Let's take a moment to review what we've learned about parts per million's definition and calculation. 0.250 g        x        1 mole         x        1 L               =        0.0102 L. 14. 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. Calculate the volume of H2 gas produced at STP by the reaction of 300. mL of 0.500 M HCl with excess Zn. Practice: Perform the following titrations and determine the concentrations of the following solutions. Molarity 1, 2. A burette filled with 2.000 M sodium hydroxide solution reads 20.20 mL initially. Calculate the mass of NaCl required to prepare 500.0 mL of a 0.500 M solution. In a titration 35.2 mL of 0.20 M H2C2O4 is used to neutralize 10.0 mL of NaOH. 19. 8. If the actual yield of NaCl in the last question was 200. g, calculate the percentage yield of NaCl. Calculate the molarity of the solution. 2HCl   +   Na2SO3(aq)       +  2NaOH(aq)          →      2NaCl(aq)    +          H2O(l) +     SO2(g). Calculate the empirical and molecular formula. 2. The following data was obtained during the titration of 1.0097 M sodium hydroxide with a 25.00 mL aliquot of hydrofluoric acid: Trial 1                   Trial 2                    Trial 3, Burette Final Reading                 34.56 mL                39.42 mL                44.20 mL, Burette Initial Reading               14.94 mL                19.86 mL                24.66 mL. 9. How many moles of NaCl are in 250. mL of a 0.200 M solution? What volume of 0.200 M H2SO4 is required to neutralize 25.0 mL of 0.300 M NaOH? 26. 84.0 g of Al reacts with 122 g O2 to produce Al2O3. Worksheet Template 4 6 Using Congruent Triangles Cpctc from Triangle Congruence Worksheet Answers , source: maveno. 25. Stoichiometry, 4. Molarity and Dilutions, 9. If the actual yield of the product containing lead is 60.0 g, calculate the         percentage yield. 0.350 L HCl          x        0.600 mol    x        1 mol H2      x        22.4 L          =        2.35 L, L                        2 mol HCl             1 mol. 13. 16. 18. 15. 20.0 mL of 0.200 M NaOH solution is diluted to a final volume of 100.0 mL, calculate the new concentration. 3. Calculate the energy produced by the complete reaction of 150. g H2. After titrating a. And specify exactly as the directions are asking. Chemistry 11 Calculations Practice Test # 2. H3PO4 (aq) + 3NaOH (aq) → Na3PO4 (aq) + 3HOH (l), 3H+ (aq) + PO4-3 (aq) + 3Na+ (aq) + 3OH- (aq) → 3Na+ (aq) + PO4-3 (aq) + 3HOH (l). 0.250 g H2SO4      x        1 mole                   x        1 L                         =          0.0102 L, 98.12 g                            0.250 mole. Pick two formulas that match each classification: 1.   a                   b                  Acid                                 a)  HCl                   e) KOH, 2.   c                   d                  Covalent Nonacid            b) CH3COOH          f) NH4Cl, 3.   h                   f                   Salt                                  c)  CH4                   g) Ba(OH)2, 4.   e                   g                  Base                                 d)  HOH                 h)  AgNO3, 5. How many grams Al2(SO4)3 are in the solution? 12. Objectives: 1. How many milliliters of 6.2 M NaOH must react to liberate 2.4 L of hydrogen at STP? If the sodium ion concentration is 0.450 M in 150.0  mL of a Na3PO4 solution. How many litres of 0.200 M AgCl are needed to provide 50 g of AgCl? What is the barium hydroxide, 46.30  -  33.10   =  13.20 mL  =  0.01320 L, 2HNO3         +          Ba(OH)2         →      Ba(NO3)2                  +          2HOH, 0.0132L HNO3      x  1.52 mole   x  1 mole Ba(OH)2, Molarity      =                                                1 L            2 mole HNO3            =          0.402 M. 4. How many litres of a 0.200 M KCl solution contain 0.250 moles? 0.2500L       x        0.250 mole            x        74.6 g          =        4.66 g KCl. Calculate the mass of H2C2O4.2H2O required to prepare 500.0 mL of a 0.200M solution. 16. 8. 6. Calculate the molarity of excess base. What is the [phosphoric acid]? Calculate the volume of 0.250 M NaCl solution that would contain 0.17 g NaCl. 25.0 g of CuSO4.8H2O is dissolved in 25.0 mL of water, calculate the molarity. 0.250 L      x        0.200 mole     =     0.0500 moles. Convert 88.3 g AgNO3 to formula units and then to atoms of O. 24. 850.0 mL of 0.280 M KOH solution is diluted to a final volume of 1000.0 mL, calculate the new concentration. 0.0250 L NaOH    x        0.300 mole    x      1 moles H2SO4      x        1 L             =    0.0188 L, 1 L                        2 NaOH                           0.200 mole. Calculate the molarity of the excess acid in the new solution formed. 40.6g of KBr is dissolved in 500.0 mL of water, calculate the molarity. 4. 7. Calculate the volume of 0.50 M NaOH required to neutralize 35.0 mL of. 2H2       +        O2     →         2H2O   +   130. 8. 2. 3. 2H2+O2             →      2H2O  +        130KJ, 150 g H2      x        1mol            x        130 KJ        =        4.83 x 103 KJ, 2.02 g                              2 mol. In a titration 35.7 mL of 0.250 M H3PO4 is used to neutralize 25.0 mL of KOH. 17. Calculate the molarity of the base. 0.52 g NaCl x        1 mole                   x        1 L                         =        0.018 L, 58.5 g                              0.500 mole. Zn3 (PO4) 2            →      3Zn 2+          +        2PO43-, 5.55 M                            16.7                       11.1 M, 5. Calculate the theoretical yield in mL and the percentage yield of H2 gas. 65.5 mL of 0.300 M is diluted to a new molarity of 0.0600 M, how much water was added? Na3PO4             →      3 Na+           +        PO43-, 50.0          0.200 M                     0.150 M                0.0500 M, Na2PO4             →      2 Na+           +        CO32-, 150.0       0.400 M                      0.600 M                   0.300 M, 8. How many moles Al are required to produce 300. g Al2O3? 40.0 mL of 0.400 M NaOH solution is diluted to a final volume of 200.0 mL,    calculate the new concentration. In a titration 0.200 M NaOH is used to neutralize 10.0 mL of H2SO4. Click "check structure" to check your answer. 1.26 g of AlCl3 are dissolved in 160.0 ml of water. What is the concentration of each ion in a 1.22 M zinc acetate solution? Calculate the volume of 0.500 M NaCl solution required to contain 0.52 g of NaCl. 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. How many grams of H2 would be needed to produce 260. 25.5 mL of 0.100 M HCl reacts with excess Zn to produce 25.3 mL of H2 gas at STP. Web site with practice finishing Lewis structures: Select a compound from the drop down menu. 16. Calculate the volume of 0.40 M KCl solution that contains 8.00 g of KCl. Calculate the molarity of the solution. How many moles of Al2O3 are produced by the reaction 200. g Al? 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. What volume of 0.200 M Ba (OH) 2 will this solution neutralize? Calculate the percentage composition of Al2(SO4)3 to three significant figures. Determine the mass of the reactant in excess and the limiting        reactant. 28. 200.0 mL of 0.200 M KOH, calculate the concentration of the excess base. 6H 2 O required to prepare 200.0 mL of a 0.300M solution. How many milliliters of hydrogen at   STP  can be generated by 500.0 mL 6.2 M NaOH completely reacting with excess Al. How many grams of 02 are required to consume 56.3 g Al? Calculate the STP volume of 10.0 g of CO2 gas. In a titration 22.5 mL of 0.200 M H3PO4 is required to neutralize 10.0 mL of KOH. Chem 11 Exam Review with Answers - Free download as PDF File (.pdf), Text File (.txt) or read online for free. NaOH         +        HCl             →      NaCl  +        H2O, 0.01000 L NaOH   x   2.120 mole      x      1 mole HCl, Molarity      =                                                  1 L                      1 mole NaOH    =   2.13 M HCl. More Study Questions; Answers. 6. 150.0 g of NaCl is dissolved in 250.0 mL of water, calculate the molarity. Answers to Worksheet of mass mole conversions, Practice Problems: Determining whether a precipitate forms; Answers, Electron configuration practice (interactive) NaCl(aq)        +        Cu(NO3)2(aq)           →, No reaction, both possible products have high solubility, 27. 7. 1. Write the formula, complete, and net ionic equation for each. 0.300 L        x        0.520 moles x        309.56 g      =        48.3 g. 3. As a member, you'll also get unlimited access to over 83,000 lessons in math, English, science, history, and more. Ph virtual lab worksheet answers Electrochemical cells involve the transfer of electrons from one species to another. 14. 11. Calculate the mass of Cu(NO3)2.6H2O required to prepare 100.0 mL of 0.200 M solution. 100. g Al reacts with excess O2 to produce 150. g Al2O3 according to. Calculate the mass of Cu 2 SO 4. Na3PO4              →            3Na+           +        PO43-, 0.150 M                          0.450 M                 0.150 M, Worksheet # 12   Chemistry 11 Calculations Practice Test # 1. 8.5 L of HCl gas at STP is dissolved in 325 mL of water, calculate the molarity of the acid solution. 13. 6.00 g                    x        1 mol           x        1 L               =        0.15 L, 9. HCl   +         NaOH   →    NaCl    +      H2O. Sr(OH)2 (aq) +        CuSO4(aq)    →      Cu(OH)2 (s)  +        SrSO4(s), Sr2+   +        2OH-           +        Cu2+            +        SO42-           →          Cu(OH)2 (s)  +        SrSO4(s), 26. 220.0 mL of a solution of NaOH is diluted by adding 250.0 mL of water to produce a new molarity of 0.0500 M. Calculate the molarity of the base. 15. 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. Read the instruction page and then click "Play Now.". How many grams of AgCl are required to prepare 150 mL of 0.200 M solution? 4Al      +         3O2       →      2Al2O3. 30. 10. How many grams of Al2O3 are produced? Calculate the [NaOH] due to excess NaOH in the new solution produced by mixing 100. mL, HCL            +                  NaOH         →      NaCl      +                  HOH, 0.100L   x   0.200 mole  =   0.0200 mol         0.100L x 0.300 mol  =   .030 mole, 1 L                                                         1 L, I                                    0.0200 mole                    0.0300 mole, C                                  0.0200 mole                    0.0200 mole, E                                   0  mole                            0.0100 mole, Total Volume = 200 mL = 0.200 L           Molarity     =         0.0100 mole           =  0.0500 M. 11. 28. What volume of 0.200 M Ba (OH)2 will this solution neutralize? 16. If the [Ga3+] concentration in 2.00 L of solution is 0.0300 M, calculate the [SO42-] and the molarity of the Ga2(SO4)3 solution. Calculate the volume of H2 gas produced at STP by the reaction of 350.0 mL of 0.600 M HCl with excess Zn. Calculate the volume of 0.500 M NaCl solution required to contain 0.0500 g of NaCl. Thank you in advance! Calculate the empirical and molecular formula. There are two no reactions. 2. So, therefore, this soil is 2300 ppm of arsenic. Beware subtraction!!!! Calculate the molarity of the base. Molarity      =                                      267.72 g      =        3.36 M. 5. Calculate the concentration. M1(220.0)             =        (0.0500)(470.0), M1                         =        0.107 M. 5. 29. I recommend starting with the Video Tour. 23. Calculate the mass of KBr required to prepare 450.0 mL of 0.350 M solution. 17. 100 g of AlCl3 is dissolved in 200 mL H2O, calculate [Al3+] and [Cl-]. To introduce the lab the class will first review the collision theory of chemical reactions. SCH3U Exam Review with Answers LONG 14. 30. 50.0 mL of 0.200 M Na3PO4 solution is mixed with 150.0 mL of 0.400 M Na2CO3. M1V1 = M2V2                                                        CaF2           →                Ca2+              +        2F-, (0.960) (3.78) = M2 (10.14)                0.358 M                          0.358 M                    0.716 M. 4. Plus, get practice tests, quizzes, and personalized coaching to help you succeed. 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. Convert 5.9 x1025 H2 molecules to grams. 16. 3AgNO3(aq)    +    Na3PO4(aq)     →    Ag3PO4(s)      +     3NaNO3(aq). 18. Stop working on the test when 2 hours and 50 minutes have elapsed. 2NaCl(aq)     +        F2(g)   →      2NaF(aq)       +        Cl2(g), 2Na+     +     2Cl-    +        F2(g)   →      2Na+    +      2F-     +        Cl2(g), 2Cl-    +        F2(g)   →                2F-     +        Cl2(g), 25. 78.9 g of CuSO4.8H2O is dissolved in 500.0 mL of water, calculate the molarity. Calculate the volume of 0.400 M H2SO4 required to neutralize 25.0 mL of 0.200 M NaOH. What volume of 0.200 M Ba (OH). Answer: was. Calculate the volume of 0.30 M AlCl3 solution that contains 6.00 g of AlCl3. If you need professional help with completing any kind of homework, Success Essays is the right place to get it. 18. In a titration 12.5 mL of 0.200 M NaOH ia required to neutralize 10.0 mL of H2SO4. 7. 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 concentration. Cheap essay writing sercice. 9. Write the formula, complete, and net ionic equation for each. 22. One sig fig is lost!!! 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. A 0.350 M solution is concentrated by evaporation to a reduced final volume of 100.0 mL and a molarity of 0.825 M. Calculate the original volume. 22. 8. 2 Al              54.0             %Al =         54.0             x        100%                    =          15.8 %, 3 S               96.3             %S =           96.3             x        100%                    =          28.1 %, 12 O            192.0           % O =         192.0           x        100%                    =          56.1%, 342.3                               342.3. 13. 1. Volume of 0.200 M NaOH         25.3 mL       25.8 mL       25.6 mL. 4. 50.0 g of NaCl is dissolved in 200.0 mL of water, calculate the molarity. 8. 16 g of Ca react with water. Ni2 (SO4) 3             →      2Ni3+            +        3S042-, 0.274 M                          0.548M                 0.822M, Molarity =   94.5 g          x        1 mole. 3.745 M 3.75 M 11.2M HCl with excess CaCO3 soil is 2300 ppm of arsenic been reached ),... The de Please help L. 14 prepare 256 mL of 0.300 M solution many millilitres of M! 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Kcl ] = 0.600 M in 100.0 mL of water 10.0 g of gas... 1.26 g of CuSO4.6H2O is dissolved in water to produce an acid solution burette... Following burette readings: burette final = 22.04 mL, calculate the concentration of the reactant in excess and percentage., 0.274 M 0.548M 0.822M, molarity = 94.5 g x 1 L = 0.018 L?!