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

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periwinklelouse135

24 Jan 2014

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UC-Davis

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Chemistry

Course

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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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	K_a	pK_a	Conjugate Base	Base Name
perchloric acid	HClO₄	>>1	< 0	ClO₄^1-	perchlorate ion
hydrohalic acid	HX (X=I,Br,Cl)	>>1	< 0	X^1-	halide ion
sulfuric acid	H₂SO₄	>>1	< 0	HSO₄^1-	hydrogen sulfate ion
nitric acid	HNO₃	>>1	< 0	NO₃^1-	nitrate ion

hydronium ion	H₃O¹⁺	1.0	0.00	H₂O	water
iodic acid	HIO₃	0.17	0.77	IO₃^1-	iodate ion
oxalic acid	H₂C₂O₄	5.9 x 10^-2	1.23	HC₂O₄^1-	hydrogen oxalate ion
sulfurous acid	H₂SO₃	1.5 x 10^-2	1.82	HSO₃^1-	hydrogen sulfite ion
hydrogen sulfate ion	HSO₄^1-	1.2 x 10^-2	1.92	SO₄^2-	sulfate ion
phosphoric acid	H₃PO₄	7.5 x 10^-3	2.12	H₂PO₄^1-	dihydrogen phosphate ion
hydrofluoric acid	HF	7.2 x 10^-4	3.14	F^1-	fluoride ion
nitrous acid	HNO₂	4.0 x 10^-4	3.40	NO₂^1-	nitrite ion
lactic acid	HC₃H₅O₃	6.4 x 10^-5	3.85	C₃H₅O₃^1-	lactate ion
formic acid	HCHO₂	1.8 x 10^-4	3.74	CHO₂^1-	formate ion
hydrogen oxalate ion	HC₂O₄^1-	6.4 x 10^-5	4.19	C₂O₄^2-	oxalate ion
hydrazoic acid	HN₃	1.9 x 10^-5	4.72	N₃^1-	azide ion
acetic acid	HC₂H₃O₂	1.8 x 10^-5	4.74	C₂H₃O₂^1-	acetate ion
carbonic acid	H₂CO₃	4.3 x 10^-7	6.37	HCO₃^1-	hydrogen carbonate ion
hydrogen sulfite ion	HSO₃^1-	1.0 x 10^-7	7.00	SO₃^2-	sulfite ion
hydrosulfuric acid	H₂S	1.0 x 10^-7	7.00	HS^1-	hydrogen sulfide ion
dihydrogen phosphate ion	H₂PO₄^1-	6.2 x 10^-8	7.21	HPO₄^2-	hydrogen phosphate ion
hypochlorous acid	HClO	3.5 x 10^-8	7.46	ClO^1-	hypochlorite ion
ammonium ion	NH₄¹⁺	5.6 x 10^-10	9.25	NH₃	ammonia
hydrocyanic acid	HCN	4.0 x 10^-10	9.40	CN^1-	cyanide ion
hydrogen carbonate ion	HCO₃^1-	4.7 x 10^-11	10.33	CO₃^2-	carbonate ion
hydrogen phosphate ion	HPO₄^2-	4.8 x 10^-13	12.32	PO₄^3-	phosphate ion
hydrogen sulfide ion	HS^1-	1.3 x 10^-13	12.89	S^2-	sulfide ion
water	H₂O	1.0 x 10^-14	14.00	OH^1-	hydroxide ion

ammonia	NH₃	<<10^-14		NH₂^1-	amide ion
hydroxide ion	OH^1-	<<10^-14		O^2-	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	K_a	pK_a	Conjugate Base	Base Name
perchloric acid	HClO₄	>>1	< 0	ClO₄^1-	perchlorate ion
hydrohalic acid	HX (X=I,Br,Cl)	>>1	< 0	X^1-	halide ion
sulfuric acid	H₂SO₄	>>1	< 0	HSO₄^1-	hydrogen sulfate ion
nitric acid	HNO₃	>>1	< 0	NO₃^1-	nitrate ion

hydronium ion	H₃O¹⁺	1.0	0.00	H₂O	water
iodic acid	HIO₃	0.17	0.77	IO₃^1-	iodate ion
oxalic acid	H₂C₂O₄	5.9 x 10^-2	1.23	HC₂O₄^1-	hydrogen oxalate ion
sulfurous acid	H₂SO₃	1.5 x 10^-2	1.82	HSO₃^1-	hydrogen sulfite ion
hydrogen sulfate ion	HSO₄^1-	1.2 x 10^-2	1.92	SO₄^2-	sulfate ion
phosphoric acid	H₃PO₄	7.5 x 10^-3	2.12	H₂PO₄^1-	dihydrogen phosphate ion
hydrofluoric acid	HF	7.2 x 10^-4	3.14	F^1-	fluoride ion
nitrous acid	HNO₂	4.0 x 10^-4	3.40	NO₂^1-	nitrite ion
lactic acid	HC₃H₅O₃	6.4 x 10^-5	3.85	C₃H₅O₃^1-	lactate ion
formic acid	HCHO₂	1.8 x 10^-4	3.74	CHO₂^1-	formate ion
hydrogen oxalate ion	HC₂O₄^1-	6.4 x 10^-5	4.19	C₂O₄^2-	oxalate ion
hydrazoic acid	HN₃	1.9 x 10^-5	4.72	N₃^1-	azide ion
acetic acid	HC₂H₃O₂	1.8 x 10^-5	4.74	C₂H₃O₂^1-	acetate ion
carbonic acid	H₂CO₃	4.3 x 10^-7	6.37	HCO₃^1-	hydrogen carbonate ion
hydrogen sulfite ion	HSO₃^1-	1.0 x 10^-7	7.00	SO₃^2-	sulfite ion
hydrosulfuric acid	H₂S	1.0 x 10^-7	7.00	HS^1-	hydrogen sulfide ion
dihydrogen phosphate ion	H₂PO₄^1-	6.2 x 10^-8	7.21	HPO₄^2-	hydrogen phosphate ion
hypochlorous acid	HClO	3.5 x 10^-8	7.46	ClO^1-	hypochlorite ion
ammonium ion	NH₄¹⁺	5.6 x 10^-10	9.25	NH₃	ammonia
hydrocyanic acid	HCN	4.0 x 10^-10	9.40	CN^1-	cyanide ion
hydrogen carbonate ion	HCO₃^1-	4.7 x 10^-11	10.33	CO₃^2-	carbonate ion
hydrogen phosphate ion	HPO₄^2-	4.8 x 10^-13	12.32	PO₄^3-	phosphate ion
hydrogen sulfide ion	HS^1-	1.3 x 10^-13	12.89	S^2-	sulfide ion
water	H₂O	1.0 x 10^-14	14.00	OH^1-	hydroxide ion

ammonia	NH₃	<<10^-14		NH₂^1-	amide ion
hydroxide ion	OH^1-	<<10^-14		O^2-	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	K_a	pK_a	Conjugate Base	Base Name
perchloric acid	HClO₄	>>1	< 0	ClO₄^1-	perchlorate ion
hydrohalic acid	HX (X=I,Br,Cl)	>>1	< 0	X^1-	halide ion
sulfuric acid	H₂SO₄	>>1	< 0	HSO₄^1-	hydrogen sulfate ion
nitric acid	HNO₃	>>1	< 0	NO₃^1-	nitrate ion

hydronium ion	H₃O¹⁺	1.0	0.00	H₂O	water
iodic acid	HIO₃	0.17	0.77	IO₃^1-	iodate ion
oxalic acid	H₂C₂O₄	5.9 x 10^-2	1.23	HC₂O₄^1-	hydrogen oxalate ion
sulfurous acid	H₂SO₃	1.5 x 10^-2	1.82	HSO₃^1-	hydrogen sulfite ion
hydrogen sulfate ion	HSO₄^1-	1.2 x 10^-2	1.92	SO₄^2-	sulfate ion
phosphoric acid	H₃PO₄	7.5 x 10^-3	2.12	H₂PO₄^1-	dihydrogen phosphate ion
hydrofluoric acid	HF	7.2 x 10^-4	3.14	F^1-	fluoride ion
nitrous acid	HNO₂	4.0 x 10^-4	3.40	NO₂^1-	nitrite ion
lactic acid	HC₃H₅O₃	6.4 x 10^-5	3.85	C₃H₅O₃^1-	lactate ion
formic acid	HCHO₂	1.8 x 10^-4	3.74	CHO₂^1-	formate ion
hydrogen oxalate ion	HC₂O₄^1-	6.4 x 10^-5	4.19	C₂O₄^2-	oxalate ion
hydrazoic acid	HN₃	1.9 x 10^-5	4.72	N₃^1-	azide ion
acetic acid	HC₂H₃O₂	1.8 x 10^-5	4.74	C₂H₃O₂^1-	acetate ion
carbonic acid	H₂CO₃	4.3 x 10^-7	6.37	HCO₃^1-	hydrogen carbonate ion
hydrogen sulfite ion	HSO₃^1-	1.0 x 10^-7	7.00	SO₃^2-	sulfite ion
hydrosulfuric acid	H₂S	1.0 x 10^-7	7.00	HS^1-	hydrogen sulfide ion
dihydrogen phosphate ion	H₂PO₄^1-	6.2 x 10^-8	7.21	HPO₄^2-	hydrogen phosphate ion
hypochlorous acid	HClO	3.5 x 10^-8	7.46	ClO^1-	hypochlorite ion
ammonium ion	NH₄¹⁺	5.6 x 10^-10	9.25	NH₃	ammonia
hydrocyanic acid	HCN	4.0 x 10^-10	9.40	CN^1-	cyanide ion
hydrogen carbonate ion	HCO₃^1-	4.7 x 10^-11	10.33	CO₃^2-	carbonate ion
hydrogen phosphate ion	HPO₄^2-	4.8 x 10^-13	12.32	PO₄^3-	phosphate ion
hydrogen sulfide ion	HS^1-	1.3 x 10^-13	12.89	S^2-	sulfide ion
water	H₂O	1.0 x 10^-14	14.00	OH^1-	hydroxide ion

ammonia	NH₃	<<10^-14		NH₂^1-	amide ion
hydroxide ion	OH^1-	<<10^-14		O^2-	oxide ion

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

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