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13.5Unit 8: Energy changes and reactions of metals

Reactions of metals with dilute acids

5 min read 5 parts Lesson 5 of 5 1 quiz

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Lesson summary

13.5 Reactions of metals with dilute acids — CHECKPOINT (CHEMISTRY) notes: Describe how metals react with dilute acids and name the salts formed.General equation — metal + acid → salt + hydrogenExample — magnesium + hydrochloric acid → magnesium chloride + hydrogenSalt = a compou…

  • Observations
  • Independent variable
  • Control variables
  • Measuring cylinder
  • Combining results
  • Reactivity

Section 1 of 5Metal and acid

  • General equation
    • metal + acid → salt + hydrogen
  • Example
    • magnesium + hydrochloric acid → magnesium chloride + hydrogen
  • Salt = a compound formed when the metal replaces the hydrogen of an acid
  • Observations
    • fizzing as hydrogen is given off, the metal gets smaller, and the tube may warm

Section 2 of 5Naming the salts

AcidSalt ending
Hydrochloric acidchloride
Sulfuric acidsulfate
Nitric acidnitrate
  • Examples
    • magnesium + sulfuric acid → magnesium sulfate + hydrogen; zinc + nitric acid → zinc nitrate + hydrogen

Section 3 of 5Order of reactivity

MetalReaction with dilute hydrochloric acid
MagnesiumFast fizzing, many bubbles
ZincSteady fizzing
IronSlow
Copper, silver, goldNo reaction
Sodium, potassium, calciumToo dangerous to test

Section 4 of 5Planning the investigation

  • Independent variable
    • the metal used
  • Dependent variable
    • how fast bubbles form or the temperature change
  • Control variables
    • the volume and concentration of acid and the size of the metal piece
  • Safety
    • wear safety glasses and do not use sodium, potassium or calcium
  • Measuring cylinder
    • choose one that measures the acid volume accurately

Section 5 of 5Reactivity order

  • Combining results
    • results from oxygen, water and acid reactions give one reactivity order
  • Poster
    • shows metals from most reactive at the top to least reactive at the bottom

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