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\author{fongrsy}
\pdfinfo{
  /Title (acids-bases-and-alkalis.pdf)
  /Creator (Cheatography)
  /Author (fongrsy)
  /Subject (Acids, Bases and Alkalis Cheat Sheet)
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\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{C}
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    \vspace{-7pt}
    {\parbox{\dimexpr\textwidth-2\fboxsep\relax}{\noindent
        \hspace*{-6pt}\includegraphics[width=5.8cm]{/web/www.cheatography.com/public/images/cheatography_logo.pdf}}
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\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Acids, Bases and Alkalis Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{fongrsy} via \textcolor{DarkBackground}{\uline{cheatography.com/65383/cs/16397/}}}
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\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{LL}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}fongrsy \\
  \uline{cheatography.com/fongrsy} \\
  \end{tabulary}
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\begin{tabulary}{5.8cm}{L}
  \SetRowColor{FootBackground}
  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 21st July, 2018.\\
   Updated 26th July, 2018.\\
   Page {\thepage} of \pageref{LastPage}.
\end{tabulary}
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  \vspace{-5pt}
  %\includegraphics[width=48px,height=48px]{dave.jpeg}
  Measure your website readability!\\
  www.readability-score.com
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\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{p{0.74655 cm} x{4.23045 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Definitions}}  \tn
% Row 0
\SetRowColor{LightBackground}
Acids & Acids are compounds which ionise/dissociate in water to produce hydrogen ions (H\textasciicircum{}+\textasciicircum{}). \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
Bases & Bases are compounds that are metal oxides or hydroxides that react with an acid to give a salt and water only. \tn 
% Row Count 7 (+ 4)
% Row 2
\SetRowColor{LightBackground}
\seqsplit{Alkalis} & Alkalis are bases that ionise/dissociate in water to produce hydroxide ions (OH\textasciicircum{}-\textasciicircum{}). \tn 
% Row Count 10 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{1.04425 cm} x{1.00248 cm} x{1.12779 cm} x{1.00248 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{4}{x{5.377cm}}{\bf\textcolor{white}{Examples of Acids \& Bases}}  \tn
% Row 0
\SetRowColor{LightBackground}
Acid & Chemical Formula & Base & Chemical Formula \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\seqsplit{Hydrochloric} Acid & HCl & Magnesium Oxide & MgO \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
Sulfuric Acid & H2SO4 & Copper (II) Oxide & CuO \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
Nitric Acid & HNO3 & Sodium Hydroxide & NaOH \tn 
% Row Count 8 (+ 2)
% Row 4
\SetRowColor{LightBackground}
Citric Acid & C6H8O7 & Potassium Hydroxide & KOH \tn 
% Row Count 10 (+ 2)
% Row 5
\SetRowColor{white}
Ethanoic Acid & CH3CO2H & Calcium Hydroxide & Ca(OH)2 \tn 
% Row Count 12 (+ 2)
% Row 6
\SetRowColor{LightBackground}
Lactic Acid & C3H6O3 & Aqueous Ammonia & NH3 \tn 
% Row Count 14 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}----}
\SetRowColor{LightBackground}
\mymulticolumn{4}{x{5.377cm}}{Acids 1 to 3 are known as mineral / inorganic acids while Acids 4 to 6 are known as organic acids. \newline  \newline Bases 1 \& 2 are insoluble bases while Bases 3 to 6 are soluble bases / alkalis.}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}----}
\end{tabularx}
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\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Metal Reactivity Series}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/fongrsy_1532572042_metal reactivity series.png}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Types of Reactions}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{Metal + Acid \{\{fa-arrow-right\}\} Salt + Hydrogen Gas \newline % Row Count 2 (+ 2)
Metal Carbonate + Acid \{\{fa-arrow-right\}\} Salt + Water + Carbon Dioxide \newline % Row Count 4 (+ 2)
Metal Oxide + Acid \{\{fa-arrow-right\}\} Salt + Water \newline % Row Count 6 (+ 2)
Metal Hydroxide + Acid \{\{fa-arrow-right\}\} Salt + Water \newline % Row Count 8 (+ 2)
Base + Acid \{\{fa-arrow-right\}\} Salt + Water (Neutralisation) \newline % Row Count 10 (+ 2)
Alkali + Acid \{\{fa-arrow-right\}\} Salt + Water (Neutralisation) \newline % Row Count 12 (+ 2)
Alkali + Ammonium Salt \{\{fa-arrow-right\}\} Salt + Water + Ammonia Gas \newline % Row Count 14 (+ 2)
Alkali + Salt \{\{fa-arrow-right\}\} Metal Hydroxide + Salt% Row Count 16 (+ 2)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Tests for Gases: \newline Hydrogen Gas - Extinguishes a lighted splinter with a 'pop' sound. \newline Carbon Dioxide Gas - Released as effervescence. Reacts with limewater to form a white precipitate. \newline Ammonia Gas - Pungent odour. Turns red litmus paper blue. \newline  \newline Notes:  \newline Base / Alkali + Acid is an exothermic reaction. \newline Pb (s) + H2SO4 / HCl \{\{fa-arrow-right\}\} PbSO4 / PbCl2 + H2  \newline Lead reacts slowly then stops. Salt forms on the surface of the lead. The salt formed is insoluble.}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{pH Scale}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{Acidic solutions have pH values \textless{} 7. \newline % Row Count 1 (+ 1)
They contain {\bf{more}} H\textasciicircum{}+\textasciicircum{} ions and {\bf{fewer}} OH\textasciicircum{}-\textasciicircum{} ions. \newline % Row Count 3 (+ 2)
Neutral solutions have pH values = 7. \newline % Row Count 4 (+ 1)
They contain {\bf{equal amounts}} of H\textasciicircum{}+\textasciicircum{} ions and OH\textasciicircum{}-\textasciicircum{} ions. \newline % Row Count 6 (+ 2)
Alkaline solutions have pH values \textgreater{} 7. \newline % Row Count 7 (+ 1)
They contain {\bf{more}} OH\textasciicircum{}-\textasciicircum{} ions and {\bf{fewer}} H\textasciicircum{}+\textasciicircum{} ions.% Row Count 9 (+ 2)
} \tn 
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\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Ionic Equations}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{1. Write a balanced chemical equation with state symbols.} \tn 
% Row Count 2 (+ 2)
% Row 1
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\mymulticolumn{1}{x{5.377cm}}{2. Check which reactants and products can form ions in water. (Aqueous)} \tn 
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% Row 2
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\mymulticolumn{1}{x{5.377cm}}{3. Split up these reactants and products into their respective ions.} \tn 
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% Row 3
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\mymulticolumn{1}{x{5.377cm}}{4. Check for ions that appear in both LHS \& RHS of the equation, these are spectator ions that can be removed from the equation.} \tn 
% Row Count 9 (+ 3)
% Row 4
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\mymulticolumn{1}{x{5.377cm}}{5. For those reactants and products which are unable to form ions, do not split the compounds.} \tn 
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% Row 5
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\mymulticolumn{1}{x{5.377cm}}{6. What is left will be the net ionic equation. The coefficients must be in the lowest ratio.} \tn 
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\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
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\begin{tabularx}{5.377cm}{p{0.86963 cm} x{1.32733 cm} x{2.38004 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{3}{x{5.377cm}}{\bf\textcolor{white}{Polyatomic Ions}}  \tn
% Row 0
\SetRowColor{LightBackground}
Charge & Name & Chemical Formula \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
1+ & Ammonium & NH4\textasciicircum{}+\textasciicircum{} \tn 
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 & Hydronium & H3O\textasciicircum{}+\textasciicircum{} \tn 
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1- & Nitrate & NO3\textasciicircum{}-\textasciicircum{} \tn 
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 & Hydroxide & OH\textasciicircum{}-\textasciicircum{} \tn 
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 & Ethanoate & CH3COO\textasciicircum{}-\textasciicircum{} \tn 
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2- & Carbonate & CO3\textasciicircum{}2-\textasciicircum{} \tn 
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 & Sulfate & SO4\textasciicircum{}2-\textasciicircum{} \tn 
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3- & Phosphate & PO4\textasciicircum{}3-\textasciicircum{} \tn 
% Row Count 9 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}---}
\SetRowColor{LightBackground}
\mymulticolumn{3}{x{5.377cm}}{Notes: \newline Silver ion: Ag\textasciicircum{}+\textasciicircum{} \newline Zinc ion: Zn\textasciicircum{}2+\textasciicircum{}}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}---}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Properties of Acids}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{1. Acids are corrosive. \newline % Row Count 1 (+ 1)
2. Acids have a sour taste. \newline % Row Count 2 (+ 1)
3. Acidic solutions conduct electricity. (Electrolytes) \newline % Row Count 4 (+ 2)
4. Acids change the colour of indicators. \newline % Row Count 5 (+ 1)
Litmus Paper: Blue to Red \newline % Row Count 6 (+ 1)
Methyl Orange Solution: Orange to Red \newline % Row Count 7 (+ 1)
Universal Indicator Paper: Orange to Red \newline % Row Count 8 (+ 1)
Universal Indicator Solution: Green to Red% Row Count 9 (+ 1)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
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\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Properties of Alkalis}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{1. Alkalis have a soapy feeling and a bitter taste. \newline % Row Count 2 (+ 2)
2. Alkaline solutions conduct electricity. (Electrolytes) \newline % Row Count 4 (+ 2)
3. Alkalis change the colour of indicators. \newline % Row Count 5 (+ 1)
Litmus Paper: Red to Blue \newline % Row Count 6 (+ 1)
Methyl Orange Solution: Orange to Yellow \newline % Row Count 7 (+ 1)
Universal Indicator Paper: Orange to Violet \newline % Row Count 8 (+ 1)
Universal Indicator Solution: Green to Violet% Row Count 9 (+ 1)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
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\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Balancing Chemical Equations}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{Step 1: Write down the chemical equation. \newline % Row Count 1 (+ 1)
Step 2: List down the atoms (or polyatomic ions) involved in both sides. \newline % Row Count 3 (+ 2)
Step 3: Count the number of atoms on both sides. \newline % Row Count 4 (+ 1)
Step 4: Compare both sides and change the coefficients (not subscripts) so that the atoms on the left side are equal to the atoms on the right side. \newline % Row Count 7 (+ 3)
(Tip: Balance the {\bf{Metals}} first, then the {\bf{Non-Metals}}, and then the {\bf{Oxygen}} atoms and {\bf{Hydrogen}} atoms.) \newline % Row Count 10 (+ 3)
Step 5: Double check both sides to make sure the atoms on both sides are equal.% Row Count 12 (+ 2)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Soluble Salts}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\bf{Soluble}} & {\bf{Insoluble}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
All nitrates & None \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
Most sulfates & Lead sulfate, barium sulfate and calcium sulfate \tn 
% Row Count 5 (+ 3)
% Row 3
\SetRowColor{white}
Most chlorides, bromides and iodides & Silver chloride, silver bromide, silver iodide, lead chloride, lead bromide, lead iodide \tn 
% Row Count 10 (+ 5)
% Row 4
\SetRowColor{LightBackground}
Sodium carbonate, potassium carbonate, ammonium carbonate & Most other carbonates \tn 
% Row Count 13 (+ 3)
% Row 5
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Sodium hydroxide, potassium hydroxide, ammonium hydroxide & Most other hydroxides \tn 
% Row Count 16 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{1.4931 cm} x{3.4839 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Uses of Acids}}  \tn
% Row 0
\SetRowColor{LightBackground}
Citric Acid & Used as a sour flavouring agent in food \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\seqsplit{Hydrochloric} Acid & Used as a rust remover \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
Sulfuric Acid & Used in car batteries \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
Nitric Acid & Used in fertilisers \tn 
% Row Count 7 (+ 1)
% Row 4
\SetRowColor{LightBackground}
Ethanoic Acid & Used as a food preservative \tn 
% Row Count 9 (+ 2)
% Row 5
\SetRowColor{white}
Carbonic Acid & Used in making soft drinks \tn 
% Row Count 11 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{1.59264 cm} x{3.38436 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Uses of Alkalis}}  \tn
% Row 0
\SetRowColor{LightBackground}
Sodium Hydroxide & Used in making soap \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Calcium Hydroxide & Used in making toothpaste and to reduce acidity in soil \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
Aqueous Ammonia & Used in making fertilisers and as a bleaching agent \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
Aqueous Ammonia & Used in making fertilisers and as a bleaching agent \tn 
% Row Count 9 (+ 2)
% Row 4
\SetRowColor{LightBackground}
Potassium Hydroxide & Used in electroplating and in making cement and plaster \tn 
% Row Count 12 (+ 3)
% Row 5
\SetRowColor{white}
Magnesium Hydroxide & Used as a detergent \tn 
% Row Count 14 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{2.83689 cm} x{2.14011 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Strength of Acids}}  \tn
% Row 0
\SetRowColor{LightBackground}
Strong Acids & Weak Acids \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Hydrochloric Acid & Citric Acid \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
Sulfuric Acid & Tartaric Acid \tn 
% Row Count 3 (+ 1)
% Row 3
\SetRowColor{white}
Nitric Acid & Ethanoic Acid \tn 
% Row Count 4 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Strong Acids: \newline React very fast \& vigorously \newline Ionise completely to produce large amounts of H\textasciicircum{}+\textasciicircum{} ions \newline  \newline Weak Acids: \newline React slowly \& less vigorously \newline Ionise partially to produce small amounts of H\textasciicircum{}+\textasciicircum{} ions \newline  \newline {\bf{{\emph{Do not confuse the strength of an acid with the concentration of an acid. The strength tells you how many H\textasciicircum{}+\textasciicircum{} ions are produced while the concentration tells you how much of an acid is dissolved in water.}}}}}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{2.58804 cm} x{2.38896 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Strength of Alkalis}}  \tn
% Row 0
\SetRowColor{LightBackground}
Strong Alkalis & Weak Alkalis \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Sodium Hydroxide & Aqueous Ammonia \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Potassium Hydroxide} \tn 
% Row Count 3 (+ 1)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Calcium Hydroxide} \tn 
% Row Count 4 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Strong Alkalis ionise completely to produce large amounts of OH\textasciicircum{}-\textasciicircum{} ions. \newline Weak Alkalis ionise partially to produce small amounts of OH\textasciicircum{}-\textasciicircum{} ions.}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{How to Carry Out Titration}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{1. For solid samples, weigh the solid and dissolve in a known volume of solution (usually 100cm\textasciicircum{}3\textasciicircum{}). \newline % Row Count 3 (+ 3)
2. Use a pipette to measure a known volume of the solution (e.g 10cm\textasciicircum{}3\textasciicircum{}) and empty into an Erlenmeyer flask. \newline % Row Count 6 (+ 3)
3. Add a few drops of indicator into the solution. \newline % Row Count 8 (+ 2)
4. Put the second chemical into a burette. This other solution will react with the synthesised chemical sample in the flask. Often the solution in the burette is an acid or alkali, and it must be of a precise, known concentration. \newline % Row Count 13 (+ 5)
5. Drop by drop, mix the chemical in the burette into the Erlenmeyer flask until the end point is reached. A colour change indicates the correct amount has been added to react completely with the chemical in the sample. \newline % Row Count 18 (+ 5)
6. Take note of the volume of the solution added from the burette.% Row Count 20 (+ 2)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
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% That's all folks
\end{multicols*}

\end{document}