Year 12 Acids and Bases

Arrhenius theory defined acids as

• substances that dissociate to produce hydronium ions

• substances that dissociate to produce neutral solutions

• proton acceptors

• proton donors

water can be act as

• an amphiprotic substance

• an acid

• a base

• nothing, it's neutral

The enthalpy of neutralisation

• is always -55.9kJ/mol

• changes depending upon the type of acid and base used

• is higher than -55.9kJ/mol when strong acids are used

• is higher than -55.9kJ/mol when strong bases are used

Tags

NGSS.HS-PS1-4

In an experiment, 50.0mL of a standard NaOH solution is added to 50.0mL of 2.0M ethanoic acid. An increase in temperature is observed from 22.0 to 33.7 degrees. Calculate the enthalpy of neutralisation.

• 489000J

• -49kJ/mol

• 489000kJ

• -55.9kJ/mol

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

Reorder the following in increasing acidity

• HCl

• HF

The pH of a 0.2M solution of HCl is

• 0.7

• -0.7

• 0.698

• -0.698

the pH of a 4.5M solution of NaOH is

• 13

• -13.3

• 0.653

• 13.4

Answer explanation

Don't forget SIGNIFICANT FIGURES

In order to make a standard solution from a solid, I will need

• scales and a spatula

• volumetric flask and a beaker

• filter funnel

• burette and a pipette

I need to make a 50mL of a 0.250M solution from a 1.00M stock solution. What volume of the stock solution do I need?

• 12.5mL

• 0.125mL

• 0.125L

• 1.25mL

What amount of water will need to be added if I am making 50mL of a 0.5M solution from a 1.5M stock solution

• 33mL

• 17mL

• 0.333L

• 0.01667L