what is the solubility of calcium hydroxide in water?
88535
Ca(OH)2 \n0.185 g/100cc at 0deg C\n        0.077 g/100cc at 100deg C
568319
in water the solubility is -6.26440763228718
407734
Hummm:  You can calculate the [OH-] from the pH.  [OH-] = 10^-2.  pH + pOH = 14 (from [H+]x[OH-] = 10^(-14):  pOH = 14 - 12 = 2.  Find the solubility product for iron (III) hydroxide in a table in the back of your textbook or a handbook of Chemistry or physics. Kp = [Fe+3] x [OH-]^3. Substitute numbers in and solve for [Fe+3].  This is also the molar solubility as one mole of iron hydroxide contains one mole of Fe+3.
572596
calcium hydroxide is a base, and is often added to acidic soils to raise the pH. this is very helpful, because some plants cannot absorb needed nutrients in acidic soil. acidic soil is commonly found in the northeast area of the US.
1180992
depends on the strength of the base actually.  water is amphoteric which means it can act like an acid or a base.  if a weak base is put in water the water can neutralize it, but water is quickly overrun yielding the below equation.\n\nB + H2O yields HO- +BH\n\nthis makes the water basic.
250762
2 HCl + CaCO3 ----> CaCl2 + H2O + CO2
883152
MgO and BaO will react with water to form the hydroxides Mg(OH)2 and Ba(OH)2, those will be neutralized by hydrochloric acid to give the chlorides MgCl2 and BaCl2 and water.  I think you may have gotten C2O wrong, that is not a real chemical compound.  If you meant CaO it will behave in the same way as MgO and BaO.
814242
Barium Hydroxide is a weak alkali which is not very soluble. If you try to neutralise it with dilute sulphuric acid you will get a precipitate of Barium sulphate. This means you won't be able to neutralise solid barium hydroxide just the solution. To neutralise either the solution or the solid use dilute hydrochloric acid.\nBa(OH)2  +  2HCl  =  BaCl2 +  2H2O\n\nIf you add carbonate ions CO3 2- to a solution of barium hydroxide Barium carbonate will be precipitated. Again carbonate ions (as in sodium carbonate solution) will not completely react with solid barium hydroxide.
491321
Deep J got it all...Another way  of testing for carbon(IV)oxide is by passing it through lime water(Ca(OH)2).The I.U.P.A.C name for lime water is calcium hydroxide....It turns milky when it is being passed through lime water...This is the cemical equation of the reaction... Ca(OH)2+CO2-CaCO3 + H2O..The milky substance is calcium trioxocarbonate(IV) which is the substance that is used in the production of chalks used in schools...
712818
more soluble in what solution?
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-
736794
I'll teach you how to do these.  The answer may seem long at first, but just try it, and you'll see it's not as bad as it first appears.  For mass/mass problems, you only have to use the first section of this answer:\n\nToo solve these types of problems, use the following general steps:\n\n[I will use the general word equation: calcium hydroxide reacts with lithium bromide to produce     calcium bromide and lithium hydroxide; as an example, throughout each step, to aid in your learning]\n\n(1)  Write the correct chemical formula for each substance in the reaction.  Be certain each chemical equation is correct!   (ex:  calcium hydroxide:    correct formula  = Ca(OH)2;   NOT CaOH.)\n\n(2)  Write out the chemical equation;   ex:  Ca(OH)2  +     LiBr   gives      CaBr2    +       LiOH    \n\n(3)  Balance this chemical equation;    ex:   Ca(OH)2  +  2LiBr   gives   CaBr2   +   2LiOH\n\n       Note:  this balanced equation is TELLING you that one mole of calcium hydroxide is reacting with 2 moles of lithium bromide to produce (gives) one mole of calcium bromide and 2 moles of lithium hydroxide.  It is TELLING you the relative number of moles of each substance.  \n\n(4)  Determine the MOLE RATIO of the substances involved;  ex:  if the question says you have 1.0 moles of calcium hydroxide and it reacts with an excess of lithium bromide, and asks how many moles of lithium hydroxide are produced,  the answer would be 2.0 moles of lithium hydroxide.  In other words, the MOLE RATIO of calcium hydroxide to lithium hydroxide is 1 to 2, also written as a “1:2 ratio“.    ex:  same question but suppose you have 3 moles calcium hydroxide.  Because the mole ratio  is 1:2, you would produce 6 moles of lithium hydroxide.   A ratio of 3:6  =  a ratio of 1:2;  (you just reduced it to simpler terms).  \n\nStop here if you  are simply given the number of moles of product you have, and asking how many moles of some different substance are produced in a chemical reaction.  \n\n\nSame type of problems, but working with grams instead of moles:\n\nyou simply have to do a couple of extra steps:\n\nI will use the same reaction as above, but will change the question to this:  \n\n“If you have  255 grams of calcium hydroxide, how many grams of lithium hydroxide will be produced, (assuming you have an excess of lithium bromide)”.  \n\n [Note:  unless the question states otherwise, assume you have an excess of the other reactant, thus giving the maximum yield of product; see “Limiting Reagents” below to solve those types of problems]. \n\nTo solve, complete the first 4 steps above (we’ve just done that):\n\n(5)  Convert grams of substance into moles of substance!!!   This is essential in solving these types of problems.  THE KEY STEP FOR ALL PROBLEMS OF THIS TYPE IS TO ALWAYS CONVERT EVERYTHING INTO MOLES FIRST!!!  The general formula’s are as follows:  \n\n                        Moles  =  grams / molecule weight\n\nOr you can use basic algebra and say the following:  \n\n                    Grams  =  Moles   X   molecular weight\n\n[Note:  “molecular weight” is used to describe molecules; “formula weight” is used to describe ionic compounds; and “atomic weight” is used to describe elements;  ALL of them are the sum of all the atomic weights of the elements in the substance. In the case of a single element, alone by itself, this refers to the atomic weight of that element.  Note that the 7 elements:  hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine and iodine only exist as “diatomic” elements, when they are ALONE by themselves (not combined with any other element(s)).  Thus H2, is the correct way to write the chemical formula for hydrogen when it is all alone, by itself.  And it is a molecule, and it’s molecular weight would be equal to 2.0.  This is the same for the all diatomic molecules:  the molecular weight will equal double the atomic weight for that particular diatomic element (because there are TWO a
805565
Ca + 2H2O yields Ca(OH)2 + H2\n\nBasically it's almost balanced already, just add a 2 in front of the H2O.
944444
Both calcium chloride and silver nitrate are soluble in water. If you swap the names you get silver chloride and calcium nitrate. Silver chloride is insoluble and calcium nitrate is soluble. So if you mix a solution of calcium chloride and a solution of silver nitrate, an insoluble precipitate of silver chloride will form and calcium nitrate will remain in solution. The balanced equation is \n\nCaCl2(aq) + 2AgNO3(aq) -----> 2AgCl(s) + Ca(NO3)2 (aq)
417834
Something that requires water in order to become a true Base\n\ne.g. CaO + H2O -> Ca(OH)2
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.
211591
Ca3PO4 and CuOH\n\n^^those are the answers