Can one calculate the number of moles of air? If so, calculate the number of moles in 1 kg of air (making sure your calculation, units and assumptions are fully explained); If not, explain why it is not possible to

78,458 results
  1. Chemistry

    Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. Solution A: 10.0 mL 3.0e-4M bromescol green

  2. Chemistry

    In this experiment 4.0g of ferrous ammonium sulfate is used. Assuming everything else is added in excess; calculate the theoretical yield of the iron complex. Work through the entire reaction sequence; do not simply assume the number of moles of limiting

  3. chem

    A 2.241 g sample of nickel reacts with oxygen to form 2.852 g of the metal oxide. Calculate the empirical formula of the oxide. 1)NiO Give the number of moles of each element to support you answer. moles of Ni 2) 1.339 mol moles of O 3)1.34 mol I know #1

  4. physics

    A 22.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.40 105 Pa and temperature of 22.0°C. (a) Calculate the temperature of the gas in Kelvin. K (b) Use the ideal gas law to calculate the number of moles of gas in the tank. mol (c) Use the

  5. Chemistry

    Two flasks A and B of equal capacity of volume contain SO3 and Co gas respectively under similar conditions of temperature and pressure. Then, which of the following statement is true? (1) A has twice the number of moles as that B. (2) B has twice the

  6. Chemistry

    Calculate the average disappearance of A between t=0 min and t=10 min in units of M/s. 0 min there are .065 moles of A 10 min there are .051 moles of A 20 min there are .042 moles of A 30 min there are .036 moles of A 40 min there are .031 moles of A The

  7. chemistry 106

    Dry air near sea level has the following composition by volume: N2, 78.08 percent; O2, 20.94 percent; Ar, 0.93 percent; CO2, 0.05 percent. The atmospheric pressure is 1.00 atm. (Hint: Since volume is proportional to the number of moles present, mole

  8. Chemistry

    2NaOH+2Al+2H2O --> 2NaAlO2+3H2 here is the reaction. If i am trying to find the mass of hydrogen produced and i am trying to convert .95 moles Al to moles H, which number from the reaction do I use for H when converting from moles to moles? Do I 6 because

  9. Chemistry

    Calculate the number of moles of magnesium, chlorine, and oxygen atoms in 6.10 moles of magnesium perchlorate, Mg(ClO4)2.

  10. General Chemistry

    The formula of a compound of lead (Pb) and sulfur (S) was determined using the method in this module. A sample of Pb was weighed into a crucible and covered with finely powdered S. The crucible was covered and heated to allow the Pb and S to react.

  11. AP Chem need serious explanation

    Calculate the number of moles of carbon atoms present in 1.4 g of ethanol (C2H6O). i get that you calculate the number of moles of ethanol whic i got was .03039 but how do you get the moles of CARBON from that.

  12. Chemistry

    Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number

  13. CHEMISTRY

    for the reaction system H2 + X2 2HX Kc = 24.4 at 300 K a system made up fron these components which is at equilibrium contains 0.150 moles of H2 and 0.600 moles of HX in a 3.00 liter. calculate the number of moles of X2 present at equilibrium.

  14. chemistry

    A 0.286g sample of Zn was used to produce H2(g)by the reaction. Zn(s)+ 2HCl(aq)> ZnCl2(aq) + H2(g) The barometric pressure was recorded as 761.6mm Hg and room temperature was 20degreesC. When the water levels of the eudiometer tube and graduated cylinder

  15. Chemistry

    I am so confused with my chemistry lab right now. We were given the following equations to work with: [Equation 1] 2 I^- + H2O2 + 2 H^+ ----> I2 + 2 H2O [Equation 9] 2S2O3^2- + I2 ----> 2I^- +S4O6^2- And During the Experiment we used the following for each

  16. chemistry

    Can one calculate the number of moles of air? If so, calculate the number of moles in 1 kg of air (making sure your calculation, units and assumptions are fully explained); If not, explain why it is not possible to calculate the number of moles of air.

  17. Chemistry

    In a reaction chamber, 3.0mol of aluminum is mixed with 5.3mol Cl2 and reacts. The reaction is described by the following balanced chemical equation. 2Al + 3Cl2 ==> 2AlCl3 a)Identify the limiting reagent for the reaction. b)Calculate the number of moles or

  18. physics

    Find the number of moles in 2.00 L of gas at 35.0°C and under 7.41×107 N/m2 of pressure. Select one: a. 0.051 moles b. 51 ×105 moles c. 58 moles d. 5.8 moles

  19. Chemistry

    . Using I2 (aq)+ 2S2O3=> S4O6 (aq)+ 2I(aq) calculate the number of moles of molecular iodine. Given that there are 0.004328482 Moles of Na2S2O3. can someone please help i have no idea how to do this question for my lab!!! if possible please explain with

  20. chemistry

    When 1.24g of an organic compound with the formula CxHyOz is burned in excess oxygen, 1.76g of carbon dioxide and 1.08g of water vapor are obtained. What is the empirical formula of the compound? Determine the moles of CO2 in 1.76grams, that will give you

  21. Chemistry

    Calculate the number of moles of KIO3 consumed by reaction (2.1). Remember, it is the limiting reagent. Using this information, calculate the number of moles of I- that must have been consumed by reaction. Unbalanced equation: IO -(aq) + I-(aq) + H+(aq) ÿ

  22. Chemistry 111

    Calculate the number of moles of alumunium sulfer, oxygen atoms in 9.00 moles of Alumunium sulfate, Al2(SO4)3?

  23. chemistry

    H2 + I2 -> 2Hl 1.2 mol of hydrogen gas reacts with 1.0 mol of iodine vapour, after 5 minutes 0.6 mol of iodine remained. A) calculate the number of moles of hydrogen that have not reacted after 5 minutes. B) calculate the number of moles of hydrogen iodide

  24. Chemistry HELP ME!!!!

    A sloution of calcium nitrate, C(NO3), reacts with a solution of ammonium fluoride, NH4F, to form solid calcium fluoride, CaF2, and ammonium nitrate, NH4NO3(ag). When 45.00 mL of 4.8724 x 10 -1M Ca(NO3)2 solution was added to 60.00 mL of 9.9981 x 10 -1M

  25. Chemistry 111

    calculate the number of moles of magnesium, chlorine, and oxygen atoms in 8.80 moles of magnesium perchlorate?

  26. Chemistry

    This is for a titration, to measure the amount of acid that can be neutralised by gaviscon. I know how to work out the first 3 but I'm not sure on the others. I think i need to use the calculation c=n x v but i don't know where and why? Theory. How do you

  27. CHEM

    9.60 g of hydrated nickel (II) sulfate is heated to produce 5.26 g of anhydrous compound NiSO4. Calculate the number of moles of anhydrous nickel (II) sulfate. Calculate the number of moles of water lost. What is the empirical formula of the hydrate?

  28. Chemistry

    A 50.0 −mL sample of 1.50×10−2 M Na2SO4(aq) is added to 50.0 mL of 1.23×10−2 M Ca(NO3)2(aq). What percentage of the Ca2+ remains unprecipitated? Calculate the moles of Ca(NO3)2 you have (concentration * volume in L). Moles of Ca(NO3)2 = moles of

  29. Math

    1. Write the balanced chemical equation for the reaction NaOH + HCI --> NaCI + H20 2. Extract the relevant information from the qustion: NaOH v= 30mL, M=0.10 HCI v= 25.0 mL, M=? 3. Convert to Liters NaOH v= 0.03 L, M= 0.10M HCI v=0.025L, M=? 4. Calculate

  30. Chemistry

    1. How many molecules does 36.0 grams of water represent? Change the following masses to number of particles by: A) dividing by the molar mass to get the number of moles, and then B) multiplying number of moles by Avogadros number

  31. chemistry

    1. In the Thermodynamics of Borax Dissolution experiment, a student quickly transferred a 5.00 mL sample of the saturated borax solution into an Erlenmyer flasks using a pipet and pipet pump after the borax solution had cooled to 35oC. The student rinses

  32. CHEMISTRY

    When air pollution is high, ozone (O3) contents can reach 0.60 ppm (ie., .60 mol ozone per million mol air). How many molecules of ozone are present per liter of polluted air if the barometric pressure is 755 mm Hg and the temperature is 79 degrees F? I

  33. ap chem repost

    a 2L container is charged with 2atm of O2 at 298 Kelvin. Ch4(g) + 2O2(g) --> CO2(g) + 2H20(g) calculate the partial pressure of methane needed to react completely with the O2 in the vessel. What is the total pressure after the reaction is complete if the

  34. chem repost

    a 2L container is charged with 2atm of O2 at 298 Kelvin. Ch4(g) + 2O2(g) --> CO2(g) + 2H20(g) calculate the partial pressure of methane needed to react completely with the O2 in the vessel. What is the total pressure after the reaction is complete if the

  35. Chemistry

    UMM.. I keep coming up with the wrong answer? How do I calculate this? 1. Calculate the number of Li atoms in 9.9 moles of Li. Express your answer using two significant figures. 2. Calculate the number of CO2 molecules in 3.13×10−2 mole of CO2.

  36. sci/chemistry

    when 1.87 g of gypsum(hydrated calcium sulfate) was heated to constant mass, it lost 0.39 g of water. What is the formula of gypsum? YOu know it is of the form: CaSO4.XH2O the idea here is to find x. calculate the number of moles of water in .39g.

  37. re-apchem post

    a 2L container is charged with 2atm of O2 at 298 Kelvin. Ch4(g) + 2O2(g) --> CO2(g) + 2H20(g) calculate the partial pressure of methane needed to react completely with the O2 in the vessel. What is the total pressure after the reaction is complete if the

  38. AP Chem - to Dr. Bob

    I don't understand how to even start this problem: A mixture of H2(g), O2(g), and 2 mL of H2O is present in a 0.5 L rigid container at 25 degrees Celsius. The number of moles of H2 and the number of moles of O2 are equal. The total pressure is 1146 mmHg.

  39. chemistry 11

    Hi, I am stuck on a couple questions in chemistry 11. The questions are 1. Calculate the number of moles of the anhydrous salt left behind 2. Calculate the number of moles of water removed by heat from your sample of hydrate. 3. Calculate the moles of

  40. Chemistry

    I can not determine the answer for this problem...can someone please help me? Determine the number if moles of MgO that form from the reaction of 4.4 moles of O2 in the following unbalanced reaction: Mg + O2 ----> MgO The balanced equation is: 2Mg + O2

  41. College Chemistry

    The density of a 0.0122 M KMnO4 is 1.037 g/mL. Suppose 26.35 g of 0.0122 M KMnO4 are required to titrate 1.072 g of a household H2O2 solution. a)Calculate the mL of MnO4^- added to reach the endpoint. b)Calculate the moles of MnO4^- added to reach the

  42. Chemistry

    Consider the following equilibrium at 1000K: 2SO2 (g) + O2 (g) ¡ê 2SO3 (g) A study of this system reveals that there are 3.5E-3 moles of sulfur dioxide gas, and 4.8E-3 moles of oxygen gas present in a 11.0L flask at equilibrium. The equilibrium constant

  43. Chemistry

    Did I do these right? Can someone let me know if I did them correctly? I had someone help me with the problems but know I want to make sure their the right answers? 1. Methane burns in oxygen according to the following equation: CH4 + 2O2 ----> CO2 + 2H2O

  44. chemistry

    Calculate the number of grams of reactant left over when 28.35 grams of silver reacts with 50.0 liters of air at STP which is 20.9476 % oxygen by volume. The density of air at STP is 1.292 g/L. attemt at a solution: m = dv = 64.6 g of air moles silver

  45. Chemistry

    Mean titre of 0.2M sodium thiosulphate = 32.2 ml 1) Calculate number of moles of S2O32- which react in the titration 2)Calculate how many moles of I2 react with this amount of S2O3 3)How many Cu2+ ions are needed to liberate this amount of I2? Use this

  46. Chemistry

    A water chemist obtained a 250 ml sample from a nearby lake and fixed the oxygen on-site with alkaline solutions of MnSO4 and KI-NAN3. Returning to the laboratory, a 200 ml sample was analyzed by acidifying the sample with conc H2SO4 and then titrating

  47. Chemistry

    I don't really know how to go about this, Please help 1. Calculate the number of moles of the gas. Calculate the volume the gas would occupy at 100.0 C and 15.0 atm. 10.8 g He 2. Given the volume of 54.0 C and 790 torr, calculate the number of moles and

  48. science

    I need some help with my science homework. Well it is not really my homework it is my study guide but the actual test is the same as the study guide almost. They just switch around the words and stuff around to mess with your mind. These were just the only

  49. science

    I need some help with my science homework. Well it is not really my homework it is my study guide but the actual test is the same as the study guide almost. They just switch around the words and stuff around to mess with your mind. These were just the only

  50. Chemistry

    1.How Many Grams Of Sulphur Contains The Same Number Of Moles As 4.6g Of Sodium? 2.Calculate The Number Of Moles In 28.6g Of Na2CO3.10H2O?

  51. chemistry

    Calculate the number of grams in each of the following: A)0.5 moles of F2 B)10.25 moles of H2 C)11.3 moles of BaSO4

  52. chemistry

    1) 14 moles of Ar 12 moles of N2 2 moles of BF3 If the total number of mol present in the mixture visualized is 1.43, calculate the number of mol of N2. 2) 11 moles of N2 4 moles of CSH4 If the total number of mol present in the mixture visualized is 1.68,

  53. Chemistry

    Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single titration was performed which required 13.73 mL of 0.100 M Na2S2O3. The density of the original, undiluted bleach unknown was

  54. chemistry

    How many moles are in 13grams of C6H6. should this question be broken down into its imperical formula (CH)6 and calculate the number of moles of CH and multiply by 6 or calculate the gram molecular wt of C6H6 and divide it into 13 grams?

  55. Chemistry

    In this lab experiment you will make 100.0 mL of a 0.100 M solution of Co(NO3)2. However you must calculate the number of moles of compound that will be needed (moles= Molarity x Liters).Then calculate the mass of Co(NO3)2 that will need to be weighed out

  56. Chemistry

    Calculate the number of moles of Co^+2 are there in the equation Co(H2O)6^+2 +4Cl CoCl4^-2 +6H2O? I had found in the previous question the number of moles of CoCl2*6H2O and I'm not sure but I believe the moles of CoCl2*6H2O are the same as CO^+2.

  57. chem

    Assuming that you have 0.4g of Y(OH)3, calculate the mass of of BaO2 required to react stoichiometrically (1Y:2Ba:3Cu) to produce YBa2Cu3O7. Now calculate the mass of of CuO required to react stoichiometrically (1Y:2Ba:3Cu) to produce YBa2Cu3O7. please

  58. Chem

    When 5.49 g of platinum reacts with an excess of fluorine, 7.65 g of platinum(_) fluoride forms. a. What is the mass of fluorine in the compound? b. Find the number of moles of platinum that reacted. c. Find the number of moles of fluorine that reacted. d.

  59. chemistry

    in a empirical formula lab how do you calculate the number of moles of Cu in 0.0114 moles of CuSo4*H2O? Thanks

  60. Chemistry

    Using I2 (aq)+ 2S2O3=> S4O6 (aq)+ 2I(aq) calculate the number of moles of molecular iodine. Given that there are 0.004328482 Moles of Na2S2O3.

  61. Chemistry

    Calculate the number of moles of ag in 5ml of .004m agno3 and the number of moles of cr04 in 5ml of .0024m k2cro4

  62. chemestry

    Calculate the number of moles of NH3 that can be formed from the complete reaction of 0.30 moles of N2 according to the equation N2 + 3H2 → 2NH3

  63. chemistry

    QUESTION 9 The number of moles of the reagent in excess can be used to calculate the moles of the products of the reaction. TRUE FALSE

  64. chemestry

    Calculate the number of moles of NH3 that can be formed from the complete reaction of 0.30 moles of N2 according to the equation N2 + 3H2 → 2NH3

  65. chemistry/ molarity, molality

    A solution is made by mixing 20.0 mL of C6H5CH3, d=.867g/mL, with 140.0mL of C6H6, d=.874g/mL. assuming that the volumes add upon mixing, what is the molarity? what is the molality? i know that molarity= moles/L and molality= moles sol/kg solvent... but im

  66. chemistry

    A 1.213g sample of an unknown weak monoprotic acid was titrated to the endpoint with 27.25mL of a 0.3016M NaOH Calculate: -the number of moles of base reacted. -the number of moles of acid originally present. -the molar mass of the acid.

  67. chemistry

    using each of the following baldfaced chemical equations calculate the number of moles of the first listed reactant need ed to produce 5.00 moles of CO2 . C7H16+11O2-->7CO2 +8H2O

  68. Chemistry

    An aqueous solution contains 2.0 % NaCl by mass. (1) Calculate the molality (NOT molarity!) of the solution. (2) Calculate the mole fraction of the solution. I know how to solve both but the problem is missing one other compound/element. I know that

  69. chemistry

    2 questions, I'm Having trouble figuring out how to calculate the moles of a solute in a solution based on the molarity and the volume. Here is what I'm working with. 1) "Use molarity of the stock solution of aspirin/Fe(No3)3(aq) (0.0044mol) and the total

  70. Chemistry

    These are what i used. 0.0375M sodium thiosulphate , 2.5% KI .47.2 ml copper sulphate solution. the average volume of Na2S2O3 is 19.25 cm, i have already calculated the number of moles of thiosulphate which is 7.218 * 10-4 moles of Na2S2O3 and also the

  71. chemistry

    2NO+O2->2NO2 a) During a certain interval of time the variation of oxygen O2 moles is -5mol. Calculate the variation of the number of moles of nitrogen monoxide NO and that of nitrogen dioxide NO2 during the same interval of time. b) The duration during

  72. chem

    mass of mg- .28 mass of o- .41 calculate the moles of mg and o what is the simples whole number ratio of the moles of mg to the moles of o? round off to the nearest whole number ratio. use this mole ratio to write the empirical formula. the molecular mass

  73. chemistry

    hot-air balloon is filled with air at a volume of 3.64 x 10^3 m^3 at 745 torr at 39C. the air in balloon is heated to 60C, causing balloon to expand to a volume of 4.50x 10^3 m^3. what is the ratio of the number of moles of the air in heated balloon to

  74. physics

    If 8.00 moles of a monatomic ideal gas at a temperature of 260 are expanded isothermally from a volume of 1.08 to a volume of 4.14 .Calculate the work done by the gas.Calculate the heat flow into or out of the gas.If the number of moles is doubled, by what

  75. chemistry

    Using each of the following equations, calculate the number total of moles of products that can be obtained through decomposition of 1.75 moles of the reactant? a. 2 NH4NO3---> 2 N2 + O2 + 4 H2O b. 2 NaClO3---> 2 NACl + 3 O2 answers are 6.12 and 4.38 but i

  76. molarity

    calculate the molarity of k+ in a soln prepared by adding .2L of .200M K3PO4 and 75.0mL of .5M K3PO4. assume volumes are additive. A few of steps here and more than one way to answer the problem You need to calculate the total number of moles of K3PO4 from

  77. phisic

    Treating air as an ideal gas of diatomic molecules, calculate how much heat is required to raise the temperature of the air in an 7.47 m by 14.9 m by 2.87 m room from 19.9°C to 21.7°C at 101 kPa. Neglect the change in the number of moles of air in the

  78. Chemistry(Please help, thank you)

    I have to calculate the concentration of I2 produced (# of moles of I2 produced / L) based on the stoichiometric ratio in the following equation. 2S2O3^2- + I2 -> 2I^- + S4O6^2- Chemistry(Urgent, please help) - DrBob222, Sunday, February 26, 2012 at 9:47pm

  79. Chemistry

    I am a bit lost as to how to go about answering this question. Any help will be appreciated. When 1.40g of hydrated magnesium sulphate is heated to constant mass, 0.68g of the anhydrous salt remains. Find the formula for the hydrated magnesium sulphate.

  80. chemistry

    Initially, there are 33 moles of A and 0 moles of B. How many moles of A and B will be present after the system reaches equilibrium? a) 33 moles A; 0 moles B b) 0 moles A; 33 moles B c) 3 moles A; 30 moles B d) equal amounts of A and B The answer is given

  81. Please help with really hard chem question?

    An electrolysis experiment was run for 17.5 minutes at an average current of 191 milliamps (mA). The mass lost by the copper anode was 0.0679 grams. a) Calculate the number of coloumbs transferred. (coloumb=ampsxsec) b) Calculate the moles of copper lost

  82. chem

    Will someone help me with this problem, please? Calculate the mass in grams of 1.20*10^24 molecules of CO2. Well, convert it to moles of CO2. number moles= 1.2*1024/avagnumber Now, you take the molecular mass of CO2 (12 + 2*16) and multiply that by the

  83. Physics

    Calculate the ideal gas constant using the moles of air, temperature of air and slope of the air vs. 1/Pressure graph. Moles of air = 4.89*10^-4 Temperature of air = 23C Slope = 2317

  84. CHEMISTRY

    Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number

  85. Chemistry

    Calculate the number of moles of sodium oxide, Na2O, that should be produced when 11.50 moles of sodium, Na, react with oxygen gas

  86. Chemistry 120

    A sloution of calcium nitrate, C(NO3), reacts with a solution of ammonium fluoride, NH4F, to form solid calcium fluoride, CaF2, and ammonium nitrate, NH4NO3(ag). When 45.00 mL of 4.8724 x 10 -1M Ca(NO3)2 solution was added to 60.00 mL of 9.9981 x 10 -1M

  87. Chemistry II

    I will be happy to critique your thinking on this. First, calculate the moles of H2 used. 2.0e8 L H2/22.4 L H2 = 8.9e6 mol H2 For every 2 mol H2 used -572 kJ of energy is produced -572 kJ/2 mol H2 = -2.86e2 kJ/mol I have a balanced equation with this

  88. chemistry

    Am doing a lab report on the determination of the product of a redox reaction: the reaction of bromate and hydroxylammonium ions. here is the lab Experiment: In this experiment you will determine the equation of a redox reaction by the use of experimental

  89. Chemistry

    calculate the ph of a solution that results from titrating 0.0500 moles of cyanic acid to the equivalence point with an equal number of moles of OH-, if the final volume of the solution is 150 ml ka= 3.50 * 10^-4

  90. Chemistry

    Calculate the number of moles of solute in each of the following solutions: Solution Moles of Solute 2.1 L of 0.21 M NH4HCO3 3.5 L of 0.28 M MgCO3

  91. chemistry

    How many moles are in 13grams of C6H6. should this question be broken down into its imperical formula (CH)6 and calculate the number of moles of CH and multiply by 6 or calculate the gram molecular wt of C6H6 and divide it into 13 grams? I took 13 grams

  92. chemistry

    Calculate the number of moles of Na2CO3 present in 100cm^3 of 2 M Na2CO3 solution.i got 5 moles.am i right

  93. Chem

    Calculate the number of moles and number of grams of solute in 250 mL of a 0.10M CaCl2.

  94. chemistry - DrBob222

    For this question can u please explain steps 3 and 4 4.0 g of ferrous ammonium sulphate, FeS04(NH4)2 SO4 6H20, is used. The oxalate is in excess, calculate the theoretical yield of the iron complex. Can someone please show me how to calculate a question

  95. chemistry stoichiometry

    My chem teacher gave us this problem Twelve-gauge copper wire,like the kind commonly used in residential electrical systems, is roughly cylindrical and has a diameter of approximately .1040in. Copper's density is 8.92g/cubic cm and copper atoms have an

  96. Chem

    Calculate the value of Qc for the reaction above if 2.30 moles of NO2, 1.50 moles of NO, and 1.20 moles of O2 are placed in a 3.50 liter container at 30°C. Kc = 0.440 at this temperature.

  97. Chemistry

    Calculations involving a limiting reactant Now consider a situation in which 20.0 g of P4 is added to 54.0 g of Cl2, and a chemical reaction occurs. To identify the limiting reactant, you will need to perform two separate calculations: 1) Calculate the

  98. chemistry

    Calculate the number of moles volume number of molecules of carbon dioxide liberated when 200 grams of limestone decomposed .

  99. chemistry

    Calculate the number of moles volume number of molecules of carbon dioxide liberated when 200 grams of limestone decomposed .

  100. Chemistry

    Calculate the pH of a 1 L buffer solution that contains 0.050 moles of acetic acid and 0.040 moles of sodium acetate to which 0.020 moles of NaOH has been added.

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