Equilibria

Question 1 of 29

1

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Acids are proton

Explanation

Question 2 of 29

1

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Acids are acceptors

Explanation

Question 3 of 29

1

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acids completely dissociate

Explanation

Question 4 of 29

1

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Weak acids dissociate to set up an equilibrium

Explanation

Question 5 of 29

1

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More H+ ions mean a stronger acid because there are

Explanation

Question 6 of 29

1

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Weaker acids dissociate less so equilibrium moves to the

Explanation

Question 7 of 29

1

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Strong bases completely dissociate into in an solution

Explanation

Question 8 of 29

1

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bases partially react to give ions. An equilibrium is set up when they dissolve in .

Explanation

Question 9 of 29

1

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Buffer solutions are solutions which resist changes in when small quantities of or are added.

Explanation

Question 10 of 29

1

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The are two types of buffer solution, and .

Explanation

Question 11 of 29

1

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Buffer solutions must be made of acids and bases so that an is present. This allows ions to be removed and produced. Strong acids can't be used as they fully dissociate so can't be removed.

Explanation

Question 12 of 29

1

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Buffer solutions are found in the and the blood.

Explanation

Question 13 of 29

1

Calculate the pH of 0.1M of HCl

Select one of the following:

1
2
1.9
12

Explanation

Question 14 of 29

1

The dissociation constant for a weak acid is given the symbol ...

Select one of the following:

Ksp
SpK
Ka
Kc
mol

Explanation

Question 15 of 29

1

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Weaker acids dissociate less to give ions so is smaller but pKa is larger.

Explanation

Question 16 of 29

1

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An acid with more is a stronger acid because the anion is more stable due to electron effect.

Explanation

Question 17 of 29

1

What is the symbol for the equilibrium constant?

Select one of the following:

Kw
mol
Ka
Kc

Explanation

Question 18 of 29

1

Calculate the pH of 0.001M NaOH...

Select one of the following:

14
3
12
11

Explanation

Question 19 of 29

1

Kw varies with temperature

Select one of the following:

True
False

Explanation

Question 20 of 29

1

Find the H+ conc in 0.01moldm-3 solution of NaOH...

Select one of the following:

1x10 to the power of -12
1
12
1x10 to the power of -2

Explanation

Question 21 of 29

1

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Many indicators are acids as they in solution. The removal of the ion causes a colour change.

Explanation

Question 22 of 29

1

Click on each orange point and write the correct answer.

Indicate on the image at what point in the titration a suitable indicator would change colour:
For boxes you believe to be incorrect insert - x
In the box you believe to be correct write - indicator

Explanation

Question 23 of 29

1

What is involved in the titration of these curves?

Select correct option below corresponding to the highlighted orange point

weak acid and weak base

strong acid and strong base

strong acid and weak base

weak acid and strong base

Explanation

Question 24 of 29

1

Fill the blank spaces to complete the text.

The 3 steps in calculating the pH of a buffer solution are as follows:

1- convert Ka to using
2-place values into equation pH=pKa+ log [] / []
3- calculate the pH

Explanation

Question 25 of 29

1

At what point during an acid base titration does
a concentrated acid = concentrated conjugate base

Select one of the following:

end point
neutralisation point
half point of neutralisation
initially ( as soon as the titration begins)

Explanation

Question 26 of 29

1

	Created by Megan Thomas over 6 years ago

Quiz for A Level Chemistry topic of Equilibria

Question 1 of 29

Fill the blank space to complete the text.

Acids are proton

Explanation

Question 2 of 29

Fill the blank space to complete the text.

Acids are acceptors

Explanation

Question 3 of 29

Fill the blank space to complete the text.

acids completely dissociate

Explanation

Question 4 of 29

Fill the blank space to complete the text.

Weak acids dissociate to set up an equilibrium

Explanation

Question 5 of 29

Fill the blank space to complete the text.

More H+ ions mean a stronger acid because there are

Explanation

Question 6 of 29

Fill the blank space to complete the text.

Weaker acids dissociate less so equilibrium moves to the

Explanation

Question 7 of 29

Fill the blank spaces to complete the text.

Strong bases completely dissociate into in an solution

Explanation

Question 8 of 29

Fill the blank spaces to complete the text.

bases partially react to give ions. An equilibrium is set up when they dissolve in .

Explanation

Question 9 of 29

Fill the blank spaces to complete the text.

Buffer solutions are solutions which resist changes in when small quantities of or are added.

Explanation

Question 10 of 29

Fill the blank spaces to complete the text.

The are two types of buffer solution, and .

Explanation

Question 11 of 29

Fill the blank spaces to complete the text.

Buffer solutions must be made of acids and bases so that an is present. This allows ions to be removed and produced. Strong acids can't be used as they fully dissociate so can't be removed.

Explanation

Question 12 of 29

Fill the blank space to complete the text.

Buffer solutions are found in the and the blood.

Explanation

Question 13 of 29

Calculate the pH of 0.1M of HCl

Select one of the following:

Explanation

Question 14 of 29

The dissociation constant for a weak acid is given the symbol ...

Select one of the following:

Explanation

Question 15 of 29

Fill the blank spaces to complete the text.

Weaker acids dissociate less to give ions so is smaller but pKa is larger.

Explanation

Question 16 of 29

Fill the blank spaces to complete the text.

An acid with more is a stronger acid because the anion is more stable due to electron effect.

Explanation

Question 17 of 29

What is the symbol for the equilibrium constant?

Select one of the following:

Explanation

Question 18 of 29

Calculate the pH of 0.001M NaOH...

Select one of the following:

Explanation

Question 19 of 29

Kw varies with temperature

Select one of the following:

Explanation

Question 20 of 29

Find the H+ conc in 0.01moldm-3 solution of NaOH...

Indicate on the image at what point in the titration a suitable indicator would change colour:
For boxes you believe to be incorrect insert - x
In the box you believe to be correct write - indicator

The 3 steps in calculating the pH of a buffer solution are as follows:

1- convert Ka to using
2-place values into equation pH=pKa+ log [] / []
3- calculate the pH

At what point during an acid base titration does
a concentrated acid = concentrated conjugate base