Preparation of magnesium hydroxide
Magnesium hydroxide in a white insoluble solid that is used as an antacid to relieve upset stomach. Obtain as solid
A).Method
B).Balanced equation
C).Net ionic equation
D)Observation
A) Method:
1. In a beaker, dissolve 5 grams of magnesium chloride hexahydrate (MgCl2•6H2O) in 50 mL of distilled water.
2. In another beaker, dissolve 5 grams of sodium hydroxide (NaOH) in 50 mL of distilled water.
3. Slowly pour the sodium hydroxide solution into the magnesium chloride solution while stirring continuously.
4. The solution should turn cloudy as the magnesium hydroxide precipitates out of solution.
5. Allow the mixture to settle for about 15 minutes.
6. Using a filter paper, filter the mixture to obtain the solid magnesium hydroxide.
7. Wash the solid with distilled water and allow it to dry completely at room temperature.
B) Balanced equation:
MgCl2 + 2NaOH → Mg(OH)2 + 2NaCl
C) Net ionic equation:
Mg2+ + 2OH- → Mg(OH)2
D) Observation:
The mixture turns cloudy as the magnesium hydroxide precipitates out of solution. The solid magnesium hydroxide obtained by filtration is white.
When Mg(NO3)2 reacts with NaOH and forms Mg(OH)2
A) write balanced equation
B).Net ionic equation
A) Balanced equation:
Mg(NO3)2 + 2NaOH → Mg(OH)2 + 2NaNO3
B) Net ionic equation:
Mg2+ + 2OH- → Mg(OH)2
When CaCl2 reacts with Na2CO3 and forms CaCO3
A).Write the balanced equation and net ionic equation
A) Balanced equation:
CaCl2 + Na2CO3 → CaCO3 + 2NaCl
B) Net ionic equation:
Ca2+ + CO32- → CaCO3
Formula for barium sulphate
BaSO4
Preparation of calcium sulphate
Calcium sulphate is slightly soluble solid that is used to make plaster.Prepare the solid.Mix solution well-the reaction may be slow to occur
A).method
B).Balanced equation
C).Net ionic equation
D).Observation
A) Method:
1. In a beaker, dissolve 5 grams of calcium carbonate (CaCO3) in 100 mL of dilute sulfuric acid (H2SO4) solution (1M).
2. Heat the mixture gently, stirring continuously to allow the reaction to occur. The reaction will produce calcium sulfate (CaSO4) and carbon dioxide (CO2) gas.
3. Allow the mixture to cool completely and the calcium sulfate to settle to the bottom of the beaker.
4. Using a filter paper, filter the mixture to separate the solid calcium sulfate from the liquid.
5. Wash the solid with distilled water and allow it to dry completely at room temperature.
B) Balanced equation:
CaCO3 + H2SO4 → CaSO4 + CO2 + H2O
C) Net ionic equation:
CaCO3 + H+ → Ca2+ + CO2 + H2O
Ca2+ + SO42- → CaSO4
D) Observation:
The mixture produces effervescence (bubbling) due to the release of carbon dioxide gas. Over time, the solid calcium sulfate settles to the bottom of the beaker. The solid obtained by filtration is white and slightly soluble.
What properties of calcium sulphate make it suitable for the use in plaster.
Calcium sulfate has several properties that make it suitable for use in plaster:
1. Setting: Calcium sulfate has a unique property of setting or hardening when mixed with water. This property allows it to be used as a binder or adhesive in construction materials, such as plaster.
2. Fire resistance: Calcium sulfate is fire-resistant, which makes it an excellent material for use in building materials, such as wallboard and plasterboard. The presence of water in the calcium sulfate hemihydrate (plaster of Paris) provides a fire-resistant barrier that s the passage of heat.
3. Low solubility: Calcium sulfate has a low solubility in water, which makes it an ideal material for use in plaster. Plaster is a mixture of calcium sulfate hemihydrate and water, which turns into a hard, solid mass upon setting. The low solubility of calcium sulfate ensures that the plaster does not dissolve or lose its strength over time.
4. Durability: Calcium sulfate is durable and resistant to wear and tear. This property ensures that plaster made from calcium sulfate can withstand the rigors of use in construction and maintain its strength over time.
Overall, the unique combination of setting, fire resistance, low solubility, and durability make calcium sulfate an ideal material for use in plaster and other construction materials.
CaCl2 reacts with H2SO4 and forms CaSO4
Write the balanced equation and Net ionic equation
Balanced equation:
CaCl2 + H2SO4 → CaSO4 + 2HCl
Net ionic equation:
Ca2+ + SO42- → CaSO4
Preparation of barium sulphate
Barium sulphate is an insoluble solid used as a paint pigment and in the "barium meal" taken for certain types of X-ray photography.Prepare the solid
A).Method
B).Balanced equation
C).Net ionic equation
D). Observation
A) Method:
1. In a beaker, dissolve 5 grams of barium chloride dihydrate (BaCl2•2H2O) in 50 mL of distilled water.
2. In another beaker, dissolve 5 grams of sodium sulfate (Na2SO4) in 50 mL of distilled water.
3. Slowly pour the sodium sulfate solution into the barium chloride solution while stirring continuously.
4. The solution should turn cloudy as the barium sulfate precipitates out of solution.
5. Allow the mixture to settle for about 15 minutes.
6. Using a filter paper, filter the mixture to obtain the solid barium sulfate.
7. Wash the solid with distilled water and allow it to dry completely at room temperature.
B) Balanced equation:
BaCl2 + Na2SO4 → BaSO4 + 2NaCl
C) Net ionic equation:
Ba2+ + SO42- → BaSO4
D) Observation:
The mixture turns cloudy as the barium sulfate precipitates out of solution. The solid barium sulfate obtained by filtration is white, insoluble and has a fine powder-like texture. It does not dissolve in water or organic solvents.
Magnesium sulphate (Epsour salt) is soluble solid that is used as an mild laxative in causing movement of bowels in human.Prepare a solution of magnesium sulphate. Obtain it as a solid
a). Method
b).Balanced equation
c).Net ionic equation
b).Observation
a) Method:
1. In a beaker, dissolve 5 grams of magnesium sulfate heptahydrate (MgSO4·7H2O) in 100 mL of distilled water.
2. Stir the mixture until the solid completely dissolves in the water.
3. Filter the solution through a filter paper to remove any impurities.
4. If you want to obtain MgSO4 as a solid, evaporate the water from the solution using a hot plate or any other heat source. Magnesium sulphate will be obtained as white crystals.
b) Balanced equation:
MgSO4 + 7H2O → MgSO4·7H2O
c) Net ionic equation:
Mg2+ + SO42- → MgSO4
d) Observation:
The magnesium sulfate dissolves easily in water to form a clear solution. On evaporation of the water, white crystals of magnesium sulfate are formed. These crystals are odorless and have a bitter taste. The crystals are soluble in water and slightly soluble in ethanol. When ingested, magnesium sulfate acts as an osmotic laxative, drawing water into the intestine and promoting bowel movement.
Mg reacts with Mg(NO3)2 and forms MgSO4
Balanced equation
Net ionic equation
Balanced equation:
3Mg + 2Mg(NO3)2 → MgSO4 + 4MgO + 2NO2
Net ionic equation:
3Mg + 2NO3- → MgSO4 + 2NO2