burns in air to give water and sulphurdioxide. (3) Potassium metal reacts with water to give potassium hydroxide and hydrogen gas. (3) 12. Balance the equations (1) HNO3 + Ca (OH ) 2 → Ca ( NO3 ) 2 + H 2O (2) NaCl + AgNO3 → AgCl + NaNO3 (3) BaCl2 + H 2 SO4 →
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of analyte in a solution through analytical chemistry. This method uses the mass of solid SO42-‚ with an unknown quantity and quality‚ to qualitatively determine the makeup of the solid SO3-. Two separate experiments with the initial compounds of BaCl2 and SO42- were put into solution to allow for the BaSO4 precipitate to form. Through filtration and ignition of precipitate containing ashless papers‚ the solid masses of BaSO4 were attained. With a gravimetric factor of 1:1‚ sample 1 resulted in
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596) = ___ _77.12____ d) 345.67/9.01 = _____38.4_____ Page 2 5. Write the names of the chemicals shown by their formulas/or the formulas from the given names. a) BaCl2 ____barium chloride_____ b) KMnO4 __potasium permanganate c) H2SO4 ____sulphuric acid______ d) H2O ______hydrogen oxide____ e) AgNO3 ____silver nitrate______ f) Sodium bicarbonate ______Na2CO3____
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Chlorine Zachary Grindle Chemistry 1301 Professor Bott June 24‚ 2010 Chlorine has an atomic mass of 35.453‚ atomic number 17‚ is a member of the halogen family (VIIA)‚ and its symbol is “Cl”. Chlorine contains 17 protons and 18 neutrons in is nucleus. There are two isotopes for chlorine as well; Cl-35 and Cl-37. Chlorine was discovered in 1774 by Swedish chemist Carl Wilhelm Sheele. Sheele came upon chlorine when he put a few drops of hydrochloric acid (HCl)‚ then known as muriatic acid
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3. Test Solution Chemical Formula Sodium Sulphate Na2SO4 Potassium Chloride KCl Iron (lll) Nitrate Fe(NO3)3 Bottle Water H20 Tap Water H20 Well Water H20 Reagent Chemical Formula Silver Nitrate AgNO3 Barium Chloride BaCl2 Potassium Thiocyanate
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Name:_________________________ MASS AND MOLE RELATIONSHIPS IN A CHEMICAL REACTION PRE-LAB QUESTIONS 1. Balance the equation for the reaction of barium chloride with silver nitrate. 2. Predict the mole ratio of BaCl2 to AgCl for the equation. 3. If an experiment with 10.2 g barium chloride produced 14.5 g silver chloride‚ calculate the experimental mole ratio of silver chloride to barium chloride. Name:_______________________
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Reaction #4A: NaOH(aq) + HCl(aq)(0.5m) H2O(l) + NaCl(aq) Observations: A clear gas was formed. Reaction #5A: NaOH(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(OH)(s) Observations: The solution turned slightly cloudy. Reaction #6A: Na2SO4(aq) + BaCl2(aq) Na2Cl2(l) + BaSO4(s) Observations: The solution turned white and cloudy. Reaction #7A: Na2SO4(aq) + Cu(NO3)2(aq) CuSO4(aq) + 2NaNO3(aq) Observations: The solution was slightly tinted blue due to the copper‚ but it
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Testing for Cation and Anions OBJECTIVE: • Determine the presence of a cation or anion by a chemical reaction • Determine the cation and anion in an unknown solution All salt solutions have both positive (Cations) and negative (Anions) ions dissolved in it. In this experiment you will observe chemical reactions to determine the presence of specific anions and cations. Compare your observations with the reactions of the known solutions and the unknown solution to determine the ions present
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CSEC CHEMISTRY NOTES ON PERIODIC TRENDS From Chemistry for CSEC by Tania Chung-Harris and Mike Taylor Chemistry for CAPE by Susan Maraj and Arnold Samai Periodic Trends in Group II Elements in Group II The elements in Group II are called alkaline earth metals. Be‚ Mg‚ Ca‚ Sr‚ Ba‚ Ra Beryllium‚ Magnesium‚ Calcium‚ Strontium‚ Barium‚ Radium These elements bond by metallic bonds (intramolecular forces) to form giant metallic structures. The size of the
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110 for 1 hour and cooled in a desiccator. Individual samples were weighed into each of three 250 mL Erlenmeyer flasks and dissolved in about 100 mL of distilled water. Small quantities of NaHCO3 was added until effervescence ceased. About 2 mL of K2CrO4 was introduced and the solution was titrated to the first
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