Acids, Alkalis, and Salts Flashcards
How to Preform a Titration
Add 50ml of Hydrochloric acid and Sodium Hydroxide too two separate beakers. Measure 25cm^3 of the Hydrochloric acid in to conical flask with a volumetric pipette filler. After add two or three drops of phenolphthalein. Add the alkali slowly into the acid from a volumetric pipette filler while swirling the conical flask. Record the results of how much of the alkali it took to make the acid go clear. Repeat to get a table of results and find a average
Titration calculation’s
concentration = moles / volume
Acids
- They are solutions that have a pH of below 7 on the pH scale
- They can contain hydrogen ions in their solution
- They can be corrosive when strong: however, some acids like citric and ethanoic acid can be eaten
Bases / Alkalis
- There are chemical substances that can react with acids to neutralise them
- They can sometimes be solids
- The types of compounds that are bases include metal oxides, hydroxides and carbonates
- Special bases that dissolve in water are “alkalis”. They have a pH of over 7 and contain “hydrogen ions”
Indicators
- These are substances that change colour depending upon whether they are acidic or alkaline solution
- Some have different colours depending upon the actual pH of the solution
Litmus indicator
- Litmus turns from red to blue in alkaline conditions
- Turns from blue to red in acidic conditions
Phenolphthalein indicator
- colourless in acidic solutions
- pink in alkaline solutions
Methyl Orange indicator
- Red in acidic solution
- Yellow in alkaline solution
The pH scale
A scale between 1-14 that is used to measure the strength of a acid or alkaline
Universal indicator
-Gives the colours that show the different pH values
-A mixture of indicators
-The colour gives you a actual pH value of the solution that you are testing
pH 1-6 is acidic
pH 7 is neutral
pH 8-14 is alkaline
Acids, Alkalis, Bases, and Salts
Acids are proton donors
Bases are proton acceptors
Alkalis are soluble bases
Salts are ionic compounds
Acid reactions
Acid + metal oxide —–> salt + water
e.g. sulfuric acid + zinc oxide —-> zinc sulfate + water
H2SO4 + ZnO —-> ZnSO4 + H2O
Acid + metal hydroxide —-> salt + water
Sulfuric acid + calcium hydroxide —-> calcium sulfate + water
H2SO4 + Ca(OH)2 —-> CaSO4 + 2H2O
Acid + metal carbonate —->salt + water +carbon dioxide
Hydrochloric acid + sodium carbonate —-> sodium chloride + water + carbondioxide
2HCl + Na2CO3 —-> 2NaCl + H2O + CO2