More reaction types. combustions and acid/base neutralizations

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1 More reaction types combustions and acid/base neutralizations

2 Combustion reactions C x H y + O 2(g) CO 2(g) + H 2 O (l) + E If the hydrocarbon contains nitrogen as well C x H y N z + O 2(g) CO 2(g) + H 2 O (l) + N 2(g)

3 Acid/Base Neutralization Hydroxide base general form Acid + Base Salt + H 2 O what s actually happening? H + + OH - H 2 O Salt = the anion from the acid + the cation from the base

4 Predicting results Acid + hydroxide base Example: NaOH + HCl 1. Write H 2 O as a product NaOH + HCl H 2 O

5 Predicting results Acid + hydroxide base Example: NaOH + HCl 2. Form the salt from the remainders of the acid and base NaOH + HCl H 2 O + Na + Cl -

6 Predicting results Acid + hydroxide base Example: NaOH + HCl 3. Balance the charges in the salt NaOH + HCl H 2 O + NaCl 4. Balance the equation NaOH + HCl H 2 O + NaCl

7 Predicting results Acid + hydroxide base Example: H 2 SO 4 + Al(OH) 3 1. Write H 2 O as a product H 2 SO 4 + Al(OH) 3 H 2 O

8 Predicting results Acid + hydroxide base Example: H 2 SO 4 + Al(OH) 3 2. Form the salt from the remainders of the acid and base H 2 SO 4 + Al(OH) 3 H 2 O + Al 3+ SO 4 2-

9 Predicting results Acid + hydroxide base Example: H 2 SO 4 + Al(OH) 3 3. Balance the charges in the salt H 2 SO 4 + Al(OH) 3 H 2 O + Al 2 (SO 4 ) 3 4. Balance the equation 3H 2 SO 4 + 2Al(OH) 3 Al 2 (SO 4 ) 3 + 6H 2 O

10 Acid/Base Neutralization carbonate base general form Acid + Base (CO 3 2- or HCO 3- ) Salt + H 2 O + CO 2 what s actually happening? 2H + + CO 3 2- H 2 CO 3 H 2 CO 3 H 2 O + CO 2 Salt = the anion from the acid + the cation from the base

11 Predicting results Acid + carbonate base Example: CaCO 3 + HCl 1. Write H 2 O + CO 2 as products CaCO 3 + HCl H 2 O + CO 2

12 Predicting results Acid + carbonate base Example: CaCO 3 + HCl 2. Form the salt from the remainders of the acid and base CaCO 3 + HCl H 2 O + CO 2 + Ca 2+ Cl -

13 Predicting results Acid + carbonate base Example: CaCO 3 + HCl 3. Balance the charges in the salt CaCO 3 + HCl H 2 O + CO 2 + CaCl 2 4. Balance the equation CaCO HCl H 2 O + CO 2 + CaCl 2

14 Predicting results Acid + carbonate base Example: H 2 SO 4 + NaHCO 3 1. Write H 2 O + CO 2 as products H 2 SO 4 + NaHCO 3 H 2 O + CO 2

15 Predicting results Acid + carbonate base Example: H 2 SO 4 + NaHCO 3 2. Form the salt from the remainders of the acid and base H 2 SO 4 + NaHCO 3 H 2 O + CO 2 + Na + SO 2-4

16 Predicting results Acid + carbonate base Example: H 2 SO 4 + NaHCO 3 3. Balance the charges in the salt H 2 SO 4 + NaHCO 3 H 2 O + CO 2 + Na 2 SO 4 4. Balance the equation H 2 SO NaHCO 3 2 H 2 O + 2 CO 2 + Na 2 SO 4

17 What reaction would be the best choice to make

18 An insoluble ionic compound? Double replacement But remember Both reactants must be aqueous solutions You CANNOT use an insoluble compound as a reactant The other product MUST be soluble

19 A soluble ionic compound? Double Replacement IF The other product is insoluble Acid/Base Neutralization But remember the reactants must be an acid and a base The other product must be water or water and CO 2

20 A free element? Single Replacement But remember the element must start as part of the compound in the reactants the reactant free element must be able to replace the desired element out of the compound Watch out for metals that react with water

21 H 2 gas? Single replacement IF the free element metal reacts with water or an acid M + HX H 2 + MX M + H 2 O H 2 + MOH

22 Water? Combustion IF You have a hydrocarbon to burn Acid/Base Neutralization But remember the reactants must be an acid and a base The other product must be a salt (and maybe CO 2 if the base is a carbonate)

23 Combustion CO 2 gas? IF You have a hydrocarbon to burn Acid/Base Neutralization But remember the reactant base must be a carbonate or bicarbonate

(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion

AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single