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Le; cartes, planches, tableaux, etc., peuvent §tre film6s d des taux de reduction diffdrents. Lorsque le document est trop grand pour Stre reproduit en un seul clif ;i6, il est film6 d partir de I'angle sup6rieur gauche, de gauche d droite, et de haut en bas, en prenant le nombre d'images n^cessaire. Les diagrammes suivants illustrent la mdthode. 1 ■ m^ * ' ^ PRICE 90 CENTS, TABLES won SIMPLE QUALITATIVE ANALYSIS, BY H. H. CROFT. TORONTO- COPP, CLARK & CO., 47 FRONT STREET EAST. 187 4. ) ■■X V. TABLES / POR SIMPLE QUALITATIVE ANALYSIS FOR LABOEATOEY USE. The following tables ; :q intended for practice in clomcntary chemical analysis, and to ajiply only to sini})le salts, consisting of one base and one acid, mostly soluble in water, ox* of the acids and bases uncombined. Many bases (oxides) ai'e insoluble in water, but can be readily dissolved in nitric or hydi-ochloric acid ; some few acids are insoluble in water, Ijut can be dissolved in potassium hydrate. Some salts are decomposed by water, but solutions can be obtained by adding a little nitric acid, and heating ; as little acid should be used as possible. Many salts which ai-e insoluble in Avatei-, such as many carbonates, phosi»hates, itc, may Ijc dissolved in the same way, using either nitric or hydrochloric acid, and the solutions can in most cases be examined in the ordinary manner. In examining a salt, about one-third should be dissolved in a small (piantity of water, and the test tulie containing the solution jjlaced always in one particular part of the stand, say the left hand upper hole. A small part of this can be diluted with two or three parts of water in another test tube, and the ex})eriTuents proceeded with. The sa7ne solution can be used for the tirst three groujjs of Table I. Thus if hydrochloric acid produces no change, pass to Gi'ouj) II., adding three times the bulk of hydrosulphuric acid ; if this produces no change, pass to Group III., adding first twice the bulk (of the original solution) of ammonium chloride, then ammonia until it smells strongly after shaking, and, lastly, a small quantity of ammo- Jiium sulphide, whether any change has been produced by the am- monia or not. /^ 6H^ The same solution may be used for Group IV. if the salt does not belong to either of the first three, but it is preferable now to employ some of the original solution. It may happen that no Ijase whatevei- is found, as would be the case in the examination of acids, and 'dee versd, no acid if the substance is a base. In the case of no metal being found, the base is in all probability hydrogen, which takes the place of true metals hi salts, producing acids. When in the investi gation for acids none have been found, the compound under exami- nation is probably a hydrate, i.e. a combination of an oxide with water. Arsenic is coixveniently ranked under both heads. It is best to commence with the detection of the base, aa this knowledge obvintcs the necessity of searching for many acids, if the substance examined has been found to be soluble in water. Thus lead in an easily soluble salt would exclude hydrochloric, hydriodic, hydrobromie, carbonic, phosphoric, sulphuric acids, &c., &c. Barium would exclude sulphuric, carbonic, phosplioric acids, &.C., ikc, but not hydrochloric, hydriodic, or hydrobromie acids, etc. A knowledge of the solubilities of salts will greatly aid the investi- gation. ^^^^i>y , 3 J ^ L- GROUP I, The white i)recipitate is allowed to settle, the liquid poured off, washed with water by decantation, and ammonia added. Precipitate dlsaolves. Silver. Original sohition jjives a crimson precipitate with potassium chro- mate. Solution of ferrous sul- phate produces a grey- ish precipitate of metal- lic silvei. Turns bliick or grey. Mercury. Solutions produce a grey stain on copper or gold, which volatihses on heating. The salts are volatile. The white precipitate formed hy hydrochloric acid, when boiled with excess of the same, turns greyiah. neinaics almost unchanged. Lead. The original white preci- pitate formed by hyilro- chloric acid is soluble in a large quantity of boiling water. To try this, most of the ])recipitate should be Eoured off, and the residue oiled with much water. The original solution gives a yellow precipitate with potassium chromate, soluble m large excess of potassium hydrate. Only a small quan- tity of the yellow precipi- tate should be employed. ^ ^ -^ -O -u rr —4 ?t t~t :J z -M f.. X ^^ >. +-1 :3 '— « 0) 3 '^ -=3 1^ -^ a, (^ 7; t: ^ ill o P S 13 S.'^ •*J -> CT O ^.2 8 O) +3 t< ^ S .. >- CO > ^-tJ p * >H l-M -a ^ 5 +j *^ M 5tr -ij • w ;h rs u P t^ ^■*" Jfl •F-t 3 i-H 1 • 1— ( C ^ c ^ ^ ^ ^ -fi +3 •V .S Ci 0" 2 ^ •fH a -2 3 3 •^ -^ •fH ^ 0^ _5 s ■J ci «*» s 3 o ^ 5 2 ** "S '3 i H .3: fa 03 I +3 c3 3^ O i "3 3 *'= O > c3 — ' X ^ ■&■« 3 ^ rt 8 a c4 S3 to C G to : Oh O _ o 3 ^ _ ^ o u - -J "-< CO ^ ■ 3 '-5 _2 surd.i J 3 i^ -r" o c3 a o r -^ G-^ s to 3 cj rt ^-'t; ^ r* ** ii •■) •"'^ tfyr c a J5 2 5 Ci a 33 s d 3 g 0.5 rr^ n f^ 1-* d rf Td 5 -r CO i2 1 .a vri e CO ►-.2 2 =^ o o o 2-§ V o tJO c • c ^ o I Cf.' t^ 'f/3 ? c6 73 1 rt ?■ -4^ -^ P_ « -:-l 2 a r} (U -t-> rt o a OJ J3 n m 00 ^ •r-l +3 CD rt •t-> ;:J .& " 'o ':; aj .3 (u ^a OS o Q 03 o •a a o '■+3 "o •a 03 ^ 2 « a •c ^ 'J 6 -=? - o s -5 - x-r o P P< 4) ? rt o o .s « .S c3 o o 3 ~ ? -co C P4 O to c ^ c3 i^.S^ O X (-, 3 H m C O ^ ^ > ^ O rt nCl a i-O ^ -^ M 1^1 §^ 1 1 ? K o .t: ■= H - c C3 n to 4) a e ■|.: 1 ; i' t rt S ^ CO cs ;s - . n3 o a) 42 rS -3 rr- u o r ~,-^^ .« ft o rC) u ? rt a) O c3 CO to p 3 o u C I, s| CO i a -J5 O I— I 03 13 O a s ,4 ■3 » n CO V rt <0 ' • c ej C ■ ^ S a) 'Ed _ .tr cS i) c 3 a ^-^ r-i n rC . -(J c'e; rt ^ c > -M u -3^ 3 X C c3 ca -fj ft n to . I p'^ _ =^ =5 r»4 a W t> — 3 § ^. 'sis "*^ "r ."S .3 «'^ Coo £ fH I— I d o c4 O p^ •s a o -^ =• 5s O to 02 ci a •- rd fl O CO 0) •al O eS d r^ -d c ,d . C '"^ .^ ■"^ =^ c8 .art 'ft to d '3^ .rH to ^ .^ 0) y .^ i) 5; X d s; ft Q) CO ft S 4) ' a 'ft -5 d' "■^ g r^ Cj cS -w d o ^ is -M if tOpi! rt CO j; -rj j; t. o X y d «-2- ^ o Ph t rt O O O " d rt o 4 +3 ^ -« CO •d ^ +2 -^ is 'd.2'5 ;3h5 CO '=': i^.g "x d-^ .S oj li- m Pho d ^ts fS S:^ S frj -« ^ d ^•3 d y to -c •a o o CO ^ to (1) to o 0) d.S^ ■^ y ' « g d ^. •Co, O >. c« >-l 4) w "0 £c a a 3 d 3 »j «; CO r/) c« d ^ ^ o M O ID 4^ 41 d .2 d- I- 0) o •S -|J -fH ^ .^ ft 3 'u "3 p— t o 3 C t, CO CO p. •c£ . o « ^;^^ 3 c3 -IJ • I— ( ft CO .tr* to _, . ft eS II Oh O 0^ o u CO O 05 ♦J 03 cS w. EC n 55 i 2 ^ m « rt "^ Q S3 rS -^ t^ -M -s V-> 0) CO -:; O '■^ +i 1-^i^ •~^. ^^ o — & o H 1—1 "rt 0) ^ T) »— ( 3 O m s i • I-* o C/2 1— H p-' ^ M a; ^ r-2 O -^ ci • fH « 2 rt 2 o F— H f- H o -5 < ^ ^ , a a; o , 0) o O '•■3 ^ ■4J 0) pi +3 rt fl> -M > o •;3 S S -^ •r -S ^ ■=! il « J2 >» :j u rt •^) Ctf ^ ^? 43 '>_' c; tn o -5 2 S jT ^ '^ r3 tH -is 3 OJ 3 5 S H J M !h i-< o C3 »< -J i .2 « -c :S 4-" -tJ on 01 o aj OS S o o En S O i-H O 2 -S « .s o 9^ 5 o ■r o I- C 4^ - ^ c •-. !ri o H ~ i; 'Eb rt c; u cs cr « II 2 e X o ftcs.a w !=0 C -M C rt 32 ^^ ft c Si rt a) .— < 03 (D ft ft « S .g 3 a a •a .a & I O :i 01 o .2 .1 'S c hi s Q a tic a = ■3 2 - JJ I, '/: -t- ^ , itM — y; "^ ^ S 3 " •- s § ■S 2 o-^ =^ a- 2 " rS ac =^ j: o a 5 -3 8 GROUP IV If the ftolutiou employcil in tho previous group tests is employed, that is, if salts of aiumouia are present, it may be better to warm t,"^ntly. With original solution this is not necessary. Tin; original solution, mixed with a large quantity of aninioniuni chloride and a modorat* quantity of annnoniuni carbonate, gives A white precipitate. Original Bolution gives, with calcium sulphate. A precipitate lit A precipitate once. after some tiuie. The salt coloura Tlio salt c(ilour,'=i the llanie of alco- the ilaiue of alco- hol — green. hoi — crimson. Barium. Strontium. No precipitate. The addition of — — sodium phosphate No precipitate, produceaapreeipi- tate, crystalline when from dilute The salt colours solutions, the llame of alco- hol — ^^orange red. Calcium. Magnesium. GROUP V Original solution, rather eoncantrated, and acidulated with hydrochloric acid, gives, with platinum tetrachloride, A yellow precipitate. No precipitate. Dry salt, heated with Dry salt, heated witli Salts colour the potassium hydrate, evolves potassium hydrate, evolves flame of alcohol — no ammonia. ammonia. yellow. Dry salt coloura the Salts are volatile, and flame of alcohol— violet. do not colour the flame of alcohol. Potassium. Ammonium. Sodium. If no metal is found, the substance is probably an acid, and the base hydrogen. 9 Notes on tfik tai'.f.es foij acids. Fivr. .ouh nvxy bo uontralisod mth potasHiuni l.vdnite, tin- ...lu- tion evaiMuat,.,! to (Iryi.e.'s, rni.l ;, salt tluis ol.tui.uxl. This is not always noeo.siiry, l.ut is ivqiiircl if tJio tost of Mackcning by heiit is to ]>o tnnl. To aA-oi(l ll.is trouble, u socoixl urrangeiuent for acids i^ appoiulcd ill Table 111. Acid salt, may be n-iderod neutral by adding a little ammonia tdl solution ,.s alkaline; and by Jieatiug, any excess of anunonia may bo removed. Silicic acid, being iusoluldo in water, and all acids except hydro- fluoric, mnst bo dissoh-cnl by boiling in sodium hydrate o.- carbonate The sodium compounds are preferable to thoae of potassium, a.s th- latter generally contain silicic acid. In testing f,y tartaric and citric acids bv means of lime water a very Lirgo quantity of the latter must be used, especially if it is the free acid und.T examination. The limo water must be added till an alkaline I'eaction is produced. Befuiv, testing a salt, it should bo tried as to its neutrality or' acidity by means of litmus paper. _ Some acid salts can be neutralised by ammonia without any preci- pitate being formed ; but some metallic oxides cannot form salt« neutral to test paper, and in these the smallest quantity of ammonia may produce a precipitate. _ In some cases, barium nitrate must be used inste=id of the chlo- ride ;^ as lead, fjilvcr, and mercurous salts would give precipitates of chlorides. hi all eases of testing for bases or acids, p.ftcr the application of the tests contained in the group f.bles, tlie .tudent should make a number of coniirmatory experiments witli otlier re-a■ •C to _j, i) i) — e 'P Z — 5 i' S •* 1-' H 73 _; +J w fs 3 -'a a = .9 s -?^ :- c o s ,7.^ b I C '-J Tt ■ '-J >- CO >■-; y cj :3 - I- '■3 CO a; '^ ^ ~ r— K^ ■ti rt D »^ rt Si c -p *— 4 «-* « r; 0) 0) «- > r— W! ^"■t »H O S +3 l; ^ _ '3 -^^ -C rt .-— 1 r* p > o '-1 cS o i—i " o ii 5 ,-r rt io: 0) H to i> ^ V2 U « 9) — _J <«-l ■r -> f !*• = — S V H -^ rt rt ^^ . i) t. — ^ V3 ^ P_-4 •;■< 4J , >• V -^ fl-= =:■ » .2 :; 2 rti: 3 ? o '->^ b ^"" f 3 E ~ '^tJ ?■ ■/: 3 3 cS v: 3 ^ iJ eS M a: rt O To* '4j rt 5'^ 3 -3 ■« -1 -• 3 i^ ■* _ ** *> = -S 3 .i a 'J a rt :.3 C 5) w ■'-'3 » 3 .H a t, i O 3 OT W - H 5 2-M rt ■g o 3 m - s -J ■S.tJ r-- O rt -rH 2.£" 3 ^ 72 --5 rt 53 rt -pt to > - ^ >^ 3 «^ 3 OJ I— I O ^^ rt •d3 rt ;3 Q Tc o rt o •c 3 -.1 '^ to Q 1) rt rt Tn rt .3 i -3^ rt -iJ T* • I— ( ""^ ^^ D — o a -^ v^ >:Jd ^3 li "3 r-t -.-I rt a rt ■e'3 rt p a 2 0) -s 3 3 F o .a '-I o 5 t" ra o ■?,_g ^3 rt S rt a rt-^ rt " -J tn <« a .3 ■=> 3 09 C rt "^a S n rt'.a a ^ 01 a; tO-w a ^ a-5 o c4 3 rt J 3 to o •J r: d . .3 3 J ^ rt .-e a 0) 3 ^ J ►-^ C rt -(J> |J ^ 3 rt rt t: m ^ ^ rt - i o • a 2 « c a ^ rt"o ^•a.23 =" rt'S ^' - ca ^^ -tJ CO *^ S « 2^ O t> *^ -*3 -S O > bD uO K m -♦J a: rt « O +3 ft i5^ o 3 -w tC 3 '•^ "S -5 2 1 2 "*-i rt -3 a. c •a a . ri sl rS "C -l^ = 2-0 y. rri - i> 2 O ^ — --^ ^ r-' t^ c CJ ^ C ^ ff fj 3 1 t; O '''H <^ O To « S ,-:. 'f - o i :^ =i f=-:3 .— W r +3 H 2 •+-J ~J a ^ tt 3 o o rt ^/5 !^ ^ Ph^ ■J '~ Oj :, hc i; ^ c 03 i Vi •,' c i= 5 •J ,—• ;.~ ^ i - W^ z u .-^ •C -•-^ --H C' P- "' :;; 1:3 •'^ 'S - -/5 c f= ;:; ;5 >- 41 c " i .S = .2 T D^ »j -f-3 ■c > 1^ m :3 > m fci .-5 ""^ ^ . — 1 K MH -^ C rt ^ ^ S'ib «^.H -- CO c^ ,-j a> ,^ d V .-ri |JH rt i> >j fS in t> — -a i !8-a S '■^ Xi rr. ."ti a; S pH ^ ~ -^ '/3 /J *3 <-^ ->-> V ■^ t h L- a T- ^• X rt r— c oj rt C, r- ri a ^ rt cr. c ■j: 'Z r- ^ ■t; .i; 'S _^ « r. •li ■? c- n c y. "C - c X - ^i T rt c js r-« -*- ;- j.; £i U '5 'S S .Hi r. 5 k. c S c i; r- -~ ^ ^ :^ c- C r^ r ^3 c: :; r\ rt t^ X5 •r ^ ^ ■/; --■ r c. c Eli r. r y; rt X -f 3 1* !C ^ r' C ■^ rr — *, 5 +3ec :j rt <;: M --> .1. rt ,a q 1= K ^ E= ^ = o o tJO ei h^ tf) c a ,-> 1-4 ■*-< -t-) cr a (U O a~. •■5 ,4 I— < =3 S t- a o I- rt O ^ ^' tn cu .^ p 3 ^< c^ C IT"* ^ a ^ <» rs (■. m <— ' ti r! c:! -1 U 1— i a - y H S « ri 3 «pU CD •J I I 14 o Pi o a 2 'o ^ s "iC 01 ^ _ „ M «■ of 2 ''■'^ '^ ,r: ^ o rt g c'' ^ -E -3 b a 1 ^ 0.3 fe -s I ^a > S3 '^ ^^a'^i" c3 a c ■;; ^ O o 2 ^ ■ c 3 £ c^ wo' M M CC t CQ p-J ^^ rn ^ H **i • >-« :§ ^ ff rt d-^ !*:^- f= 2 Si 2 S a s § e8±j o ti "^ O •5b o U o 'o o ■-d o fl '-I -♦-> d u d o y « 4J V m o rt o 3 O d s "^ ^ "d ^ 3) V o 3 c3 a • rH o S «> ■tJ .2 rt C +^ 'E "S '-S o u a o jj ® d u to » ra i- > o o Sb-r P< >> .S d y a aj 00 r3 .•ti a o a-d — ' a) o a § «^ >d o 33 u n rd u fUiS d d 0> o o l-'E -1. +^ • rH pd p» -d u +3 y •^ 2 •■? a d !* o a d a> rt ;r: .s tn ,^ pHM-< 2 o a'^3 to M d u 5l o tn " 'd ^ 3 f^ a o d-^ S ^ O --i .g r3 o 1— * d -3 CO m >. a ,d ^ ^ ^ 0) ^ . >■ ^ ^ ■Eb &-I3 4) d > 3 iS to OJ-d o o <0 Ti *o M u o rt rO a> 0) rr> m r^ ^ -M ^ 'ET *-H 1* +5 O -*^ « d «* rd 4) . is -d '-' , CO P^ c3 •- rt i^c-r, 'd 1= rt «« • q w 03 d^ ■rH ^J rP d Tl o jii d cj •rH rH to ""^ d a> a-* § '-' 1^ ^ si 03 t> > m 2 "c .a t> O c« (Urd -S -fj d o •2S|| •15 3rP rd fl^ O P- o 02 cj •E b 2 >> -SI? ;§.2 S « J is ~ CO « r-H 1? d CC rH »- tH d S O P • r3 0) d.S o .5 15 C5 £ = ^ i; > '.-' o 3 3 ? o o s J» c ►- O 7J o S '- c5 o c ^ e ^ f— Ch O <15 J5 ^ c !3 =3 ., c o ■:0 ''" H 2 I-S S r^i y *^ /-^ -J o ■— 1 ■A ^ ' u « p c ^ t-' 1-1 ;3 s« c ^ rj o o o +2 "^ £ g u £ ? (^ ■^ n '^ '-J -^ ^4 <^4 *^.:2 v. .- ' - -V^ ,3" .':! .5 r: ? r' '> "^ C J ^^ -i! i K , ^ 5 s >'^ i''-— c ^ 2 'T 1'^ --S'S ii >■ ^ L, : o :-' ^ O t.-d -J rt.H 2? '^ ^n — 'fl S- 32 -i.-t; 71 'i-i X, »r rHO ^<, '~^< o ^ o-?. q o i, - :- ;. •/. «: ci JiL ^ -i I- u >w -H 1— I O O St: ;:; c ^ s 2 O =3 to r-7« CI c '72 •^rf c ^ 1h rt ;i >w X r—i ph m c te H ^' .2 ." S 'S 'S p -a o J- crj m r IG SUBSTANCES INSOLUBLE IN WATER, BUT SOLUBLE IN HYDROCHLORIC ACID OR AQUA REGIA. Many metals are .soliil)le in liytlroclilorio aeid, others in nitivc acid. Tin and antiniony are converted into insolnble oxides by nitric acid, but can be dissolved by hydrochloric with a little nitric. Many in- soluble metallic conii)ounds may be decompo.setal. The oxalic acid also, cannot be deteck^d by calcium chloi-ido, as the chromo-calcium oxalate ifi solu])le in water ; the test with sulphuric acid, or the same acid with manganese dioxide, must be resorted to. Tlie same applies to the double tartrates and citi-ates ; these must bo decompo.sed by tnuxting with hy(lrosul])huric acid. All the tartrates can be recognised by the peculiar smell evolved on heating. Chromates insoluble in water may be recognised by the action of hydrochloric acid and alcohol, which give a green solution containing oxide of chromium ; the metal may remain partly undissolved as with lead, or may be held in solution, precipitable in some cases by hydro- sulphuric acid. In the case of zinc and similar metals not so preci- pitable, the chromatt must be decomposed by boiling or fusiu" with sodium carbonate. Arsenites and arsenates may be decomposed by boiling or fusing with sodium carbonate, when the acid combined with sodium may be washed out, the oxide or carbonate remaining behind ; or the salt may be dissolved in acid, treated with hydrosulphuric acid, when the sulphide of arsenic will be precipitated, free from metals of Groups III. and IV., but mixed with sulphides of metals of Groups I. and II. These sulphides can of course be separated by ammonium sul- phide, but the process with sodium carbonate is preferable. Phos- phates, borates, oxalates, &c., of metals of Groups I., II. and III. may be dissolved in acid, treated with hydrosulphuric acid or ammo- nium sulphide ; the solution, after digestion, will contain the acid, the residue the metal as sulphide. The phosphates, &c., of metals of Group IV. are best examined by boiling or fusion with sodium carbonate. Many may be examined directly. See apatite, among tests for minerals. Calcium sulphate, when in fine powder, will dissolve in boiling water, and the base and acid can be detected in the solution; strontium sulphate dissolves very slightly in water; the sulphuric acid can be detected in the solution by barium chloride. Barium sulphate is quite insoluble. These sulphates are best examined by boiling or fusing with sodium carbonate, separating the earthy carbonate by washing, dissolving in acid, and applying proper tests ; the filtrate can be examined for sulphuric acid after neutralisation. 8 18 Ijt'iul Mil|)liiit(' may lio oxaminotl iit tlio saino way, and (listiii^uisln'(l atoiuTfrom the al)Ovo l»y tiiniiiii,' Mack with aimiiouiuui sulpliidc. The iiisoluMc cliloriilc, idclidcs, and lirdiii'uh* of lucrcury may he cxamim-d hy tifatiiig wilh ammonium .sulphide, oi' by hoiling with .sodium hyih'atc oi' ('.u'hoiiat*'. Calomel will dissolve when heated with nitric acid Of u^ua re;.jia. Th(> iodine, chlorine and brominc! in th«! .silvci' compounds can \>o sofniratcd hy fusing witli sodium carbonate. Tin tetroxide must be fused witli pota.ssium cyanidi', the resulting motiil dissolved in dilute hydi'oddoric acid, and the metal detected by appropriate tests. TKSTS FOR SOMK OB^ THE MORE (lOMiMONLY OCC'JRRIN(J mini: HALS. Shell Maul. — By washing with water and 2)ouring olF tho ligjiter particles, fragments of shells may readily be detected. The mineral dissolves readily in dilute nitric acid, gives a precipitate with oxol' acid and ammonia; tho precipitate, separated after warming, .><■ filtration, and the filtrate tested for magnesia by means of .sodium phosjihate. The nitric solution heated with .ammonium molybdate may give (rarely) a faint yellow precii)itate or colour, owing to pi'esence of phosphate. Limestones may be examined in the same manner ; many contain magnesia (Kockwood). They sometimes contain bituminous matter which causes them to evolve a disagreealde smell when pounded oi- heated. Calcspar is generally met with in the rhombic or the scalcnoliodral form; effervesces even with weak acids; can be scratched with a knife. Fluorspar is usually crystallisev' in cubes; treated with suli)hui'i( acid evolves a gas which cori'odes glass ; Ciumot be scratcluMl with a knife. Apatite — (Jaicium phosphate — is usually of a greenish or reddish colour; occurs generally in six-sided prisms; when in powder dissolves readily in nitiic acid. The phosphoric acid can be detected by heating the solution with ammonium molybdate, when a yellow precipitate is formed ; or by adding silver nitrate to a solution obtained by boiling an excess of the mineral with a very little nitric acid, a yellow j)i-e- 1 19 cipitate will be formed. The addition of ammonia dissolvps the silver phosphate, but of course preciititatos the original salt. The lime csiii be detected by adding oxalic acid and excess of sodium acetate to the acid solution. A light coloured pyroxene is often mistaken for apatite, readily distinguished by being much harder, and quite insoluble in nitric or hydrochloric acid. HjEMATITE — Ferric oxide — is not magnetic ; when in fine powder dissolves in hydrochloric acid. The addition of nitric acid to the hot solution does not change its odour. The ii'on can be detected by usual tests ; the ore gives a brown red streak on rough porcelain. Magnetic Iron Ore. — Attracted by the magnet, the hydrochloric solution turns first black on the addition of nitric acid, and then brownish yellow. Ore gives a black streak. TiT.M'«ii; Iron Ore. — Scarcely attracted by the magnet; dissolves in hydi-ochloric rcid only when very finely pounded. The titanic acid is best detected by fusing with an excess of potassium bisulphate ; dissolving in a large quantity of cold water and boiling for a long time, a white or yellow precipitate is formed. Sulphides, with the exception of cinnabar (mercuric sulphide, not occurring in Canada), are acted on by nitric acid, red fumes are evolved, and the solution contains sulphuric acid, J a the case of galena (lead sulphide), the sulphuric acid remains combined with the lead oxide, as insoluble lead sulphate. (See Galena.) The sulphur can generally be detected by heating a i)ortion of the ore in a tube, open at both ends, held slanting, and testing the gas evolved by iodic starch ])aper. Some sulphides, such as those of zinc, antimony and bismuth, may be dissolved in hydrochloric, with evolution of hydro- sulphuric acid, and the solutions examined by the proper tests. Iron Pyrites, or iron bisulphide, when heato