 mL of solution, and replace the cap. Attach a 27 to 33 G needle onto the syringe, and then push a small amount of sample through the needle to expel air and any residues from previous dispensing.
3. Two methods may be used to project sample drops into the N₂-Ar mixture.
   1. For samples with large non-aqueous component concentrations (>45% w/w) that can be vitrified with modest cooling rates, lightly press the syringe to displace a small (250 μm to 1 mm) diameter, ~10 nL to 1 μL drop that hangs from the needle tip by surface tension. Gently tap the needle to detach and project the drop toward the liquid N₂-Ar mixture.
   2. For samples that require faster cooling for vitrification, place the outlet of a gas tube connected to a vacuum generator (supplied by lab compressed air) in the gas space above the liquid N₂-Ar mixture, and gently suction away the cold gas layer that forms. This increases cooling rates for small samples¹¹.
      1. Carefully touch the needle tip to a 25-75 μm thick clear polymer strip to dispense a small volume (<10 nL, corresponding to a drop diameter <200 μm) of sample.
         NOTE: To obtain the smallest, most nearly spherical, and most easily removed drops, soak the strip in a hydrophobic coating solution for 10 min and let dry prior to sample dispensing.
      2. Grab the strip using an attached plastic or wood rod, and manually plunge the rod plus the strip into the liquid N₂-Ar mixture.
      3. Once the drop has solidified and boiling has ceased, grab the strip edge opposite the rod using tweezers. Flex the strip, keeping it immersed in the liquid N₂-Ar, until the sample drop pops off and floats to the surface.

7. Assessment of the State of the Sample

1. Using a long working distance (5-10 cm) binocular microscope and bright, cool illumination from an LED or fiber optic illuminator, carefully examine the drop while keeping it immersed in the liquid N₂-Ar. Vitrified drops should appear clear^12,13. Reject drops that are hazy or cloudy (likely containing more than one phase) and/or that show optical imperfections including cracks (which may be associated with voids that change the average density).
   NOTE: Painting the inside surface of the copper chamber to provide a black background can facilitate the identification of sample imperfections.

8. Determination of the Density of the Sample

1. The dispensed drop will initially float, sink, or (rarely) be neutrally buoyant in the N₂-Ar mixture. Floating drops may sometimes be held up by surface tension, tiny bubbles, or adhered ice particles. Inspect the entire drop surface with the microscope. Displace the drop downward from the liquid surface using a small (2-3 mm diameter, 10 cm long) precooled plastic or wood rod and observe its response.
2. If the drop sinks, increase the density of the liquid N₂-Ar using the procedure in step 4 until the drop becomes neutrally buoyant or floats.
3. If the drop floats, decrease the density of the liquid N₂-Ar by adding liquid nitrogen using a 1.8 mL cryovial. At large initial mixture densities (1.2-1.3 g/mL), adding N₂ in 1 mL increments gives appreciable density changes, but this should be increased toward 5 mL at low densities (0.8-0.9 g/mL). Gently mix the N₂-Ar (so as not to lose track of the sample drop) using the thin perforated copper foil sheet up-and-down in the copper chamber.
4. After each N₂ addition, use a small pre-cooled rod to gently displace the floating drop downward into the liquid, and observe its speed as it returns to the surface.
5. When the solution density has been adjusted so that the drop appears to be neutrally buoyant or ascends very slowly (<50 μm/s will ensure ~0.1% or better density accuracy for drops with volumes down to 50 pL), measure the N₂-Ar mixture density as described in step 5. Then add additional liquid N₂ until the drop first begins to slowly sink, and measure the N₂-Ar mixture density again. These two measurements will provide bounds on the drop density.