Unit 2 Test Review. Elements, Compounds, and Mixtures. Molar Mass & Percent Composition: SHOW WORK!
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1 Unit 2 Test Review Name Elements, Compounds, and Mixtures Molar Mass & Percent Composition: SHOW WORK! Chemical Molar Mass of the compound Formula PbO2 Pb: 1 x = O: 2 x = mole PbO2 = grams MnS % Composition of each element %Pb = %O= =. % 100 =. % (NH4)2SO4 XeF4
2 Empirical & Molecular Formula Find the mass of the empirical formula first. Then, divide the molar mass of the molecular formula by the mass of the empirical formula. This ratio will tell you how many times bigger the molecular formula is. Determine the Empirical and Molecular Formula for the following problems: 1. Succinic acid is a substance produced by lichens. Chemical analysis of succinic acid indicates that it is composed of 40.68% carbon, 5.08% hydrogen, and 54.24% oxygen and has a molecular weight of g/mol. Determine the empirical and molecular formulas for succinic acid. Empirical Formula Molecular Formula 2. Salicylic acid is the active ingredient of Aspirin. Salicylic acid is composed of % carbon, 4.38% hydrogen, and 34.76% oxygen and has a molecular weight of g/mol. Determine the empirical and molecular formulas for salicylic acid. Empirical Formula Molecular Formula
3 Molar Conversions: SHOW WORK! 1. How many grams are in 5.66 moles of calcium carbonate (CaCO3)? 2. What is the number of moles in 368 grams of H2SO4? 3. How many molecules are in 32.4 moles of KF? 4. How many grams are there in 4.99 x atoms of sodium? 5. A sample of Na2SO4 has a mass of 14.5 g. Calculate the number of Na2SO4 molecules present in the sample.
4 Solutions (Molarity): SHOW WORK! 1. What is the molarity of a solution in which 116 g of NaCl are dissolved in 1.5 L of solution? 2. What is the molarity of a solution in which 15.0 g of AgNO3 is dissolved in 250. ml of solution? 3. How many grams of NaNO3 should be used to prepare 2.50 L of a M solution? g of LiCl is dissolved to prepare a 0.75 M solution. What is the volume of the solution?
5 Dilutions: SHOW WORK! 1. How much concentrated 18 M sulfuric acid is needed to prepare 250 ml of a 6.0 M solution? 2. How much concentrated 12 M hydrochloric acid is needed to prepare 100. ml of a 2.0 M solution? 3. To what volume should 25 ml of 15 M nitric acid be diluted to prepare a 3.0 M solution? ml of 12 M hydrochloric acid is needed to produce 4.0 M solution? What is the final volume of the solution? How much water does the 50 ml of HCl need to be added to?
6 Beer s Law Reference table: Color of Solution Color Being Absorbed Wavelength of color being absorbed Green Red 700 nm Blue-green Orange-red 600 nm Violet Yellow 550 nm Red-violet Yellow-green 530 nm Red Green 500 nm Orange Blue 450 nm Yellow Violet 400 nm 1. There are four wavelengths on the colorimeter (430 nm, 470 nm, 565 nm, and 635 nm). Which of the four wavelengths would you choose to measure the absorbance of Potassium Permanganate, a violet colored solution? Justify your answer. 2. Known concentrations were made and the absorbance for each concentration were recorded in the data table below. The concentrations and absorbance were graphed and the line that best fits was determined. Absorbance vs. Concentration y = 0.96x If an unknown solution has an absorbance of 0.183, what is the concentration of the unknown solution? EXPLAIN how to find it and then SHOW WORK.
7 Separation Techniques 1. Determine the property which differs between the following pairs of substances: Ice & lemonade Salt & oil Mud and water Substances Homo-/Hetero-geneous Separation Method Water & rubbing alcohol 2. Determine the physical properties that each separation technique takes advantage of in order to separate the different components of a mixture Type of Mixture (heterogeneous Separation Technique Physical Properties and/or homogeneous) Distillation Decanting Filtration Evaporation Centrifuge Paper Chromatography Column Chromatography Physical/Chemical, Extensive/Intensive Properties 3. Circle the correct term that correctly completes the sentence for the next few problems 1. ( Physical or Chemical ) properties describe matter. 2. ( Physical or Chemical ) properties of a substance can be easily observed. 3. One can use their five senses to determine the ( Physical or Chemical ) properties of a substance. 4. ( Physical or Chemical ) properties usually describe how a substance reacts. 5. ( Physical or Chemical ) properties are not as easy to observe. 6. ( Physical or Chemical ) properties can be used to identify substances. 4. Classify each property as being a physical (P) or chemical (C) property. Also indicate whether it is an intensive (I) or extensive (E) property in each box.
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