c5 salts and acids reactivity of metals and acids

Which ion do acids produce in aqueous solution?

H+ ions

How to obtain soluble salt crystals from an acid-base reaction

1. lace dilute acid in a beaker and heat gently.

2. Add the solid base bit by bit until it stops reacting, which means it's in excess.

3. Isolate the salt solution by filtering out the excess solid base using filter paper and a funnel.

Part 2 - Isolate the soluble salt crystals from the solution 

1. Heat the salt solution gently in a water bath until crystals start to form.

2. Let the solution cool further, which will cause more crystals to precipitate.

3. Filter out the soluble salt crystals using filter paper and funnel. 

how ud answer How to obtain soluble salt crystals from an acid-base reaction

To form the soluble salt 'nickel sulfate' you would need to react an insoluble base that contains nickel ions, and an acid that contains sulfate ions.

-nickel oxides

- sulfate acid. 

Nickel sulfate is composed of a nickel ion and a sulfate ion. This means that we need nickel oxide for the nickel ion, and sulfuric acid for the sulfate ion.

what is the name of this reaction: Acids reacting with alkalis

neutralisation

equation for acid + metal

acid + metal —> salt + hydrogen

add potassium hydroxide (solution) to the (conical) flask 1 add (a few drops of) indicator 1 add the (sulfuric) acid (from the burette) 1 until the colour (of the indicator) changes 1 read the volume from the burette

what does Hydrochloric acid produce

_____ (metal ie copper) + chloride

when we react acid with base or alkali,what is produced

when we react acid with base or alkali,salt and water is produced

when acids react with metal carbonate,what is produced

when acids react with metal carbonate,salt water and carbon dioxide is produced

predict the producss of this reaction: hydrochloric acid + copper carbonate → ____

hydrochloric acid + copper carbonate → copper chloride + salt + water + carbon dioxide

weak acid

produces H+,partially ionised

predict the products of this reaction: zinc oxide sulfuric acid → _____ + _____

zinc oxide sulfuric acid → zinc sulfate + water

what does hydrochloric,nitric and sulfric acid produce

(hydrochloric acid → produces chlorides,

nitric acid → produces nitrates,

sulfuric acid → produces sulfates)

what do bases that are chemicals do

bases are chemicals that neutralise acids to produce salt and water

whats alkalis

bases that are soluble in water are alkalis

in aqeous solutions, what do alkalis produce?

in aqeous solutions, alkalis produce hydroxide ions OH-

red- very acidic 0

green-netural 7

purple-very alkaline 14

equation for neutralisation

h+ (aq) + OH-(aq)→ h20 (l)

why do Insoluble bases like metal oxides and metal carbonates react with acids

Insoluble bases like metal oxides (e.g., copper oxide) and metal carbonates (e.g., copper carbonate) react with acids to form salts and water

dilute solution

A dilute solution means there is a ) small amount of acid per unit volume

A concentrated solution

A concentrated solution means there is a large amount of acid in a small volume of water (high concentration).

why do strong acids ionize completely in aqoeus solutions

ionic equation for neutralisaiton

h+ + OH- -> h20

what acid have ph of

acids have ph below 7strong acids have ph closer to 0,weak acids have ph closer to 6,

what base have ph of

base have ph above 7,strongbase have ph close to 14,weak base have ph close to 8

the higher the h+ conc the stronger the ___

the higher the h+ conc the stronger the acid

,the higher the oh- concentration the stronger the __

,the higher the oh- concentration the stronger the alkali

what has a lower pH than weak acids at the same concentration.

Strong acids have a lower pH than weak acids at the same concentration.

whats e.g of bases

bases = Insoluble metal hydroxides and metal oxides (

Describe a safe method for making pure crystals of copper sulfate from copper carbonate and dilute sulfuric acid. Use the information in the figure above to help you. In your method you should name all of the apparatus you will use

e content • sulfuric acid in beaker (or similar) • add copper carbonate one spatula at a time • until copper carbonate is in excess or until no more effervescence occurs • filter using filter paper and funnel • filter excess copper carbonate • pour solution into evaporating basin / dish • heat using Bunsen burner • leave to crystallise / leave for water to evaporate / boil off water • decant solution • pat dry (using filter paper) • wear safety spectacles / goggles Students. may choose to use a named indicator unt

Describe a method to make pure, dry crystals of magnesium sulfate from a metal oxide and a dilute acid.

use magnesium oxide and sulfuric acid • add sulfuric acid to a beaker • warm sulfuric acid • add magnesium oxide • stir • continue adding until magnesium oxide is in excess • filter • using a filter paper and funnel • to remove excess magnesium oxide • heat solution in an evaporating basin • to crystallisation point • leave to crystallise • pat dry with filter paper

burette measures variable volume

oxidation and reduction in terms of oxygen

oxidation- gain oxygen re

soluble/insoluble meaning

dissolves in water,doesnt

titration practical e.g Describe a method to find the exact volume of sodium hydroxide thatreacts with 25.0 cm3 of hydrochloric acid

fill burette with sodium hydroxide 1 add sodium hydroxide from the burette to the hydrochloric acid and indicator 1 stop when colour changes 1 measure volume used from burette

method of salt practical

general Method for Preparing Salts from an Acid and a Metal Carbonate:

1. Materials:

   • Metal carbonate (e.g., copper carbonate (CuCO₃), magnesium carbonate (MgCO₃), calcium carbonate (CaCO₃))

   • Acid (e.g., hydrochloric acid (HCl), sulfuric acid (H₂SO₄), nitric acid (HNO₃))

   • Conical flask, filter paper, funnel, beaker, evaporating dish, heat source

2. Method:

   • Step 1: Measure 25 cm³ of acid (e.g., hydrochloric acid (HCl)) and pour it into the conical flask.

     • What to change: Use the acid specified in the question (e.g., sulfuric acid for sulfates, nitric acid for nitrates).

   • Step 2: Add metal carbonate (e.g., copper carbonate (CuCO₃)) to the acid in the flask.

     • What to change: Use the metal carbonate specified (e.g., magnesium carbonate or calcium carbonate).

     • Reaction example: Metal carbonate+Acid→Salt+Water+Carbon dioxide (CO₂)\text{Metal carbonate} + \text{Acid} \rightarrow \text{Salt} + \text{Water} + \text{Carbon dioxide (CO₂)}Metal carbonate+Acid→Salt+Water+Carbon dioxide (CO₂)

   • Step 3: Continue adding the metal carbonate until the reaction stops, which is when no more bubbles (effervescence) are produced. This indicates all the acid has reacted.

   • Step 4: Filter the solution to remove any unreacted metal carbonate.

     • The salt will be dissolved in the remaining solution, while any excess metal carbonate will be left behind in the filter paper.

   • Step 5: Evaporate the filtered solution to remove the water, leaving behind salt crystals.

     • What to change: The salt produced will depend on the acid you used:

       • If you used hydrochloric acid (HCl) → the salt will be copper chloride (CuCl₂).

       • If you used sulfuric acid (H₂SO₄) → the salt will be copper sulfate (CuSO₄).

       • If you used nitric acid (HNO₃) → the salt will be copper nitrate (Cu(NO₃)₂).

   • Step 6: Dry the salt crystals by leaving them in a warm place or using filter paper.

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What is the Salt?

The salt is the product formed when the acid reacts with the metal carbonate. It consists of the metal ion (from the metal carbonate) and the anion (from the acid).

• In copper chloride (CuCl₂): The copper ion (Cu²⁺) comes from the copper carbonate (CuCO₃), and the chloride ion (Cl⁻) comes from the hydrochloric acid (HCl).

• In copper sulfate (CuSO₄): The copper ion (Cu²⁺) comes from the copper carbonate (CuCO₃), and the sulfate ion (SO₄²⁻) comes from the sulfuric acid (H₂SO₄).

• In copper nitrate (Cu(NO₃)₂): The copper ion (Cu²⁺) comes from the copper carbonate (CuCO₃), and the nitrate ion (NO₃⁻) comes from the nitric acid (HNO₃).

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Key Parts to Change in the Method:

1. Acid: Change depending on the salt you need:

   • Hydrochloric acid (HCl) → produces chlorides.

   • Sulfuric acid (H₂SO₄) → produces sulfates.

   • Nitric acid (HNO₃) → produces nitrates.

2. Metal carbonate: Change depending on the question:

   • Copper carbonate (CuCO₃) → produces copper salts.

   • Magnesium carbonate (MgCO₃) → produces magnesium salts.

   • Calcium carbonate (CaCO₃) → produces calcium salts.

Summary of What You Need to Change:

Summary of What You Need to Change:

• The acid will determine the type of salt (chlorides, sulfates, nitrates).

• The metal carbonate will determine the metal ion in the salt.

• Everything else in the method stays the same (filtering, evaporating, drying).

Write the ionic equation for this neutralisation reaction. Include state symbols.

H+ (aq) + OH− (aq) → H2O(l)

gen thing

acid in burette or flask • alkali/sodium hydroxide or acid in burette or flask • volume of acid or alkali measured using the pipette • indicator in flask • white tile under the flask • slow addition • swirling/mixing • colour change of indicator • burette volume measured