When 125 mL of a magnesium nitrate solution is mixed with 175 mL of a 1.50 mol L
Calculate the equilibrium concentration of magnesium ions in this solution. (5 marks)
--- 12 WORK AREA LINES (style=lined) ---
Aussie Maths & Science Teachers: Save your time with SmarterEd
When 125 mL of a magnesium nitrate solution is mixed with 175 mL of a 1.50 mol L
Calculate the equilibrium concentration of magnesium ions in this solution. (5 marks)
--- 12 WORK AREA LINES (style=lined) ---
When a sample of solid silver chloride is added to a
Calculate the equilibrium concentration of silver ions in the resulting solution, given that the
--- 6 WORK AREA LINES (style=lined) ---
Stormwater from a mine site has been found to be contaminated with copper
--- 5 WORK AREA LINES (style=lined) ---
--- 6 WORK AREA LINES (style=lined) ---
--- 7 WORK AREA LINES (style=lined) ---
a. Recommended Treatment:
→ Calcium hydroxide is a slightly soluble compound, while copper
→ When these compounds are added to water, the metal ions tend to precipitate out of solution.
→ For example, the addition of solid calcium hydroxide to water produces calcium ions
→ These reactions are represented by the equations:
b. Atomic absorption spectroscopy (AAS):
→ Can be used for determining the concentration of metal ions in a sample by measuring the absorbance of light at specific wavelengths that are characteristic of each metal.
→ AAS uses light wavelengths that correspond to atomic absorption by the element of interest, and since each element has unique wavelengths that are absorbed, the concentration of that element can be selectively measured in the presence of other species.
→ As a result, AAS can be used to independently measure the concentrations of different metal ions, such as lead
c. Concentrations of ions:
→ Concentrations of copper and lead have been significantly reduced.
→ Convert concentrations to compare with standard:
Conclusion:
→ The concentration of copper ions has been reduced to a level that is lower than the discharge limit (0.16 < 1.0) but the lead ion concentration has not (1.76 > 1.0).
→ The treatment has only been partially successful.
a. Recommended Treatment:
→ Calcium hydroxide is a slightly soluble compound, while copper
→ When these compounds are added to water, the metal ions tend to precipitate out of solution.
→ For example, the addition of solid calcium hydroxide to water produces calcium ions
→ These reactions are represented by the equations:
b. Atomic absorption spectroscopy (AAS):
→ Can be used for determining the concentration of metal ions in a sample by measuring the absorbance of light at specific wavelengths that are characteristic of each metal.
→ AAS uses light wavelengths that correspond to atomic absorption by the element of interest, and since each element has unique wavelengths that are absorbed, the concentration of that element can be selectively measured in the presence of other species.
→ As a result, AAS can be used to independently measure the concentrations of different metal ions, such as lead
c. Concentrations of ions:
→ Concentrations of copper and lead have been significantly reduced.
→ Convert concentrations to compare with standard:
Conclusion:
→ The concentration of copper ions has been reduced to a level that is lower than the discharge limit (0.16 < 1.0) but the lead ion concentration has not (1.76 > 1.0).
→ The treatment has only been partially successful.
Consider the following equilibrium.
Which row of the table correctly identifies the strongest acid and the strongest base in this system?
A. | ||
B. | ||
C. | ||
D. |
→ The small size of
→ This shifts the equilibrium towards the reactants, which means that the reverse reaction is more likely to occur.
→ Because
→ On the other hand,
In aqueous solution, iodide ions
The following relationships can be derived from the reaction mechanism:
where 'initial' designates the initial concentration and 'eq' designates the equilibrium concentration.
The absorbance of the solution in the UV-Vis spectrum is given by:
Determine the value of the equilibrium constant, given that
The following apparatus was set up in a temperature-controlled laboratory.
Excess solid sodium hydroxide is added to the beaker.
Which row of the table correctly identifies the change in the
→ The addition of
→ According to Le Chatlelier’s Principle, the system would shift right in an attempt to counteract the change and increase
→ The blue colour will fade since the
A precipitate of strontium hydroxide
What is the
--- 10 WORK AREA LINES (style=lined) ---
Equal volumes of two 0.04 mol L ¯1 solutions were mixed together.
Which pair of solutions would give the greatest mass of precipitate?
→ Reaction B produces 2 molecules of precipitate
→ Reactions A and D produce 1 molecule of precipitate each
→ Reaction C does not produce a precipitate.