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CHE 2A Study Guide - Sodium Nitrite, Sodium Nitrate, Nitrous Acid

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UC-Davis
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Chemistry
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CHE 2A
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A N D R E A S T O U P A D A K I S

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CHE 2A Full Course Notes
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Related Questions

What is the pH of a solution made by dissolving 4.3 g of K2CO3 and 1.6 g of KHCO3 in 500. mL of water? (See the appendix.)

Table 3 An Acid-base table
Acid Name ConjugateAcid Ka pKa Conjugate Base Base Name
perchloric acid HClO4 >>1 < 0 ClO41- perchlorate ion
hydrohalic acid HX (X=I,Br,Cl) >>1 < 0 X1- halide ion
sulfuric acid H2SO4 >>1 < 0 HSO41- hydrogen sulfate ion
nitric acid HNO3 >>1 < 0 NO31- nitrate ion
hydronium ion H3O1+ 1.0 0.00 H2O water
iodic acid HIO3 0.17 0.77 IO31- iodate ion
oxalic acid H2C2O4 5.9 x 10-2 1.23 HC2O41- hydrogen oxalate ion
sulfurous acid H2SO3 1.5 x 10-2 1.82 HSO31- hydrogen sulfite ion
hydrogen sulfate ion HSO41- 1.2 x 10-2 1.92 SO42- sulfate ion
phosphoric acid H3PO4 7.5 x 10-3 2.12 H2PO41- dihydrogen phosphate ion
hydrofluoric acid HF 7.2 x 10-4 3.14 F1- fluoride ion
nitrous acid HNO2 4.0 x 10-4 3.40 NO21- nitrite ion
lactic acid HC3H5O3 6.4 x 10-5 3.85 C3H5O31- lactate ion
formic acid HCHO2 1.8 x 10-4 3.74 CHO21- formate ion
hydrogen oxalate ion HC2O41- 6.4 x 10-5 4.19 C2O42- oxalate ion
hydrazoic acid HN3 1.9 x 10-5 4.72 N31- azide ion
acetic acid HC2H3O2 1.8 x 10-5 4.74 C2H3O21- acetate ion
carbonic acid H2CO3 4.3 x 10-7 6.37 HCO31- hydrogen carbonate ion
hydrogen sulfite ion HSO31- 1.0 x 10-7 7.00 SO32- sulfite ion
hydrosulfuric acid H2S 1.0 x 10-7 7.00 HS1- hydrogen sulfide ion
dihydrogen phosphate ion H2PO41- 6.2 x 10-8 7.21 HPO42- hydrogen phosphate ion
hypochlorous acid HClO 3.5 x 10-8 7.46 ClO1- hypochlorite ion
ammonium ion NH41+ 5.6 x 10-10 9.25 NH3 ammonia
hydrocyanic acid HCN 4.0 x 10-10 9.40 CN1- cyanide ion
hydrogen carbonate ion HCO31- 4.7 x 10-11 10.33 CO32- carbonate ion
hydrogen phosphate ion HPO42- 4.8 x 10-13 12.32 PO43- phosphate ion
hydrogen sulfide ion HS1- 1.3 x 10-13 12.89 S2- sulfide ion
water H2O 1.0 x 10-14 14.00 OH1- hydroxide ion
ammonia NH3 <<10-14 NH21- amide ion
hydroxide ion OH1- <<10-14 O2- oxide ion

Calculate the pH change that results when 12 mL of 5.9 M NaOH is added to 763 mL of each the following solutions. (See the appendix.)

(a) pure water


(b) 0.10 M NH4Cl


(c) 0.10 M NH3


(d) a solution that is 0.10 M in each NH4+ and NH3

Acid Name ConjugateAcid Ka pKa Conjugate Base Base Name
perchloric acid HClO4 >>1 < 0 ClO41- perchlorate ion
hydrohalic acid HX (X=I,Br,Cl) >>1 < 0 X1- halide ion
sulfuric acid H2SO4 >>1 < 0 HSO41- hydrogen sulfate ion
nitric acid HNO3 >>1 < 0 NO31- nitrate ion
hydronium ion H3O1+ 1.0 0.00 H2O water
iodic acid HIO3 0.17 0.77 IO31- iodate ion
oxalic acid H2C2O4 5.9 x 10-2 1.23 HC2O41- hydrogen oxalate ion
sulfurous acid H2SO3 1.5 x 10-2 1.82 HSO31- hydrogen sulfite ion
hydrogen sulfate ion HSO41- 1.2 x 10-2 1.92 SO42- sulfate ion
phosphoric acid H3PO4 7.5 x 10-3 2.12 H2PO41- dihydrogen phosphate ion
hydrofluoric acid HF 7.2 x 10-4 3.14 F1- fluoride ion
nitrous acid HNO2 4.0 x 10-4 3.40 NO21- nitrite ion
lactic acid HC3H5O3 6.4 x 10-5 3.85 C3H5O31- lactate ion
formic acid HCHO2 1.8 x 10-4 3.74 CHO21- formate ion
hydrogen oxalate ion HC2O41- 6.4 x 10-5 4.19 C2O42- oxalate ion
hydrazoic acid HN3 1.9 x 10-5 4.72 N31- azide ion
acetic acid HC2H3O2 1.8 x 10-5 4.74 C2H3O21- acetate ion
carbonic acid H2CO3 4.3 x 10-7 6.37 HCO31- hydrogen carbonate ion
hydrogen sulfite ion HSO31- 1.0 x 10-7 7.00 SO32- sulfite ion
hydrosulfuric acid H2S 1.0 x 10-7 7.00 HS1- hydrogen sulfide ion
dihydrogen phosphate ion H2PO41- 6.2 x 10-8 7.21 HPO42- hydrogen phosphate ion
hypochlorous acid HClO 3.5 x 10-8 7.46 ClO1- hypochlorite ion
ammonium ion NH41+ 5.6 x 10-10 9.25 NH3 ammonia
hydrocyanic acid HCN 4.0 x 10-10 9.40 CN1- cyanide ion
hydrogen carbonate ion HCO31- 4.7 x 10-11 10.33 CO32- carbonate ion
hydrogen phosphate ion HPO42- 4.8 x 10-13 12.32 PO43- phosphate ion
hydrogen sulfide ion HS1- 1.3 x 10-13 12.89 S2- sulfide ion
water H2O 1.0 x 10-14 14.00 OH1- hydroxide ion
ammonia NH3 <<10-14 NH21- amide ion
hydroxide ion OH1- <<10-14 O2- oxide ion

Calculate the pH change that results when 12 mL of 5.9 M NaOH is added to 753 mL of each the following solutions. (See the appendix.)

A) 0.10 M NH4Cl


B) 0.10 M NH3


Acid Name ConjugateAcid Ka pKa Conjugate Base Base Name
perchloric acid HClO4 >>1 < 0 ClO41- perchlorate ion
hydrohalic acid HX (X=I,Br,Cl) >>1 < 0 X1- halide ion
sulfuric acid H2SO4 >>1 < 0 HSO41- hydrogen sulfate ion
nitric acid HNO3 >>1 < 0 NO31- nitrate ion
hydronium ion H3O1+ 1.0 0.00 H2O water
iodic acid HIO3 0.17 0.77 IO31- iodate ion
oxalic acid H2C2O4 5.9 x 10-2 1.23 HC2O41- hydrogen oxalate ion
sulfurous acid H2SO3 1.5 x 10-2 1.82 HSO31- hydrogen sulfite ion
hydrogen sulfate ion HSO41- 1.2 x 10-2 1.92 SO42- sulfate ion
phosphoric acid H3PO4 7.5 x 10-3 2.12 H2PO41- dihydrogen phosphate ion
hydrofluoric acid HF 7.2 x 10-4 3.14 F1- fluoride ion
nitrous acid HNO2 4.0 x 10-4 3.40 NO21- nitrite ion
lactic acid HC3H5O3 6.4 x 10-5 3.85 C3H5O31- lactate ion
formic acid HCHO2 1.8 x 10-4 3.74 CHO21- formate ion
hydrogen oxalate ion HC2O41- 6.4 x 10-5 4.19 C2O42- oxalate ion
hydrazoic acid HN3 1.9 x 10-5 4.72 N31- azide ion
acetic acid HC2H3O2 1.8 x 10-5 4.74 C2H3O21- acetate ion
carbonic acid H2CO3 4.3 x 10-7 6.37 HCO31- hydrogen carbonate ion
hydrogen sulfite ion HSO31- 1.0 x 10-7 7.00 SO32- sulfite ion
hydrosulfuric acid H2S 1.0 x 10-7 7.00 HS1- hydrogen sulfide ion
dihydrogen phosphate ion H2PO41- 6.2 x 10-8 7.21 HPO42- hydrogen phosphate ion
hypochlorous acid HClO 3.5 x 10-8 7.46 ClO1- hypochlorite ion
ammonium ion NH41+ 5.6 x 10-10 9.25 NH3 ammonia
hydrocyanic acid HCN 4.0 x 10-10 9.40 CN1- cyanide ion
hydrogen carbonate ion HCO31- 4.7 x 10-11 10.33 CO32- carbonate ion
hydrogen phosphate ion HPO42- 4.8 x 10-13 12.32 PO43- phosphate ion
hydrogen sulfide ion HS1- 1.3 x 10-13 12.89 S2- sulfide ion
water H2O 1.0 x 10-14 14.00 OH1- hydroxide ion
ammonia NH3 <<10-14 NH21- amide ion
hydroxide ion OH1- <<10-14 O2- oxide ion