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% Document Info
\author{Jackqueslack23}
\pdfinfo{
  /Title (gcse-chemistry-reactions-of-acids.pdf)
  /Creator (Cheatography)
  /Author (Jackqueslack23)
  /Subject (GCSE Chemistry - Reactions of Acids Cheat Sheet)
}

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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{GCSE Chemistry - Reactions of Acids Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{Jackqueslack23} via \textcolor{DarkBackground}{\uline{cheatography.com/166796/cs/37604/}}}
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  \vspace{-2pt}Jackqueslack23 \\
  \uline{cheatography.com/jackqueslack23} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 9th March, 2023.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
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\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{x{1.44 cm} x{6.56 cm} }
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Acids and Bases}}  \tn
% Row 0
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{\bf{ACIDS}} & Acids in solution are sources of hydrogen ions. \tn 
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% Row 1
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 & Acidic solutions have lower pH values than neutral pH 7. \tn 
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{\bf{BASES}} & A base is any substance that reacts with an acid to form a salt and water only. \tn 
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 & Alkalis (soluble bases) in solution are sources of hydroxide ions. \tn 
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 & Alkaline solutions have higher pH values than neutral 7. \tn 
% Row Count 12 (+ 2)
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\mymulticolumn{2}{x{8.4cm}}{Higher H+ concentration = lower pH​  \newline Higher OH- concentration = higher pH}  \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Descriptions/Forms of Acid}}  \tn
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{\bf{Concentrated acid}} & a relatively large amount of solute dissolved in the solvent. \tn 
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{\bf{Dilute acid}} & a relatively smaller amount of solute dissolved in the solvent. ​ \tn 
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% Row 2
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{\bf{Strong acid}} & completely ionised in aqueous solution. Hydrochloric, nitric and sulfuric acid.​ \tn 
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\SetRowColor{white}
{\bf{Weak acid}} & only partially ionised in aqueous solution. Ethanoic, citric and carbonic.​ Further, it has a lower pH than a strong acid (aq) of the same concentration.​  This is because a weak acid has a lower concentration of hydrogen ions.​ \tn 
% Row Count 19 (+ 9)
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Reactions (Part2)}}  \tn
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Salts can be made by reacting an acid with an alkali. & Acid + Alkali + Salt + Water \tn 
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Salts can be made by reacting an acid with a insoluble base.​ & Acid + Bases = Salt + Water​ \tn 
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Salts can be made by reacting an acid with a metal carbonate.​ & Acid + Metal carbonate = Salt + Water + Carbon dioxide \tn 
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\mymulticolumn{2}{x{8.4cm}}{Acids are neutralized by alkalis (e.g.: soluble metal hydroxides) and bases (e.g.: insoluble metal hydroxides and metal oxides) to produce salts and water and by metal carbonates to produce ​salts, water and carbon dioxide. The salt name depends on the acid used and the positive ions in the alkali, base or carbonate.​}  \tn 
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\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Indicators}}  \tn
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\mymulticolumn{1}{x{8.4cm}}{Litmus goes red in acid and blue in alkali.} \tn 
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% Row 1
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\mymulticolumn{1}{x{8.4cm}}{Methyl orange is red in acidic conditions, yellow in neutral and alkaline conditions.} \tn 
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\mymulticolumn{1}{x{8.4cm}}{Phenolphthalein is colourless in acidic and neutral conditions and pink in alkaline conditions.} \tn 
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\mymulticolumn{1}{x{8.4cm}}{Universal indicator - scale runs from 0 (red), 7 (green) to 14 (blue).} \tn 
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Salts made when metals react with nitric acid are called nitrates.​ & Zinc +  Nitric acid = Zinc Nitrate + Hydrogen​ \tn 
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Salts made when metals react with sulfuric acids are called sulfates.​ & Iron + Sulfuric Acid = Iron Sulfate + Hydrogen​ \tn 
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Salts made when metals react with hydrochloric acid are called chlorides.​ & Magnesium + Hydrochloric acid = Magnesium Chloride + Hydrogen \tn 
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\mymulticolumn{2}{x{8.4cm}}{Reactions between metals and acids only occur if the metal is more reactive than the hydrogen in the acid.  If the metal is too reactive, the reaction with acid is violent.​}  \tn 
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% That's all folks
\end{multicols*}

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