150 mL of a 0.20 mol L
Calculate the pH of the resulting solution, assuming that the volume of the resulting solution is 250 mL and that its temperature is 25°C. (4 marks)
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150 mL of a 0.20 mol L
Calculate the pH of the resulting solution, assuming that the volume of the resulting solution is 250 mL and that its temperature is 25°C. (4 marks)
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20 mL 0.08 mol L
What is the pH of the resultant solution?
The pH of two solutions,
Explain the pH changes that occurred in solutions
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→ The diagram shows that the pH of solution
→ When
→ In contrast, the
→ The diagram shows that the pH of solution
→ When
→ In contrast, the
A solution was made by mixing 75.00 mL of 0.120 mol L
What is the pH of the solution? (3 marks)
Propanoic acid dissociation in water can is represented in the following equation:
Explain how the pH of the propanoic acid solution would change if it was diluted. (3 marks)
→ Propanoic acid only partially ionises in solution and is defined as a weak acid.
→ Any dilution of the acid will result in a decrease of the concentration of all species (including the hydronium ion).
→ According to Le Chatelier, the decreasing concentrations of dissolved species will cause the equilibrium to shift to the right.
→ While this effect causes an increase in ionisation, it is not sufficient to counter the decrease in hydronium ion concentration caused by the original dilution.
→ Since the net effect causes the hydronium ion concentration to decrease, the solution will become less acidic and the pH will increase.
→ Propanoic acid only partially ionises in solution and is defined as a weak acid.
→ Any dilution of the acid will result in a decrease of the concentration of all species (including the hydronium ion).
→ According to Le Chatelier, the decreasing concentrations of dissolved species will cause the equilibrium to shift to the right.
→ While this effect causes an increase in ionisation, it is not sufficient to counter the decrease in hydronium ion concentration caused by the original dilution.
→ Since the net effect causes the hydronium ion concentration to decrease, the solution will become less acidic and the pH will increase.
The graph shows changes in pH for the titrations of equal volumes of solutions of two monoprotic acids, Acid 1 and Acid 2.
Explain the differences between Acid 1 and Acid 2 in terms of their relative strengths and concentrations. (3 marks)
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→ Acid 1 is a strong acid. Its initial pH = 1 and its equivalence point is at pH = 7.
→ Acid 2 is a weaker acid. Its initial pH ~ 2 and its equivalence point is >7.
→ Acid 2 has a higher concentration than Acid 1 as it doesn’t take that much more
→ Acid 1 is a strong acid. Its initial pH = 1 and its equivalence point is at pH = 7.
→ Acid 2 is a weaker acid. Its initial pH ~ 2 and its equivalence point is >7.
→ Acid 2 has a higher concentration than Acid 1 as it doesn’t take that much more
40 mL of 0.10 mol L¯1
What is the pH of the resulting solution?
20.0 mL of 0.020 mol L¯1 barium hydroxide solution is added to 50.0 mL of 0.040 mol L¯1 hydrochloric acid solution.
What is the pH of the final solution?
What is the pH of the resultant solution after 20.0 mL of 0.20 mol
The reaction when
→
Therefore,