which other acidic compounds do not comtain oxygen, like hydrochloric acid?
119409
silicone, carbon, nitrogen, sulphur ect. basically eny  elements from grp 4 - grp 7, all group 3 elements r amphoteric( both acid n base) n grp 1 n2 oxides r basic
377266
1) Zinc Chloride\n2) Copper (II) Sulphate\n3) there is no such thing as NH4OH, but oh well..\n    Ammonium Hydroxide\n4) Iron (III) Sulphide\n5) Aluminium Phosphate\n6) Lead (II) Nitrate\n7) Sulphur hexafluoride\n8) Sodium Sulphate\n9) Mercury (II) oxide\n10) Potassium Clorate (V)\n11) Tin (II) Choride\n12) Iron (II) hydroxide\n13) Mercury (II) Sulphate\n14) Carbon Dioxide
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There really is not a set formula, as the -ite anions don't have a set formula themselves (PO3 2- for phosphite, NO2- for nitrite, SO3 2- for sulfite, Cl02- for chlorite, etc.)
445022
I'm not quite sure what "PCC" is, but I do know that it is necessary to have at least one hydrogen atom on the carbon atom holding the -OH group of an alcohol before it can be oxidides. Tertiary alcohols don't have this H atom, so only primary and secondary alcohols can be oxidised.
472130
A.  Mercury does not hold on to oxygen readily, so at high temp (in absence of air) it decomposes to mercury metal and oxygen.\n2HgO (+heat) ---> 2Hg + O2\n...so the atoms remaining are Hg and O\nB.  Calcium carbonate neutralizes hydrochloric acid, giving off carbon dioxide.\nCaCO3 + 2HCl ---> CaCl2 + H2O + CO2 (gas)\n...these are the MOLECULES remaining...if you really want atoms, they would be Ca, Cl, H, O, and C.\nC.  Sucrose is partially dehydrated with heat...loses water and the rearranges to colored products.\nC12H22O11 (+ heat) ---> H2O + mixture of by-products determined by time and temperature.
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weak organic acid= vinegar\nTitanium Oxide = sun block\nalkaline earth hydroxide= milk of magnesia\nalkali metal= NaCl\npaper chromatography= a penny and iron vinegar mixture\ntransition element= iron or copper\nnonmetal=sugar\nelectrolyte= NaCl\na noneletrolyte solution= sugar and water\noxide  of a element = rust or sun block
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Franpal is correct, hydrogen and oxygen.  If you're thinking of a D, it may be 'heavy water', which has Deuterium rather than hydrogen (an isotope of hydrogen).
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MgCO3 + 2HCl ---> MgCl2 + CO2 + H2O\n\n2HCl + MgO ---> H2O + MgCl2\n\nBarium hydroxide is a base so can be neutralised with any acid.  An example being HCl.\n\nBa(OH)2 + 2HCl ---> BaCl2 + 2H2O\n\nor H2SO4\n\nBa(OH)2 + H2SO4 ---> BaSO4 + 2H2O
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It's pentanal, because it's a terminal carbonyl. It's certainly not pentanol, because otherwise you'd have a carbon missing 2 bonds, or a carbon missing 1 bond and an oxygen missing 1.
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acidic solutions. they will form nitric acid and sulpurous/sulphuric acid respectively. why is quite beyond the scope of explaining on yahoo answers sorry- its got to do with valence electrons and bond formation abilities ( i could if you are familiar with these-but im not sure)- in essence, they form compounds that are able to donate H+ ions. these are called arhenius acids
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n-hexanoic acid\n\nThere are a LOT of compounds with that chemical formula.  Check chemfinder.com for more.
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phosphate\nsulfate\nnitrate\nperchlorate\n\nThe oxidation state of the anion will not change.  These anions simply have a proton (or a couple protons) as the cation instead of a salt.  The name of the acid directly reflects the anion's name.  All the acids you listed had an -ic suffix which implies a fully oxidized state.  The per- prefix on perchloric sugggest it is one step beyond fully oxidized.  \n\nFor example, another oxoacid is sulfurous acid.  The -ous suffix informs us that the oxidation state of the non-oxygen element is lower than those with an -ic ending
536011
Look up the chemical in a pKa ( -log of dissociation constant K)table of acids. H2PO4- has a pKa of 7.20. It is not very acidic.
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6 moles of hydrochloric acid will react at a faster rate than 1 mole of hydrochloric acid because the solution will not dilute as fast as the smaller amount of acid- more acid to react with the Zinc.\n\nSounds good to me...
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An acid and its conjugate base differs by a hydrogen cation (or proton) H+, so:\n\na. H2SO4 and HSO4-\nd. HCl and Cl-\ne. HF and F-\n\nare conjugate acid-base pairs
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NH4ClO4 --> NH4^+ + ClO4^-\n\nNow in a water solution,\nClO4^- + H2O --> HClO4 + OH- --> This doesn't happen because HClO4 is a strong acid.  Therefore the only contribution to the pH is from the NH4^+\n\nNH4^+ <=> NH3 + H^+\nYou start with [NH4^+] = 0.40 M, and [NH3]=[H^+] = 0 M; after undergoing equilibrium [NH4^+] = 0.40 - x, while [NH3]=[H^+] = x; Ka = [NH3][H^+]/[NH4^+] = (x)(x)/(0.40-x) = Kw/Kb = (1 x 10^-14)/(1.8 x 10^5)\nAssume x << 0.40, so x^2/0.40 = 5.56 x 10^-10\nx = 1.49 x 10^-5 M = [H^+]\npH = -log(1.40 x 10^-5) = 4.827
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Oxygen in peroxides\n\nPeroxides include hydrogen peroxide, H2O2. This is an electrically neutral compound and so the sum of the oxidation states of the hydrogen and oxygen must be zero.\n\nSince each hydrogen has an oxidation state of +1, each oxygen must have an oxidation state of -1 to balance it