Calculate the mass of Cu 2 SO 4. 7. 15. The following data was obtained during the titration of 2.0554 M hydrochloric acid with a 25.00 mL aliquot of barium hydroxide: Trial 1                   Trial 2                    Trial 3, Burette Final Reading                22.92 mL                25.32 mL                41.30 mL, Burette Initial Reading                 0.06 mL                 2.58 mL                 18.54 mL. Calculate the number of grams CaCl2 in 350. mL of a 0.250M solution. Click the Names button to go from the formula to the name. 65.5 mL of 0.300 M is diluted to a new molarity of 0.0600 M, how much water was added? How many milliliters of 6.2 M NaOH must react to liberate 2.4 L of hydrogen at STP? Calculate the theoretical yield in mL and the percentage yield of H2 gas. Calculate the volume of H2 gas produced at STP by the reaction of 400.0 mL of  0.800 M HCl with excess Zn. In a titration 0.200 M NaOH is used to neutralize 10.0 mL of H2SO4. Calculate the volume of 0.250 M H3PO4 required to neutralize 25.5 mL of. If 3.78 L of 0.960 M calcium fluoride solution is added to 6.36 L of water, what is the resulting concentration of each ion? Difference                       =          9.96 mL              Beware subtraction!!!! 11. 4. Calculate the amount of excess reactant. H3PO4 (aq) + 3NaOH (aq) → Na3PO4 (aq) + 3HOH (l), 3H+ (aq) + PO4-3 (aq) + 3Na+ (aq) + 3OH- (aq) → 3Na+ (aq) + PO4-3 (aq) + 3HOH (l). Calculate the mass of NaCl required to prepare 500.0 mL of a 0.500 M solution. 10. 4 Fe     +      3 O2             →                2 Fe2O3, Initial                     12.0 mol       8.0 mol                            0, End:                       1.3 mol        0 mol                               5.3 mol, 12. 4Al               +                  3O2                        →                2Al2O3, 84.0 g  x  1 mole             122 g  x  1 mole, 27.0 g                                32.0 g, I         3.111 mole                                3.8125 mole                                        0, C       3.111 mole                                2.333 mole                                          1.5556 mole, E        0                                                1.4795 mole                                        1.5556 mole, 47.3 g                                                  159 g. 9. 8. 39.22  -  15.62   =  23.60 mL  =  0.02360 L, 3NaOH       +        H3PO4                   →      Na3PO4       +        3H2O, 0.02360 L NaOH  x  2.557 mole  x   1 mole H3PO4, Molarity      =                                                1 L             3 mole NaOH                 =        0.8046 M. 5. If the [Al3+] concentration in 3.00 L of solution is .0275 M, calculate all of the ion concentrations and the molarity of a Al2(SO4)3 solution. 24. How many moles of NaCl are in 250. mL of a 0.200 M solution? Calculate the empirical and molecular formula. A2 Basic notes and equations on acids, bases, salts, uses of acid-base titrations - upgrade from GCSE! 28. What is the concentration of each ion in the solution formed when 16.5 g of Aluminum sulphate is, [Al2 (SO4) 3] =                                               342.3 g        =   0.0803 M, Al2 (SO4) 3   →      2Al3+ +         3SO42-, 0.0803 M              0.161 M      0.241M, 9. 1. In a titration 35.2 mL of 0.20 M H2C2O4 is used to neutralize 10.0 mL of NaOH. 0.200 L        x        0.300 moles x        267.72 g      =        16.1 g. 2. molar mass and molecular formula for the gas. 17. 9. What is the concentration of each ion in a 10.5 M sodium sulphite solution? 21. Calculate the molarity of the acid. Study Questions; Answers. 8. Calculate the molarity of the excess acid in the new solution formed. 10.0 g of Al2(SO4)3 is dissolved in 155 ml of water. 0.52 g NaCl x        1 mole                   x        1 L                         =        0.018 L, 58.5 g                              0.500 mole. Convert 88.3 g AgNO3 to formula units and then to atoms of O. 18. 12.6 g . Al2(SO4)3             →          2Al3+           +        3SO42-, 0.0138 M                          0.0275 M               0.0413 M. 38. Lesson             Day                  Date                 Topic, 1. 2 Al    +                  3 I2               →      2 AlI3, Initial                     12.0 mol                 15.0 mol                    0, End:                       2.0 mol                  0mol                      10.0 mol, 10. A 0.125 M solution is concentrated by evaporation to a reduced final volume of 100.0 mL and a molarity of 0.150 M. Calculate the original volume. 1. 22 does not divide evenly into 143. H2SO4                   +        2KOH         →, 0.0450 L H2SO4    x        0.320 moles x        2 mole KOH         x        1 L                  =        0.0576 L, 1 L                         1 mole H2SO4                 0.500 mole. Calculate the mass of AlCl3 required to prepare 250.0 mL of 0.250 M solution. 100. g Al2O3          x        1 mole         x        3 mole O2   x        22.4 L  =   32.9 L, 102 g                     2 mole Al2O3                   1 mole. 12. So, therefore, this soil is 2300 ppm of arsenic. 150.0 mL of 0.200 M HCl and 250.0 mL of 0.300 M HNO3 react with excess CaCO3. Determine the number of millilitres of 0.246 M AgNO3 required to precipitate all the phosphate ion in a solution containing 2.10 g of sodium phosphate. A burette filled with 2.557 M sodium hydroxide solution reads 15.62 mL initially. How many milliliters of hydrogen at   STP  can be generated by 500.0 mL 6.2 M NaOH completely reacting with excess Al. 4. - 'PET for Schools' Answer Key and Recording Scripts Practice Test (Complete PET). Whether you are looking for essay, coursework, research, or term paper help, or with any other assignments, it is no problem for us. 0.250 L        x        0.250 mol    x        133.5 g        =        8.34 g. 8. These problems have the answers worked out in detail. 10. 3. 150.0 mL of 0.200 M HCl and 250.0 mL of 0.300 M HNO, Chemistry 11 Calculations Practice Test # 1, Chemistry 11 Calculations Practice Test # 2. The site also includes flashcards other people have made. What volume of 0.300 M solution must be diluted to a final volume of 1200.0 mL and have a molarity of 0.2500M. With your fun and explanatory videos, relevant practice questions and helpful colour-coded multiple choice questions for each lesson (at SUCH an affordable price) I managed to get two 9s at GCSE for Combined Science last year. Na2CO3(aq)    +        2HCl(aq)        →      2NaCl(aq)     +     H2O(l)     +     CO2(g), 0.775 g Na2CO3      x      1 mole  x   2 mole HCl        x      1 L     x        1000 mL          =  13.4 mL, 106 g       1 mole Na2CO3         1.09 moles             1 L. 3. Calculate the energy produced by the complete reaction of 150. g H2. 0.5000 L x  0.100 mole             0.4000 L x  0.40 mole, I                   0.0500 mole                                0.16 mole, C                 0.0500 mole                                 0.100 mole, E                  0 mole                                         0.06 mole, [NaOH]       =        0.06 mole  =        0.07 M, Note that the final volume is 500.0 + 400.0 mL. If 1.78 L of 0.420 M barium fluoride solution is added to 2.56 L of water, what is the resulting, M1V1 = M2V2                                                          BaF2          →         Ba2+             +          2F-, (0.420)(1.78) = M2 (4.34)                   0.172 M                0.172 M                0.345 M. 10. Under Science, click on Elements. Calculate the volume of 0.500 M NaCl solution required to contain 0.0500 g of NaCl. 24. The solution is blue. 11. Then select a Question Style. Worksheet Template 4 6 Using Congruent Triangles Cpctc from Triangle Congruence Worksheet Answers , source: maveno. Calculate the mass of KBr required to prepare 450.0 mL of 0.350 M solution. 26. 19.9 g . H2SO4                   +        2KOH         →      2K2SO4                 +          2HOH, 0.1 L H2SO4    x   0.0200mol       x    2 mole KOH    x   1 L   x          1000 mL, 1L                          1 mole H2SO4       0.100 mol    1 L. 12. Calculate the theoretical yield of CO2. What volume of 0.200 M Ba (OH) 2 will this solution neutralize? Calculate the theoretical yield in mL and the percentage yield of H2 gas. 16. the questions. 64.5 L of HCl gas at STP are dissolved in water to produce an acid           solution. 20. 7. 15.0 mL of a solution of NaOH is diluted to a final volume of 250.0 mL and the new molarity is 0.0500 M. Calculate the original molarity of the base. Calculate the volume of 0.30 M BaCl2 solution that contains 6.00 g of KCl. Calculate the mass of H2C2O4.2H2O required to prepare 500.0 mL of a 0.200M solution. Molarity  H3PO4                  =        0.02000 L    x        2.000 mole  x          1 mole H3PO4. Calculate the mass of 2.35 x 1020  molecules of CO2. C        +        2Cl2              →                CCl4, Initial                     16.0 mol       34.0 mol                            0, End:                       0 mol           2.0 mol                            16.0 mol, 11. If you need professional help with completing any kind of homework, Success Essays is the right place to get it. Molarity and Dilutions, 9. How many moles of BaCl2 are in 250.0 mL of a 0.200 M solution? Determine the number of grams reactant in excess and number of grams H2O produced. From Lee Marek's web site, here's a way to remember the hydrocarbon prefixes. Calculate the energy produced by the complete reaction of 150. g H2. Analytical Chemistry 7e by Gary D. Christian 13. 100.0 g of an aqueous compound that is 45.49 % Pb, 12.31 % N, and 42.20 % O reacts with another compound that is 28.16 % N, 8.13 % H, 20.79 % P, and 42.91 % O. Calculate the molarity. Zn3 (PO4) 2            →      3Zn 2+          +        2PO43-, 5.55 M                            16.7                       11.1 M, 5. 15.2 g of Al reacts with 14.3 g O2 to produce Al2O3. Molarity Unit Review # 2, 12. buffers, titrations, titration curves, pH indicators, oxidation & reduction; voltaic cells, standard half-cell voltages, radioactivity, radioactive decay, nuclear fission, fusion, Practice Problems: Classification of Matter, Practice Problems: Naming compounds from formula and vice versa, Practice Problems: Periodic Table and simple ionic compounds, Practice Problems: Percent composition and empirical formula, Practice Problems: Writing and classifying equations, Answers to Worksheet of mass mole conversions, Practice Problems: Determining whether a precipitate forms, Electron configuration practice (interactive), Web site with practice finishing Lewis structures. Change 9.7x1019 atoms Fe to moles. 0.1000 L  x  0.200 mole   =    0.0200 mole HCl, 0.2000 L  x  0.100 mole   =    0.0200 mole HBr, 0.175L  x  0.100 mole   =    0.0175 mole Ba(OH)2, I           0.0400 mole                0.0175 mole, C        0.0350 mole           0.0175 mole, E         0.0050 mole                0.0000, Total Volume =  100.0 mL  +  200.0 mL  +  175 mL   =   475 mL. Calculate the volume of 0.40 M KCl solution that contains 8.00 g of KCl. 0.250 mol    x              L                      =        1.09 L. 14. 15. What is the [phosphoric acid]? What volume of 0.100M KOH will it neutralize? 2.9 L of HCl gas at STP is dissolved in 225 mL of water, calculate the molarity of the acid solution. How many grams of silver nitrate must be used in the preparation of 150. mL of 0.125 M solution. Calculate the mass of NaCl required to prepare 360.0 mL of a 0.35 M solution. Calculate the weight of H2C2O4.2H2O required to make 750.0 mL of a 0.480 M solution. 4. READ PAPER. Volume of 0.200 M NaOH         25.3 mL       25.8 mL       25.6 mL. Change 2.66 moles of H2O to molecules. ", Practice Problems from the ChemTeam: Partial pressure problems; Some answers will be used more than once. BaS (aq)        +        2KOH(aq)     →      Ba(OH)2(s)   +        K2S(aq), Ba2+    +        S2-      +        2K+    +        2OH-           →      Ba(OH)2(s)   +          2K+     +            S2-, Ba2+   +        2OH-           →      Ba(OH)2(s), 24. H2SO4                   +                  2XOH       →, 0.2500 L  x  0.100 mole                      0.1000 L   x  0.400 mole        +     0.2000 L   x  0.200 mole, 1 L                                                         1L                                                            1L, I         0.0250 mole                              0.0800 mole, C       0.0250 mole                               0.0500 mole, E        0                                               0.0300 mole, [NaOH]       =        0.0300 mole                    =        0.0545 M. 37. In a titration 22.5 mL of 0.100 M HCl ia required to neutralize 20.0 mL of Ba(OH)2 . 55.6 g of NaCl is dissolved in 562 mL of water, calculate the molarity. Calculate the mass of NaCl required to prepare 256 mL of a 0.35 M solution. HCl         +      CaCO3        ®      CO2      +      CaCl2          +    H2O, 0.1500 L HCl    x   0.200 mole    x    1 mole CO2   x   44.0 g     =    0.660 g, 1 L                 2 mole HCl        1 mole, HNO3        +      CaCO3        ®      CO2      +      Ca(NO3)2              +    H2O, 0.2500 L HNO3    x   0.300 mole    x    1 mole CO2   x   44.0 g     =    1.65 g, 1 L                    2 mole HCl        1 mole. 0.250 L      x        0.200 mole     =     0.0500 moles. What is the concentration of each ion in the solution formed when 94.78 g of iron (III) sulphate, Fe2 (SO4)3   →      2Fe3+                +        3SO42-, 0.4309 M              0.8619 M              1.293 M, [Fe2 (SO4) 3]          =                                    399.9 g          = 0.4309 M, 6. 3. 27. Answer: was. Calculate the concentration of the acid. A empty beaker has a mass of 25.86 g. The same beaker is filled with 0.250 L with a solution of Cl2 and weighs 87.26 g. The solution is evaporated to dryness and the mass of the beaker and solid is 36.31 g. Calculate the molarity of the solution. Dilutions, 7. 17. models, pH and pOH, strong and weak acids and bases. What volume of 2.549 M NaOH is needed to fully titrate 50.0 mL of 1.285 M HCl solution ? 7. 150.0 g of NaCl is dissolved in 250.0 mL of water, calculate the molarity. 23. How many litres of a 0.300 M KCl solution contain 0.350 moles? 2 Na            46.0 g                              % Na                    =        32.4 %, 1 S               32.1 g                              % S                       =        22.6 %, 4 O              64.0 g                              % O                      =        45.0 %. 30. 18. Start by writing an equation. Calculate the molarity. 1.50 g of NaCl is dissolved in 100.0 mL of water. How many grams AlCl3 are in the solution? 4Al      +         302       →      2Al2O3, 56.3 g Al      x        1 mol           x        3 mol O2      x        32.0 g                    =        50.0 g O2, 27.0 g                    4 mol Al                 1 mol. Worksheet # 10              Molarity Unit Review # 1. 16. One sig fig is lost!!! A 10.00 mL sample of 2.120 M sodium hydroxide solution is placed in a 250.0 mL Erlenmeyer flask. Thank you in advance! Determine the mass of the reactant in excess and the limiting reactant. 5. 100.0 mL of 0.100 M H2SO4 reacts with 50.0 mL of 0.20 M NaOH, calculate the concentration of the excess acid. What volume of 1.146 M KOH is needed to fully titrate 20.8 mL of 0.557 M H2SO4 solution ? In a titration 0.250 M KOH is used to neutralize 25.0 mL of H3PO4. 88.3 g   x   1 mol       x    6.02 x 1023 FU      x        3 atoms O   =        9.39 x  1023 atoms O, 169.9 g                        1 mol                 1 FU. Worksheet # 11    Molarity Unit Review # 2. 2. 250.0 mL of 0.100 M H2SO4 reacts with 100.0 mL of 0.400 M NaOH and. What is the molarity of the base? Molarity      =                                      267.72 g      =        3.36 M. 5. 2. Calculate the mass of CuSO4.5H2O required to prepare 100.0 mL of 0.100 M solution. What is the concentration of each ion in a 5.55 M zinc phosphate solution? 11. 50.0 mL of 0.200 M Na3PO4 solution is mixed with 150.0 mL of 0.400 M Na2CO3. Molarity      =                                      303.76 g                =        0.519 M. 1. The first letter of each word in the following statement is the 1st letter of each of the 10 alkanes in order. M1(220.0)             =        (0.0500)(470.0), M1                         =        0.107 M. 5. 2. Worksheet of Problems from the ChemTeam on density, mass percent, molality and molarity. 2Al(s)  +        6NaOH(aq)     →        2Na3AlO3(aq)              +         3H2(g). What is the, empty beaker has a mass of 25.86 g. The same beaker is filled with 0.250 L with a solution of Cl, 31. Calculate the volume of 0.50 M NaOH required to neutralize 35.0 mL of. 150.0 mL of 0.025 M NaOH solution is added to 150.0 mL of water. 15. 8. Calculate the mass of NaCl required to prepare 565.0 mL of a 0.450 M solution. 9. Calculate the mass of 2.25 x 105 mL of H2 gas at STP. Zn (CH3COO) 2    → Zn 2+       +        2CH3COO-, 1.22 M                       1.22M              2.44M, 11. Cheap essay writing sercice. 56.3 g of CuSO4.8H2O is dissolved in 30. mL of water, calculate the molarity. How many moles Al are required to produce 300. g Al2O3? 2. How many moles of Al2O3 are produced by the reaction 200. g Al? 1.5 L of HCl gas at STP is dissolved in 225 mL of water, calculate the molarity of   the acid solution. 2. 6. What volume of 0.200 M H2SO4 is required to neutralize 25.0 mL of 0.300 M NaOH? 4. Calculate the volume of 0.250 M H2SO4 required to neutralize 20.0 mL of 0.100 M NaOH. 3AgNO3(aq)    +    Na3PO4(aq)     →    Ag3PO4(s)      +     3NaNO3(aq). Beware subtraction!!!! Calculate the concentration. A empty beaker has a  mass of 29.86 g. The same beaker is filled with 0.250 L with a solution of CaCl2 and weighs 87.26 g. The solution is evaporated to dryness and the mass of the beaker and solid is 62.31 g. Calculate the molarity of the solution. Molarity =                     133.5 g           =     3.745 M     AlCl3    →    Al3+       +       3Cl-, 3.745 M                     3.75 M       11.2M. 25.4 L of HCl gas at STP are dissolved in 2.5 L of water to produce an acid solution. Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 3. One sig fig is lost!!! Calculate the volume of 0.250 M NaCl solution that would contain 0.17 g NaCl. Use the Worksheet tab of the Gizmo to calculate each analyte concentration. Calculate the mass of KCl required to prepare 250.0 mL of 0.250 M solution. Convert 5.9 x1025 H2 molecules to grams. 18. 20. mol H2 reacts with 8.0 mol O2 to produce H2O. Calculate the volume of 0.500 M NaCl solution required to contain 0.52 g of NaCl. Chemistry 11 Calculations Practice Test # 1, 13. 6. 150.0 mL of 0.200 M HCl and 250 mL of 0.300 M HNO3 react with excess CaCO3. 50.0 mL of 0.025 M NaOH solution is added to 150.0 mL of water. 16. Titrations Lab 2      Homework WS # 5, 6. 2H2       +        O2         →      2H2O  +  130. H2SO4                   +                  2NaOH                 →      Na2SO4          +        2HOH, 0.2000 L  x  0.200 mole            0.250 L  x  0.40 mole, 1 L                                             1 L, I                   0.0400 mole                              0.100 mole, C                 0.0400 mole                              0.0800 mole. 5. 8. Lesson Summary. To introduce the lab the class will first review the collision theory of chemical reactions. 22. Combined gas law problems and answers to Examples and Problems, Worksheet of Molarity Problems from the ChemTeam. 11. 3. 85.0 mL of a solution of NaOH is diluted to a final volume of 290.0 mL and the new molarity is 0.0500 M. Calculate the original molarity of the base. Calculate the mass of Cu2SO4.6H2O required to prepare 200.0 mL of a 0.300M solution. How many grams Al2(SO4)3 are in the solution? 13. Identify the limiting reactant. Molarity Unit Review # 1, 11. Calculate the number of formula units in 250. g  CaCl2. 0.0500 L HCl  x   1.285 mol   x   1 mole NaOH      x   1L          =       0.0252 L, 1 L                1 mole HCl            2.549 mole. 15. 7. Calculate the volume of H2 gas produced at STP by the reaction of 150.0 mL of 0.500 M HCl with excess Zn. 25.2 g of NaCl is dissolved in 365 mL of water, calculate the molarity. Calculate the volume of H2 gas produced at STP by the reaction of 350.0 mL of 0.600 M HCl with excess Zn. 23. 14. 32.6%         ,           22.5%       ,          44.9%. 60.0 g of Al react with 60.0 g of O2. 6. 4. What is the concentration of each ion in a 1.22 M zinc acetate solution? Study Questions; Answers. 4Al  +  302   →      2 Al2O3. 100.0 mL of 0.200 M MgCl2 reacts with 300.0 mL of 0.400 M AlCl3, calculate all ion concentrations. 100.0 mL of 0.200 M HCl, 200.0 mL of 0.100 M HBr, and 175 mL of 0.100 M Ba(OH)2. Calculate the volume of 0.450 M H2SO4 required to neutralize 25.0 mL of, 0.025 L NaOH      x        0.200 mol    x        1 mol H2SO4              x           L                  =        0.00556 L, L                        2 mol NaOH                   0.450 mol. 20.0 mL of 0.200 M NaOH solution is diluted to a final volume of 100.0 mL, calculate the new concentration. 8. 0.250 g        x        1 mole         x        1 L               =        0.0102 L. 14. 15. 10. Ga2(SO4)3   →      2Ga3+          +        3SO42-, 0.0150 M              0.0300 M              0.0450 M. 14. 25.0 g of CuSO4.8H2O is dissolved in 25.0 mL of water, calculate the molarity. 84.0 g of Al reacts with 122g O2 to produce Al2O3. Calculate the molarity of the solution formed when 200 g of NaCl is dissolved in. Calculate the number of grams barium carbonate that can be precipitated by      adding 50.0 mL of 0.424 MBa(NO3)2. 100.0 mL of 0.250 M HCl solution is diluted by adding 250.0 mL of water, calculate the new concentration. 28 g of KCl is dissolved in 225 mL of water, calculate the molarity. Write the formula, complete, and net ionic equation for each. 1. 13. Zn      +   2HCl       →    H2     +           ZnCl2. 6. Titrant Analyte Indicator Titrant volume 4Al      +         3O2       →      2Al2O3. SCH3U Exam Review with Answers LONG KJ. The chemical laboratory is a place where you can perform in actual the different reactions that you had learnt in the books or heard in lectures. Scoring the Practice Test The worksheet on page 51 lists the correct answers to . Calculate the number of formula units of KCl in 200.0 mL of 0.300 M solution. 16 g of Ca react with water. The following data was obtained during the titration of 2.0554 M hydrochloric acid with a 25.00 mL aliquot of barium hydroxide: Burette Final Reading                  22.92 mL                25.32 mL                41.30 mL, Burette Initial Reading               0.06 mL                 2.58 mL                 18.54 mL, Vol. AlCl3             →          Al3+           +        3Cl-, 20.0         0.300 M                     0.150 M                0.450 M, CaF2              →         Ca2+           +        2Cl-, 20.0         0.300 M                      0.150 M                 0.300 M, 32. Ionic nomenclature interactive quizzes: Click the Formulas button to go from the name to the formula. M                                 0.200 M, [ H2SO4]                =        0.03435 L   x   0.200 mole   x  1 mole H2SO4       =    0.137 M, 10. 19. Which element in the n 4 13a. Molarity 1, 2. 2Al(s)  +        6NaOH(aq)    →        2Na3AlO3(aq)            +         3H2(g). 50.0 g of NaCl is dissolved in 200.0 mL of water, calculate the molarity. 32. AlCl3            ®      Al3+    +        3Cl-, 0.200 M                                    0.600 M, 0.1000 L     x    0.200 mole   x   133.5 g       =        2.67 g. 17. Calculate the volume of 0.400 M H2SO4 required to neutralize 25.0 mL of 0.200 M NaOH. 11. How many millilitres of 1.09 M HCl are required to react with a solution formed by dissolving 0.775 g of sodium        carbonate? measurement, significant figures, precision & accuracy, conversion factors, matter, atomic theory, intro to Periodic Table, formulas & names of compounds, mole, molar mass, percentage composition, calculating formula, chemical equations, stoichiometry, limiting reactant, yield, precipitation reactions, acid-base reactions, molarity, solution stoichiometry, atomic spectra, Bohr model for H atom, electron configurations, quantum numbers, periodic trends, covalent & ionic bonding, Lewis structures, molecular geometry & polarity, orbital hybridization, sigma and pi bonding, saturated, unsaturated, & aromatic hydrocarbons, functional groups, polymers, gas laws, gas stoichiometry, partial pressure, kinetic theory, intermolecular forces, types of solids, vapor pressure, phase diagrams, types of solutes, concentration, solubility, colligative properties, reaction rate, factors affecting rate, activation energy, reaction mechanisms, catalysis, equilibrium calculations, equilibrium constant, Le Chatelier’s Princinciple. 2H2       +        O2     →         2H2O   +   130. What volume of 1.146 M KOH is needed to fully titrate 20.8 mL of 0.557 M H, Note that the final volume is 250.0 + 200.0 mL, 1. 50g   x      1 mole   x           1 L       =    1.7 L. 8. [NaOH]       =        0.020 mole  =        0.044 M, 0.4500 L                                    Note that the final volume is 250.0 + 200.0 mL. 25. 14. 28. Sr(OH)2 (aq) +        CuSO4(aq)    →      Cu(OH)2 (s)  +        SrSO4(s), Sr2+   +        2OH-           +        Cu2+            +        SO42-           →          Cu(OH)2 (s)  +        SrSO4(s), 26. A2 Case studies of buffer function 6H 2 O required to prepare 200.0 mL of a 0.300M solution. H2SO4         +        2NaOH       →      Na2SO4       +        2HOH, 0.250 L NaOH  x  0.250 mole  x  1 mole H2SO4    x        1 L     x        1000 mL          =        156 mL, 1 L          2 mole NaOH            0.200 mole            1 L. 9. 6. 2Na3PO4 (aq) + 3Ca(NO3) 2 (aq) → Ca3 (PO4) 2 (s) + 6NaNO3 (aq), Na+ (aq) + 2PO43- (aq) +3Ca2+ (aq) + 6NO3- (aq) → Ca3 (PO4) 2 (s) + 6Na+ (aq)+ 6NO3- (aq), 3Ca2+ (aq) + 2PO43- (aq) → Ca3 (PO4) 2 (s). 14. 0.100 L        x        0.100 mole            x        249.7 g        =        2.50 g, 1 L                                   1 mole. 0.300 L         x   0.500 moles   x    1 mole H2      x       22.4 L     =   1.68 L, 1 L                 2 mole HCl             1 mole. Calculate the volume of 0.500 M NaCl solution required to contain, 14. Calculate the volume of 0.500 M KOH required to neutralize 45.3 mL of  0.320 M H2SO4 . How many litres of O2 gas are required to produce 100. g Al2O3? 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