Acids, Bases, and pH - SS2 Chemistry Past Questions and Answers - page 2
If the hydrogen ion concentration of a solution is 10-12 M, what is the pH of the solution?
2
4
10
12
To calculate the pH from the hydrogen ion concentration, we use the equation pH = -log[H+]. Taking the logarithm (base 10) of 10-12, we find that the pH is 12.
Calculate the pH of a solution with a hydrogen ion concentration of 1 x 10-3 M.
The pH of a solution can be calculated using the formula:
pH = -log[H+]
Given that the hydrogen ion concentration ([H+]) is 1 x 10-3 M, we can substitute this value into the formula:
pH = -log(1 x 10-3)
pH = -(-3) = 3
Therefore, the pH of the solution is 3.
Determine the hydrogen ion concentration ([H+]) of a solution with a pH of 9.
The hydrogen ion concentration can be calculated by taking the antilog of the negative pH value:
[H+] = 10(-pH)
Given that the pH is 9, we can substitute this value into the formula:
[H+] = 10(-9)
[H+] = 1 x 10(-9)
Therefore, the hydrogen ion concentration of the solution is 1 x 10(-9) M.
Calculate the pH of a solution with a hydroxide ion concentration of 1 x 10-11 M.
To calculate the pH of a solution based on the hydroxide ion concentration, we can use the pOH formula:
pOH = -log[OH-]
Since pH + pOH = 14 (at 25°C), we can subtract the pOH value from 14 to obtain the pH:
pH = 14 - pOH
Given that the hydroxide ion concentration ([OH-]) is 1 x 10-11 M, we can calculate the pOH:
pOH = -log(1 x 10-11) = 11
Substituting the pOH value into the pH formula:
pH = 14 - 11 = 3
Therefore, the pH of the solution is 3.
Calculate the pH of a solution with a hydroxide ion concentration of 1 x 10-11 M.
To calculate the pH of a solution based on the hydroxide ion concentration, we can use the pOH formula:
pOH = -log[OH-]
Since pH + pOH = 14 (at 25°C), we can subtract the pOH value from 14 to obtain the pH:
pH = 14 - pOH
Given that the hydroxide ion concentration ([OH-]) is 1 x 10-11 M, we can calculate the pOH:
pOH = -log(1 x 10-11) = 11
Substituting the pOH value into the pH formula:
pH = 14 - 11 = 3
Therefore, the pH of the solution is 3.
Which of the following indicators is commonly used to detect the endpoint in an acid-base titration?
Bromothymol blue
Phenolphthalein
Methyl orange
Litmus
Which indicator is suitable for determining the pH of a strong acid solution?
Bromothymol blue
Methyl orange
Phenolphthalein
Thymol blue
Which indicator would be most appropriate for measuring the pH of a weak base solution?
Bromothymol blue
Methyl orange
Phenolphthalein
Litmus
Which indicator is commonly used to distinguish between acidic and basic solutions based on colour changes?
Bromothymol blue
Phenolphthalein
Methyl orange
Litmus
An indicator that changes colour in a pH range of 4.0 to 6.0 is:
Bromothymol blue
Methyl orange
Phenolphthalein
Litmus