If you're using a P-2 to pipet 1 μl, you'd set it at 1.00 μl, so 1.00 μl would be the correct answer for a quiz. Most of the lab experiments are done with a Pipetman, which has a practical precision of three significant figures. Significant figuresīe realistic about your significant figures the level of precision should reflect the way you would do the experiment. You don’t need to remember that a nanogram is 10 -9 grams just remember that there are 1000 ng in 1 μg and 1000 μg in 1 mg and 1000 mg in 1 g. For each step, you multiply or divide by 1000. Alternatively, you could remember: m > μ > n > p. You could memorize this list, and you'll be ready to do the various conversions in the Bio 6B lab. 1 μg = 1 microgram = 10 -3 mg = 10 -6 g (that’s a greek letter μ, not a u).The prefixes we normally use in this course are in multiples of 1000: If you do a 10-fold dilution, you'll have a concentration of 0.1X. For example, if you start with an unknown concentration of a bacterial culture, you could call it X. You'll use the mysterious X frequently in lab. We’ll use these units for DNA and proteins, which are variable in size. g/l, or μg/μl, or similar units (mass over volume).Percent (%) usually means mass/volume: For example, if you want to make a gel with an agarose concentration of 0.5%, you would use 0.5 g agarose per 100 ml of solution.In this lab, we’ll usually express concentrations in μM or mM. Molar (M), defined as moles of solute per liter of solution.I'm sure you are familiar with these from your chemistry and physics classes:Ĭoncentration, or the amount of stuff in a given volume, can be given several ways: For the labs in this course, there are only a few kinds of units, and the prefixes that go with them. If you work in a lab, you need to pay attention to units of measurement. Almost all of them are either conversions or dilutions, so two basic kinds of equations will solve all your problems.

Therefore the boiling point elevation would be 2oC.You'll need to do a lot of calculations in Bio 6B. For example the boiling point of pure water at 1.0atm is 100oC while the boiling point of a 2% saltwater solution is about 102oC. The boiling point elevation is the amount that the boiling point temperature increases compared to the original solvent. What is the boiling point of a solution when compared to the pure solvent? Hence a 1.00 m NaCl solution will have a boiling point of about 101.02☌.

The increase in the boiling point of a 1.00 m aqueous NaCl solution will be approximately twice as large as that of the glucose or sucrose solution because 1 mol of NaCl produces 2 mol of dissolved ions. Will the elevation in boiling point be the same for 1’m NaCl 1M glucose Why? NaCl dissociate to give two ions while BaCl.

Since both the salt solution have same concentration therefore the salt which gives maximum number of ions will show higher boiling point. Which will have greater boiling point 0.1 molar sodium chloride or 0.1 molar barium chloride solution in water? The number of particles are more in NaCl the elevation in boiling point is higher. 0.1 M NaCl will dissociate into Na + and CI – whereas 0.1 M sugar solution will not dissociate. Solution: The elevation in boiling point depend on the dissociation of particle in solution. Will the elevation in boiling point be same for 0.1 molar aqueous solution of NaCl and glucose explain?

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