Acids and Bases
description
Transcript of Acids and Bases
Acids and Bases
Take 2!
pH
• pH depends on the concentration of hydrogen ion (H+)in the solution
–Lots of hydrogen ion = low pH
–Very little hydrogen ion = high pH
What’s concentration?
• Involves the amount of solute (solute is the dissolved
stuff) and the volume of the solution
• Demo of concentration
Vocabulary
• Dilute:
–Verb – to make less concentrated, usually by adding solvent (water)
–Adjective - of or pertaining to a solution that has a low concentration of solute
Diluting acids
• Does the amount of acid change when you add water to it?
• What changes?
• Will the pH change?
• How much?
Molarity (M)
• Concentration is usually measured in units of molarity. It is defined as:
• Molarity =
• Solute could be acid or base moles!
lutionlitersofso
utemolesofsol
Dilution
• When you add water to the acid, you dilute it, but the number of moles of acid DO NOT change. Only the volume of the liquid solution changes.
Molarity Practice
• If 3.00 moles of acid are added to enough water to make 3.00 liters of solution, what is the concentration (molarity) of the acid solution?
Molarity Practice
• If 1.00 moles of acid are added to enough water to make 4.00 liters of solution, what is the concentration (molarity) of the acid solution?
Molarity Practice
• If 4.00 moles of base are added to enough water to make 2.00 liters of solution, what is the concentration (molarity) of the acid solution?
Molarity Practice
• In 0.200 L of a 1.00 M acid solution, how many moles of acid are there?
Molarity Practice
• In 0.500 L of a 0.200 M acid solution, how many moles of acid are there?
Neutralization
• When acid and base are added:
• Acid + base water + a salt
• Remember salts include almost all ionic compounds
Neutralization
• Example
• HCl + NaOH H2O + NaCl
• This one makes water and table salt!
Neutralization
• Example
• HCH3COO + NaOH H2O + NaCH3COO
• This one makes water and a different salt!
Forming water
• Water is made because the H+ from the acid and the hydroxide ion (OH-) from the base get together to form water.
• If you don’t add exactly the same moles of acid and base, you will have more than just water and salt!
Did I add too much Base?
• How could you know whether you’ve exactly cancelled out the acid?
• Ans: TITRATION!!!!!!!
–And – use an indicator or check the pH
Titration
• Add Base carefully to acid and measure EXACTLY how much was used.
• The picture shows a burette tube being used to drop base in acid.
Measuring Volumes
• The meniscus is the curve at the top. Measure from the bottom of the meniscus.
• Notice that the low numbers are on top!
Measuring Volumes
• Notice that you can see if the meniscus is between lines or right on a line.
• Your volume measurement should have 2 decimal places.
Measuring Volumes
• What volume is this indicating?
Phenolphthalein
• It turns pink in base – but is clear in acid.
• The range is 8-9
• This needs to be swirled to see if the pink will go away!
ENDPOINT
• The titration is done at the ENDPOINT.
• That’s where the solution stays pink! (hopefully light pink, otherwise there is too much base!)
Calculations
• The whole point is to calculate the concentration of the acid or base.
• At the endpoint
moles of acid = moles of base
Calculations
• And remember –Moles = molarity X volume
• so
MaVa = MbVb
Molarity X volume = molarity X volume
Practice calculations
• 10.0 mL of a solution of potassium hydroxide was titrated with a 0.10 M solution of hydrochloric acid. 13.5 mL of the acid was required for neutralization. Calculate the concentration of the potassium hydroxide solution.
Practice Calc.
• Write down everything you know.
• ACID BASE• Hydrochloric Acid Potassium hydroxide
• Volume used = 13.5mL Volume used = 10.0 mL
Va Vb • Conc. = 0.10 M Concentration =?
Ma Mb • Then set up MaVa = MbVb
Answer
• 0.1M x 13.5 = Mb x 10.0
• Mb = 0.135 M