LAB 2: BIOCHEMICAL CALCULATIONS; PROPERTIES OF SOLUTIONSThe purposes of this lab session are for you to develop competencies in (1) the use of logarithms and exponentials in calculations, (2) the description of physical characteristics of solutions, and (3) using concentrations of solutions in calculations. Bring your calculator to every lab session.Higher Order Objective:- Students will be able to define physical properties of solutions and use concentrations in biochemical calculations.Lower Order Objectives:- Know how to use a scientific calculator, including exponents, scientific notation, and logarithms.- Understand the concept of solubility and the terms solute and solvent.- Understand the different types of solutions (molar and percent) and how to make dilutions. - Understand how to calculate concentration and how to prepare different solutions.- Understand the effect of temperature on solubility and the concept of supersaturation.- Understand the concept of polar and non-polar properties of compounds and how these properties affect solubility in various solvents.Bring your calculator to all lab sessions.It is important that you learn how to use your calculator and how to do all of the calculations in this exercise because you will encounter these types of calculations throughout this course and in your future careers in the health sciences. If you have difficulty with these calculations, get help from your instructor. Most everyone will have some difficulty with this exercise, and we will be happy to spend asmuch time as necessary with you.Useful material in your textbook is found in Chapter 6: Solutions. See in particular Sections 6.1 (Properties of Solutions), 6.2 (Concentration based on mass), and 6.3 (Concentration of Solutions: Moles and Equivalents), and the related practice problems and end-of-chapter summary and review problems. PRE-CLASS ASSIGNMENT BEFORE coming to class, you need to read Sections A, B and C. You should also complete the practice problems in Section A. Then, you need to log into Sakai and take the short pre-class quiz to make surethat you understand the material covered in these sections.A. USING SCIENTIFIC CALCULATORSYou should already know how to use the common mathematical functions (addition, subtraction, multiplication, and division) and the memory function of your calculator. Recall that very large and verysmall numbers are most conveniently handled when expressed in scientific notation (a number between 1 and 10 with an exponential term denoting the position of the decimal point). Your calculator will have an exponent key (marked either EE for "enter exponent" or EXP or something similar). You should already know how to do calculations using scientific notation, if you need a review, here is a video explaining scientific notaion on calculators (https://www.youtube.com/watch?Biochem 107L3-2v=1jDfRhMl0z4). For this pre-class assignment, you will get some practical experience using the log/antilog functions on your calculator. LOGARITHMS: We will also use the log/anti-log functions on your calculator repeatedly in this course, particularly when we consider pH and acid-base balance. We will cover logarithms in moredetail at that time, but you need to start becoming familiar with their use. Logarithms can be thought of as exponents of the base 10. Think of logs in the following manner: number = 10 log of that numberConversely, the antilog is the number that the log of the number corresponds to. The table below illustrates the relationship between a number, its exponential form, and its log. Converting a logarithm back to its antilog is the exact reverse of calculating the log of a number. Make sure you can do these types of conversions on your calculator.For example, find the log of 36950; the log of 36950 is 4.5676. Another way of saying this is that 36950 = 104.5676. Although your calculator will calculate logs up to 8 decimal places, you should only record them to four decimal places.The antilog of 4.5676 is 36950. Note again that converting a log to its corresponding antilog is the reverse (or opposite) of converting a number to its corresponding log (the usual key for this is 2nd log or INV log, but this may vary with individual calculators).PRACTICE PROBLEMS: Find the logs of the numbers below; record them on a separate sheet. If the number is not already given in scientific notation, record it in that way below before determining the log. Always record logs to 4 decimal places. Include this problem set in your report.a) 1.265 g) 0.00137b) 26.53 h) 22000000c) 348.49 i) 22000d) 7695.3 j) 220e) 894341 k) 3.24 x 109f) 3987654 l) 3.24 x 10–9 N Exponential form Logarithm1 100 0.000010 101 1.000010,000 104 4.00000.0001 10–4 –4.00005 (5 x 100) 100.6989 0.6989500 (5 x 102)102.6989 2.698950,000 (5 x 104)104.6989 4.6989Biochem 107L3-3Find the antilogs of the numbers given below. Express them in real numbers and then in scientific notation (to 2 decimal places, always) and record both below. Include this problem set in your report. a) 0.3249 h) –3.4771b) 1.3249 i) 1c) 6.3249 j) 3d) –3.3249 k) 5e) 0.4771 l) 10f) 2.4771 m) 0g) –5.4771B. SOLUBILITY, MISCIBILITY, AND SOLUTIONSSOLUTIONS: There are two components to every solution. The dissolving medium, the solvent, and the material that is dissolved, i.e., the solute(s). For example, if we dissolve sodium chloride (NaCl; table salt) in water, sodium chloride is the solute and water is the solvent. The formation of a solution is governed by the properties of both the solute and the solvent. Because water is a polar molecule (the oxygen has a partial negative charge while the two hydrogens have slight positive charges), water is an effective solvent. Solutions in which water is the solvent are called aqueous solutions. Solutes that are polar molecules, such as sugars and ionic compounds, are generally soluble in water. Ionic compounds are compounds that dissociate into positively and negatively charged ions (e. g., sodium chloride, calcium sulfate, calcium chloride). NaCl  Na+ + Cl–CaSO4  Ca++ + SO4=CaCl2  Ca++ + 2 Cl–When a crystal of sodium chloride is placed in water, the water molecules collide with and exert an attractive force upon the Na+ and Cl- ions on the crystal surface. The attractive forces between the bombarding solvent molecules and the solute ions will overcome the attractive forces within the solute