What is the general name for a solution that produces positive ions and has a pH of 0 to 7?
541583
pH from 0 to 7: Acid solution.\nPH from 7 to 14: Basic solution.
172666
When a salt derived from a strong acid and a weak base dissolves in water, the solution becomes acidic. For example, consider the process\n \nNH4Cl(s) ----H2O ---> NH4+(aq) + Cl-(aq)\n\nThe Cl- ion has no affinity for H+. The ammonium ion NH4+ is  a weak conjugate acid of the base NH4+(aq) and ionizes as follows \n\nNH4+(aq) + H2O(l) <=> NH3(aq) + H3O+(aq)\n\nor simply  \n\nNH4+(aq) <=> NH3(aq)  + H+(aq)\n\nThe equilibrium constant ( or ionization constant) for this process is given by \n\n\n\nKa = Kw / kb  =   1.0*10^-14 / 1.8*10^-5 = 5.6*10^-10\n\n\n      x^2 / .10 =  5.6*10^-10\n\n           x^2  =   5.6*10^-11\n\n             x  =    7.5*10^-6 M  =  [H+]\n\npH  =  -log [H+]\n    \n    =  5.12\n\n     my answer is  C , NH4Cl
297566
Pure water (which is impossible to get, by the way), has a pH of exactly 7.0. This is because the Kw of water is 1.0e-14, so you get 1.0e-7 M of hydronium ions (and 1.0e-7 M of hydroxide ions). The pH is defined as -log[H+], so the negative log of 1.0e-7 is exactly 7.0.\n\nEDIT: sammi, 7.2 would be slightly basic.
706351
KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
1125360
H2O2 can exist in many forms at pH = 7, \n\nH3O2+, H3O3- are among the possibilities.
109387
Maybe you are referring to aqueous solutions of these species? If so, then a solution of glucose will be pH 7 since it does not have any proton or hydroxide to change the neutral pH of water. As for solutions of the rubidium, potassium and cesium IONS, they can accept hydroxide from water if they are stable enough to form the metal hydroxide or if they convert to metal oxides. That means hydrogen ions are also formed and this makes the solution acidic, and hence the pH drops. But large cations like Rb and Cs do not readily take in hydroxide owing to the low polarizability of the cations (see me winking here ;p  ), unlike the small K ion. So, with these clues, can you now find out by yourself the answer to your question? Don't we just love chemistry!
874983
1. Molarity = concentration and it expressed as mol per dm^3\n    Change the mass to mole and the 851 ml to dm^3. Then find   \n    the ratio of the number of moles to volume in dm^3\n\n2. Soluble ionic compounds breaks up the water molecules in H^+ ions and OH^- ions. Sodium carbonate give Na^+ ions and CO3^2- ions......Other ions that are present are HCO3^- ions called hydrogen carbonate ions. I have found that a solution of sodium carbonate is alkaline: implying that there are more OH^- ions to H^+ ions, due to the formation of HCO^- ions.\n3. OH^- (aq) + H^+(aq) ----> H2O (l)\n4. H^+ ions (ie. hydrogen ions), OH^- ions (ie. hydroxyl ions),\n   Ca^2+ calcium ions and Cl^- chloride ions\n5. Hydrogen ions, hydroxyl ions. ammonium ions and sulphate ions.\n6. Actually the calcium metal reacts with water to give hydrogen gas and calcium hydroxide. At the same time, calcium reacts with nitric acid to give calcium nitrate, water and brown nitrogen dioxide gas.\nHence there is no simple ionic equation for your question\nYou may want to consider this one:\nCa^0  +  2H^+   + 2OH^-  -----> H2(g)  + Ca^2+  + 2OH^-\n7. Hydrogen ions, hydroxyl ions, iron (III) ions Fe^3+  and sulphate ion SO4^2-
725443
d) basic\n\n[Non-metal oxides do the opposite and form acidic solutions if they are soluble e.g. sulphur dioxide dissolves to form sulphurous acid)
188856
An ionic liquid is a solution where dissociated ions are found. For instance, Sodium Chloride in water dissociates yielding the ions Na+ and Cl-. Similarly, any salt or ionic compound of the chmical formula AB dissociates yielding the cation A+ and the anion B-.\n\nNaCl ----> Na+ + Cl-\n\nAB ------> A+ + B-\n\nThis is due to the ionic property of some solutes. They always dissociates fairly in solutions, and thus the name an ionic liquid or solution.
729404
They yield K3PO4 and H2CO3.... Just switch the positive ion with the negative ion and make sure the charges cancel out to zero on each new salt.
1133019
There are a lot of sites that have info.  Search for "formula writing polyatomic ions".\nIf you have a list of polyatomic ions like "SO4", "SO3", "PO4", etc. you will see that they have specific charges associated with them.  SO4 and SO3 both have a negative 2 charge.  Hydrogen has a +1 charge.  A compound must be neutral so you need 2 H to pair with one SO4.  +2-2=0.\nPO4 has a negative 3 charge, so you'd need 3 H+ to offset the 3 negatives.  H3PO4.\n\nAs far as naming them, search for "naming chemical compounds"  The examples you are asking about are actually acids, so you might need to look up "naming acids".
679839
An acid has a higher concerntration of H+ ions in the solution. The PH scale is based on a logorithimic equation where a PH of 7 is neutral, andything below 7 is acidic and anything above 7 is basic. The conjugate acid is the H part of HX where the X- is the conjugate base. \n\nWikipedia has a great explination: http://en.wikipedia.org/wiki/Conjugate_acid
806865
Na2SO4 + H2O\n\nYou always get a type of salt plus water in acid-base neutralization.
965402
The protein will be negatively charged because th high pH of the solution cause the solution to have a high hydroxide concentration (relatively) and will cause extraction of hydrogen atoms from acidic residues on the aminio acids of the protein.  I would use a weak anion exchanger for the ion exchange chromatography of this protein.
1180433
No.  Any salt has a pH of 7.  Any acid has a pH of less than seven.  They're contradictory.  If you mixed some acid and some salt, I wouldn't call it salt any more.  I'd call it acid.
282642
actually, pure water does not have a pH of 7.0, it is slightly acidic, around 5.6-5.8 from what i have seen at work.
706856
Acidic.\nBecause sodium nitrate is a salt solution, and is neutral. Since you are adding an acid to a neutral soution, the end reault will be an acidic mixture.