Titrations

acid + base ₋>

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

HCl + NaOH → 

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

What is the endpoint of a titration

• Where the amount of acid and base are balanced according to the equation
• Where there is no base
• At the end

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

• 2.5mL
• 5mL
• 25mL
• 50mL

Tags

NGSS.HS-PS1-7

what is the reading on this burette?

• 4.40mL
• 3.50mL
• 3.60mL
• 4.50mL

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

• 0.8 M
• 1 M
• 1.25 M

Tags

NGSS.HS-PS1-7

Identify the products of the chemical equation
3 LiOH + H₃PO₄ →

• Li₃PO₄ + 3 H₂O
• LiPO₄ + 3 H₂O
• Li(PO₄)₃ + 3 H₂O
• BOY + La + N₂

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

What acid and what base would you choose to prepare the salt potassium chlorate?

• KOH and HClO₃
• KOH and HClO₂
• HK and OHClO₃
• HK and OHClO₂

A 50.0 mL sample of Ca(OH)₂ is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)₂ solution.

• 1.0 M
• 0.50 M
• 0.15 M 
• 0.30 M

How many moles of Ca(OH)₂ are needed to neutralize three moles of HCl? 

• 8
• 1.5
• 6
• 3