Titrations

acid + alkali ₋>

• salt + hydrogen
• salt + water
• salt + carbon dioxide + water
• salt

HCl + NaOH → 

• NaH + ClOH
• NaCl + H₂
• NaCl + H₂O
• NaCl + Cl₂

Tags

NGSS.MS-PS1-1

NGSS.MS-PS1-2

NGSS.MS-PS1-5

What is the endpoint of a titration

• Where the amount of acid and alkali are balanced according to the equation
• Where the colour changes
• At the end

Why should you repeat your titration until you have results that are concordant (within 0.1cm³ of each other)

• To make sure your answer is accurate
• To make sure your answer is precise

I am titrating 1M HCl with 1M NaOH.  I have 25cm³ of HCl. How much NaOH will I need?

• 2.5cm³
• 5cm³
• 25cm³
• 50cm³

what is the reading on this burette?

• 4.4cm³
• 3.5cm³
• 3.6cm³
• 4.5cm³

I have 25cm³ of 1M HCl which neutralises 20cm³ of NaOH. What is the concentration of the NaOH?

• 0.8 M
• 1 M
• 1.25 M

I have 50cm³ of 0.1M HCl. How many moles of NaOH will I need to neutralise it?

• 5
• 0.5
• 0.05
• 0.005

What's the white tile for in the titration?

• To clearly see the colour change
• To protect the workbench from acid spills

Why do we use water to wash the solution from the burette into the flask

• To ensure accuracy (all solution reacts)
• To dilute the reagents
• To help the reaction go faster
• To see the colour of the indicator better