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% Document Info
\author{TheGoldenClover}
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  /Title (tahsili-chemistry-acids-and-bases.pdf)
  /Creator (Cheatography)
  /Author (TheGoldenClover)
  /Subject (Tahsili Chemistry (Acids and Bases) Cheat Sheet)
}

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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Tahsili Chemistry (Acids and Bases) Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{TheGoldenClover} via \textcolor{DarkBackground}{\uline{cheatography.com/201551/cs/42925/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}TheGoldenClover \\
  \uline{cheatography.com/thegoldenclover} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 4th April, 2024.\\
   Updated 2nd April, 2024.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{x{2.812 cm} x{3.496 cm} x{1.292 cm} }
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\mymulticolumn{3}{x{8.4cm}}{\bf\textcolor{white}{Properties of Acids and Bases}}  \tn
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\SetRowColor{LightBackground}
Arrhenius theory & acids are substances that contains hydrogen and dissociates to produce H\textasciicircum{}+\textasciicircum{}, and a base is any substance that cointains hydroxide and dissociates to produce OH\textasciicircum{}-\textasciicircum{} &  \tn 
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disadvantage of arrhenius theory & not all bases contain OH, but can produce it when dissolved in water & Ex: NH3 - NaCO3 \tn 
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\seqsplit{Bronsted-Lowry} Theory & Acids are H\textasciicircum{}+\textasciicircum{} donors, bases are H\textasciicircum{}+\textasciicircum{} acceptors &  \tn 
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Conjugate Pairs & acids that donate H\textasciicircum{}+\textasciicircum{} and become bases are called conjugate bases, while bases that accept H\textasciicircum{}+\textasciicircum{} and become acids are called conjugate acids &  \tn 
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\mymulticolumn{3}{x{8.4cm}}{{\emph{acids and bases are both electrolytes}}} \tn 
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\mymulticolumn{3}{x{8.4cm}}{{\emph{water can act as an acid and base, so it is amphoteric}}} \tn 
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\par\addvspace{1.3em}

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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{PH and POH}}  \tn
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PH = -log{[}H\textasciicircum{}+\textasciicircum{}{]}\{\{ac\}\} & POH = -log{[}OH\textasciicircum{}-\textasciicircum{}{]}\{\{ac\}\} \tn 
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\mymulticolumn{2}{x{8.4cm}}{PH + POH = 14\{\{ac\}\}} \tn 
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\mymulticolumn{3}{x{8.4cm}}{\bf\textcolor{white}{Monoprotic and Polyprotic Acids}}  \tn
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Monoprotic Acid & can only donate one H\textasciicircum{}+\textasciicircum{} ion &  \tn 
% Row Count 2 (+ 2)
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Polyprotic Acid & can donate multiple H\textasciicircum{}+\textasciicircum{} ions &  \tn 
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Lewis Theory & acids are an electron pair acceptor, bases are an electron pair donor &  \tn 
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Lewis Acids & BF3, BCl3, H\textasciicircum{}+\textasciicircum{}, Ag\textasciicircum{}+\textasciicircum{} &  \tn 
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Lewis Bases & F\textasciicircum{}\_\textasciicircum{}, PCl3, NH3, Cl\textasciicircum{}\_\textasciicircum{} &  \tn 
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Acidic Anhydrides & nonmetal oxides that react with water to produce an acid & Ex: CO2 \tn 
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Basic Anhydrides & metal oxides that react with water to form a base & Ex: CaO \tn 
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water dissociation constant (kw) & {[}H\textasciicircum{}+\textasciicircum{}{]} x {[}OH\textasciicircum{}\_\textasciicircum{}{]} = 10\textasciicircum{}-14\textasciicircum{} &  \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Neutralization and Titration}}  \tn
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\seqsplit{Neutralization} Reaction & acid + base = water + salt \tn 
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Titration & a method of finding an unknown acid or base's concentration by using a known one (standard solution) \tn 
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Equivalence Point & Moles H\textasciicircum{}+\textasciicircum{} = Moles OH\textasciicircum{}-\textasciicircum{} \tn 
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acid-base indicators & substances that change color in acidic or basic solutions (bromothymol, phenolphthalein) \tn 
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Hydrolysis of salt & a reaction in which one of the salt's ions reacts with water to produce an acidic or basic solution \tn 
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Buffer Solution & a solution that resists a change in its PH \tn 
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Buffer capacity & the amount of acid or base that can be added without a significant change in PH \tn 
% Row Count 22 (+ 4)
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% That's all folks
\end{multicols*}

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