04_Acid Base Chemistry - A. CH3OH(aq) B. NaOH(aq) C....

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A. CH 3 OH(aq) B. NaOH(aq) C. CH 3 COOH(aq) D. Cannot determine from Figure 4.2
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A. Ag + (aq) and Cl - (aq) B. NO 3 - (aq) and Cl - (aq) C. Na + (aq) and NO 3 - (aq) D. No spectator ions are involved
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Acids The Swedish physicist and chemist S. A. Arrhenius defined acids as substances that increase the concentration of H + when dissolved in water. Both the Danish chemist J. N. Brønsted and the British chemist T. M. Lowry defined them as proton donors.
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Acids There are only seven strong acids: Hydrochloric (HCl) Hydrobromic (HBr) Hydroiodic (HI) • Nitric (HNO 3 ) • Sulfuric (H 2 SO 4 ) • Chloric (HClO 3 ) • Perchloric (HClO 4 )
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Acids HX, HY, and HZ are put in water (illustrated). Which is the strong acid?
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Bases Arrhenius defined bases as substances that increase the concentration of OH when dissolved in water. Brønsted and Lowry defined them as proton acceptors.
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Bases The strong bases are the soluble metal salts of hydroxide ion: Alkali metals Calcium Strontium Barium
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Acid-Base Reactions In an acid–base reaction, the acid donates a proton (H + ) to the base.
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04_Acid Base Chemistry - A. CH3OH(aq) B. NaOH(aq) C....

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