CHEM 212 Lecture Notes - Equivalence Point, Sodium Hydroxide, Titration

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graymole855

19 Jan 2013

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Problem: write the net ionic equation for the reaction that occurs when aqueous solutions of magnesium sulphate (mgso4) and sodium oxalate (na2c2o4) are mixed. Acids are identified by their sour tastes, their ability to react with a variety of metals and carbonate minerals. From a chemist"s standpoint, an acid can be defined as a substance that provides hydrogen ions (h+) in aqueous solutions. A strong acid completely ionizes in a water solution: Hcl (aq) (h20) h+ (aq) + cl- (aq) (aq). A weak acid, on the other hand, does not go towards completion and is also a weak electrolyte. A example is acetic acid: hc2h3o2 (aq) h+ (aq) + c2h3o2. Hcl h+ + cl- : strong electrolyte, strong acid. Ch3cooh h+ + ch3coo- : weak electrolyte, weak acid. H2so4 h+ + hso4- : strong electrolyte, strong acid. From a practical standpoint, a base is bitter in taste and slippery.

Related Questions

Fill the questions according to Data Table 7-2

5. balanced formula equation: for each combination of solutions that produced new product. write correct chemical formulas for the new compounds that could form from the ions present. Indicate which of the new compunds is a precipitate. If no reaction occurs, write NR.

6. complete ionic equation: write complete ionic equations for the precipitation reactions that you observed. show the reactants as ions, the precipitate as a solid, and the spectator ions as unchanged. balance each equation for mass and change. the total charge should be zero on each side of the equation.

7. net ionic equation: write the net ionic equations for each reaction in the preceding question.

1. Balance each equation:

a) H2 +I2 = HI b) Al+O2 = Al2O3 d) Al+HBr = Albr3+H2

2. Calcium oxide is prepared by heating limestone (calcium carbonate, CaCO3) to a high temperature, at point it decomposes to calcium oxide and carbon dioxide. Write a balanced equation for this preparation of calcium oxide.

3.When a piece of aluminum metal is dropped into hydrochloric acid, HCI, hydrocloric acid, HCI, hydrogen is released as a gas and a solution of aluminum chloride forms. Write a balanced equation for the reaction.

4. In the equation: 2Na^+(aq)+CO3^2-(aq)+Sr^2+(aq)+2CI^-(aq)+SrCO3(s)+2Na^+(aq)+2CI^-(aq)

a) Identify the spectator ions b) Write the balaanced net ionic equation

5. When a solution of sodium hyroxide is added to a solution of ammonium carbonate, H2O is formed and ammonia gas, NH3, is released whe the solution is heated. Write a net ionic equation for this reaction. Both NaOH and (NH4)2CO3 exist as dissociated ions in aqueous solution.

6. Using the solubility generalizations given in Section 4-3 predict which of these ionic compounds are soluble in water.

a)MgCl2 b)CaCO3 c)Na2SO3 d)NH4NO3 e)Pb(OH)2

7. When a piece of sodium metal is added to water, hydrogen is evolvedas a gas . and a solution of sodium hydroxide is formed.

a) Write a balanced equation for this reaction.

b) What is oxidized in this reaction? What is reduced?

8. Calculate the formula weight of:

a)Na3PO4 b)Al2(SO4)3

9. Calculate the number of moles in:

a) 32g of methane,CH4 b)184.4g of chlorine dioxide ClO2

10. Calculate the number of grams in:

a) 1.77 mol of nitrogen dioxide, NO2 b) 3.69 mol of uranium hexaflouride, UF6

Could you please answer these questions