Complete each of the following reactions by determining the products and balanci

Question

Complete each of the following reactions by determining the products and balancing the equations

a) Ag+(aq)+Cl-(aq) -->

b) Na2SO4(aq)+BaCl2 -->

3. Determine the chemical equation for the reaction between Fe3+ and Cu2+ with NH3

4. Using the pH scale of 1-14, describe an acidic solution and a basic solution. At what pH would a solution be considered neutral? Why?

5. Write the balanced reaction between calcium carbonate and water to produce carbon dioxide.

6. Look up the solubility data for barium sulfate and magnesium sulfate. How does this data explain why barium sulfate is seen as a precipitate in the reaction in this lab?

7. Write a balanced reaction for a double displacement reaction not performed in this experiment.

Explanation / Answer

1. Balancing reactions:

a) Ag+(aq)+Cl-(aq) --> AgCl (s)

b) Na2SO4(aq)+BaCl2 --> BaSO4(s) + 2NaCl

3. Chemical equation for the reaction between Fe3+ and Cu2+ with NH3

Fe3+ + 6NH3 -------> [Fe(NH3)6]3+

Cu2+ + 4NH3 -------> [Cu(NH3)4]2+

4. Higher the pH higher is the basicity and lower is the acidity and vice versa. This is because

pH = -log [H+]. But, for acids the higher the H+ concentration lower is the pH, reverse the case for the bases. A typical pH scale is as follows.

An acidic solution has pH range from: 1<pH<7

Basic solution has pH ranges from: 7<pH<14

Neutral solution has pH=7. Because for a neutral solution the [H+]= [OH-].

5. CaCO3(s) + H2O(l) ----> CO2(g) + Ca(OH)2

6. A precipitate is a compound which is less soluble or insolube in water of in any solvent medium, hence it precipitates out in the reaction. As the solubility of BaSO4 in water is very less 0.0002448 g/100 mL (20

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