Write the net ionic reaction that occurs upon the addition of HNO3 to a solution which contains methylamine (CH3NH₂) and methylammonium chloride (CH3NH3CI). (Be sure to include states of matter.)
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- (8) Answer each of the following questions: (a) Ka for HNO2 is 4.6 x 10-4. What is the Kb for its conjugate base ? (b) Calculate the pH of 0.1 M of HNO2 solution using the ka above.Consider the reaction between H3PO4 and NH3 to produce (NH4)2HPO4. (a) What mass of ammonia would have to be added to 31.5 g of phosphoric acid if a 25% excess of ammonia is required? g(b) What is the theoretical yield of (NH4)2HPO4 under the conditions given in Part (a)?Which of the following statements about the reaction H2(g)+O2(g)→H2O(l)H2(g)+O2(g)→H2O(l) is true? (i) This is an example of an acid–base reaction. (ii) O2O2 is oxidized in this reaction. (iii) H2H2 is reduced in this reaction. Which of the following statements about the reaction is true? (i) This is an example of an acid–base reaction. (ii) is oxidized in this reaction. (iii) is reduced in this reaction. iii only i only ii and iii ii only None of them are true.
- Consider the series of reactions to synthesize the alum (KAl(SO4 )2 · xH2O(s)) from the introduction. (a) Assuming an excess of the other reagents, from one mole of aluminum Al (s), how many moles of alum will be produced? (b) Assuming an excess of the other reagents, from one mole of potassium hydroxide KOH, how many moles of alum will be produced? (c) Assuming an excess of the other reagents, from one mole of sulfuric acid H2SO4 , how many moles of alum will be produced? (d) If you start the synthesis with 1.00 g of Al, 40.0 mL of 1.50 M KOH, and 20.0 mL of 9.00 M H2SO4 , which of the three will be the limiting reagent? (e) Assuming that the product is anhydrous (that there are no waters of hydration), calculate the theoretical yield of alum, in grams, based on the amounts of reagents in part (d). 3. Consider the nickel salt: (NH4 )2Ni(SO4 )2 ·y H2O (Ammonium Nickel Sulfate Hydrate), where y is the number of coordinated waters. (a) Assuming that the product is anhydrous (y = 0),…State what would happen when (CH3)3P is added to the Lewis acid-Lewis base adduct (CH3)2O·BH3 in a (CH3)2O solution.Do you expect the following reaction to occur? Why?
- Write a balanced equation for the acid–base reaction thatleads to the production of each of the following salts.Name the acid, base, and salt.(a) CaF2 (c) Zn(NO3)2(b) Rb2SO4 (d) KCH3COO3. Write balanced formula equations for each of the following reactions. Physicai states of reactants and products need not be shown. (i) The combustion of ethane gas, C2H6, in excess air to form carbon dioxide and water. (ii) oxide andcarbon dioxide. The decomposition of solid całcium carbonate by heat to form calcium (iii) The decomposition of hydrogen peroxide to form water and oxygen(iv) The reaction of iron with chlorine to form iron(III) chloride.Structure and Bonding Cyanamide, NH2CN, has a melting point of 45 °C. (a) Draw a dot-and-cross diagram to illustrate the electron arrangement in NH2CN. (b) Name the predominant intermolecular interaction that could account for the melting point of cyanamide, and illustrate your answer with a diagram. (a) The melting point of NaCl was found to be 801 °C. Suggest, with reasons, whether the melting point of MgO will be higher or lower than that of NaCl. 3 (Refer to Section 1.2.2, pg 4 of Topic 3 Lecture Notes to revise how to compare ionic bond strength) (b) The boiling points of ammonia, carbon monoxide and carbon dioxide are given in the table below: gas formula Mr b.p. /°C ammonia NH3 17 -33 carbon monoxide CO 28 -192 carbon dioxide CO2 44 -78 With reference to their structure and bonding, account for their boiling points. (Refer to Section 5, pg 22 of Topic 3 Lecture Notes to revise how to identify the type of IMF)
- a) Compare between equivalence point and endpoint. Distinguish which point comes first. b) Sulfanilamide, C6H4N2O2S is a sulfonamide antibacterial drug. The purity of sulfanilamide (168.18 g/mol) can be determined by the following steps. First, oxidize sulfur to SO₂ gas. Next, allow SO₂ gas generated to pass through H₂O₂ to produce H₂SO4. The acid is then titrated with NaOH standard solution. Given a 0.5136 g of sulfanilamide sample required an average titre volume of 48.13 mL 0.1251 M NaOH. Suggest a suitable indicator to be used in this titration and predict the purity of sulfanilamide being analysed. (Note: 1 mol sulfanilamide = 1 mol H₂SO4)1: Write all the chemical reactions involved in the formation of acid rain from sulfur dioxide (SO2) and rain (H2O).Give the balanced chemical equation when reacting C5H12O with H3O+Cl-