August 28‚ 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Chapter 16 Acid-Base Equilibria and Solubility Equilibria Student: ___________________________________________________________________________ NOTE: A table of ionization constants and Ka’s is required to work some of the problems in this chapter. 1. In which one of the following solutions will acetic acid have the greatest percent ionization? A. B. C. D. 2. Which one of the following is a buffer solution? A. B. C. D. E. 3. 0.40 M HCN and
Free PH Buffer solution Sodium hydroxide
ICSE Class X Chapter 5 Hydrogen Chloride and Hydrochloric Acid Hydrogen chloride (HCl) : Formula : HCl Nature : Covalent. Molecular Mass : 36·5u [i.e. HCl = 1 + 35·5 = 36·5] Occurrence : (i) Present in gastric juices. (ii) Present in volcanic gases. Laboratory preparation of HCl gas : Hydrogen chloride gas is prepared in laboratory by heating conc. H2SO4 with NaCl. NaCl + H2SO4 Heat → NaCl + NaHSO4 Heat → NaHSO4 + HCl Sodium hydrogen sulphate Na2SO4 + HCl
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Flame Tests The flame testing is a method used in chemistry to detect the presence of certain ions‚ primarily metal ions‚ based on each element’s characteristics emission spectrum. The colour of the flames normally depends on the temperature. Different types of Bunsen burner with flame types depend on the oxygen supply. The flame of rich fuel with no premixed oxygen produces a yellow diffusion flame. The flame of lean fully oxygen premixed flame produces no soot and the flame colour is produced
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SEMI – MICRO QUALITATIVE ANALYSIS OF SIMPLE INORGANIC SALT _______________________________________________________________ CATIONS: Pb2+ ‚Hg2+ ‚Cu2+ ‚Cd2+ ‚ Ag+ ‚ Fe2+ ‚ Fe3+ ‚ Al3+ ‚ Zn2+ ‚ Mn2+ ‚ Co2+ ‚ Sr2+ ‚ Ba2+ ‚ Mg2+ ‚ NH4+ ANIONS: CO32- ‚ S2- ‚ SO32- ‚ SO42- ‚ NO2- ‚ NO3- ‚ Cl- ‚ Br2- ‚ PO43- ‚ CH3COO- _______________________________________________________________ PRELIMINARY TESTS 1. Note the state (amorphous or crystalline) and colour of salt. 2. Test the solubility of the salt in
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We then observe if there are any evidence of reaction which would be bubbling or appearance of metallic deposits on the surface of the metal stip. TABLE 1: Chemical Reaction SOLUTION and METAL EVIDENCE of REACTION PRODUCT 1. AgNO3 + Cu deposits of Ag —> Ag + Cu(NO3)2 2. Cu(NO3)2 + Pb deposits of Cu —> Cu + Pb(NO3)2 3. Pb(NO3)2 + Zn deposits of Pb —> Pb + ZnNO3 4. MgSO4 + Zn no reaction —> no reaction 5. HCl2SO4 + Cu no reaction —> no reaction 6. HCl2SO4 + Zn deposits of H —>
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Version 017 – Exam 1 – Laude – (52455) This print-out should have 30 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. 001 1 003 6.0 points What would be pH of a 1 M solution of a very expensive weak base‚ unobtainamine‚ whose pKb is 3.4? 6.0 points 1. 12.3 correct Consider a reaction with ∆Hrxn = 997 kJ · mol−1 . Which of the following pairs of K values and temperatures is possible for this reaction? 1. K1 =
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supernatant III and pour half of the solution into a second clean test tube. To one test tube add drops of 1M Na2CO3 solution and watch for formation of a white CaCO3 precipitate. (Ca2+ would also be confirmed by; to the second test tube add drops of 1M K2CrO4 solution and watch for formation of a canary yellow CaCrO4 precipitate.) The other test tube of solution can be used for a flame test – reddish flash confirms Ca2+. Use the Outline below when collecting your data and writing your lab
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HOW ARE REDOX REACTIONS DIFFERENT? Redox is the term used to label reactions in which the acceptance of an electron (reduction) by a material is matched with the donation of an electron (oxidation). A large number of the reactions already mentioned in the Reactions chapter are redox reactions. Synthesis reactions are also redox reactions if there is an exchange of electrons to make an ionic bond. If chlorine gas is added to sodium metal to make sodium chloride‚ the sodium has donated an electron
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During the tests for the anions present in the unknown solutions we learned a lot about our solutions. For the first test‚ chloride anion‚ we received positive results from A and C. This is because they had chloride anions present and when mixed with AgNO3 and HNO3 the chloride ion solutions are used because silver nitrate is insoluble in HNO3. During the acetate anion test we had a positive result for solution D that proved the presence of the acetate ion. This reaction was from one drop of concentrated
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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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