What is the salt produced when magnesium hydroxide reacts with sulfuric acid?
438725
Magnesium Sulfate\n\nMgSO4\n\nMg(OH)2 + H2SO4 -> MgSO4 + 2HOH\n\nHOH = H20\nJust in case...
788847
The column elutes sulfuric acid, H2SO4\n\nMolarity is mol/L (mol/dm^3) and is also mmole/mL\n\nYou used 25 mL of a KOH solution containing 10^-2 mmoles/mL, or a total of 0.25 mmoles\n\nThe neutralization reaction is   H2SO4  +  2 KOH  ---->  K2SO4  +  2 H2O\n\nThe column reaction is  CaSO4 + 2 i-EH+  ---->  i-E2Ca+2  +  H2SO4   (i-E is ion-Exchange)\n\nBottom line is that there is a sulfate for every TWO KOH's, and there is a Calcium for each ONE sulfate.\n\nHope this helps.
101127
You get Mg2O2 (magnesium peroxide) and water H2O.
728971
(The) second experiment was to observe the reaction when a magnesium ribbon was ignited. The ribbon was put to the flame of a burner (delete ,) and was ignited. The reaction was very (intensive) (change to intense), and (burned with a) (delete was with) very bright white light. Usually when a substance is ignited in air, it reacts with H2 or O. In this case, because the Mg was the positive ion, it must have reacted with oxygen, (which is a ?)negative ion. In this experiment, because Mg was joined to O2 to make 2MgO of different composition, this was a combination reaction.\nThe third experiment 0.1 M CuSO4 and 6 M NH3 were used. CuSO3, a Sky blue liquid,  was place in a test tube, and then 1 drop of 6 M NH3 was added. Right after NH3 was added, the top of (the) liquid changed to navy color.  After the liquid was stirred the color of the liquid changed to a blue that was darker than the color of CuSO3. Ten more drops (of CuSO4?) were added to the contents, and the color of (the) contents changed to a violet color.
800284
a alkali will form a salt\na acid will not react\na metal will form a metalic sulphate and liberate hydrogen\n1)NAOH +H2SO4=NA2SO4+H20\n2)HCL +H2SO4=NO REACTION\n3)Zn+H2SO4=ZnSO4+H2
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.
135415
That's a difficult question to answer because magnesium hydroxide is practically insoluble in water with a ksp value of like 1.8 x 10^-11 so very little magnesium hydroxide is dissolved in water.  But if you were to compare the solubility of magnesium hydroxide at 25C with 80C my guess is that it would be more soluble at a higher temperature but only by an almost insignificant amount.  \n\nIn short, Mg(OH)2 is pretty much insoluble in water so my direct answer after all the reasoning would probably be: no, Mg(OH)2 does not fit the pattern due to its extremely low solubility.
904363
(NH4)2CO3+MgSO4->(NH4)2SO4+MgCO3
457901
Any acid reacted with any base creates a salt -- that is the definition of a salt.\n\nThe most recognized salt, of course, is table salt -- sodium chloride (NaCl).  This is the product of reacting hydrochloric acid (HCl) with sodium hydroxide (NaOH).  The equation is:\n\nHCl + NaOH ---> NaCl + H2O
1175982
I think you can get zinc sulphide by reacting zinc with sulphur straightaway (though I can't say the exact conditions required) . Or you could add ammonium sulphide to zinc hydroxide solution and and get zinc sulphide precipitated out.\n\nOr else, it can also be precipitated by hydrogen sulphide, from an alkaline or neutral solution of a zinc salt - in which case zinc chloride can be used. \nThe reaction would be:\n\nZn2+ (aq) + S2- (aq) -------> ZnS (s)
787481
NaHCO2 + H2SO4 --> Na2SO4 + CO2(g) + H2O(L)\n\nSodium bicarbonate + sulphuric acid equals sodium sulfate + carbon dioxide + water
941585
Simple, just react the metal with a strong acid such as HCl(hydrochloric acid), to produce the salt+ hydrogen gas \n\nex. Au+HCl=> AuCL+H2( silver+hydrochloric acid= silver chloride(salt) + hydrogen gas). same goes for all other metals.
455269
H2SO4 + Mg(OH)2 -> 2H2O + MgSO4
795289
If the solution contains a diprotic acid, there are two hydrogen atoms available for the acid to lose (such as H2SO4).\n\nA solution of 50mL of a 1.012 M solution would contain 0.0506mol of diprotic acid which would then dissociate to give you 0.1012mol of H+ ions. \n\nThen you must have as much hydroxyl anions (OH-) as you do hydrogen ions (H+), so you must have 0.1012mol of OH-. Using the formula 2H+ + 2OH- -----> 2H2O.\n\nTo convert 0.1012mol OH- into grams of Mg(OH)2, you divide the OH- concentration in half because of the equation\nMg2+ + 2OH- -----> Mg(OH)2\n\nwhich would give you the 0.0506mol Mg(OH)2.\n\nFinally you would convert the 0.0506mol Mg(OH)2 into grams Mg(OH)2 by multiplying the number of mol by the molecular weight of magnesium (II) hydroxide--the calculation is shown below:\n\n0.0506mol x 58.31g/mol = 2.95 g Mg(OH)2\n\nSo you would need 2.95 grams of Mg(OH)2 to neutralize the solution. \n\nHope this helps!!
298301
Hmm. This is exactly what I've been doing for the past few weeks. I'm assuming these are aqueous solutions of the three, right?\n\nWell, both magnesium and strontium form precipitates with hydroxides, so you could add some sodium hydroxide and centrifuge it down. To the liquid remaining, add some kind of sulfate, like potassium sulfate, because barium precipitates with sulfates, forming BaSO4.\n\nTo the solid containing strontium and magnesium, add ammonia to make the solution basic, then add sodium carbonate. The magnesium should complex with the carbonate and fall out, forming Mg4(CO3)3(OH)2. Then, whatever's left is strontium.
429367
It doesn't form into anything. You said it yourself, it's soluble. The hydroxide part of the milk of magnesia (magnesium hydroxide) and the hydrogen of the sulfuric acid combine to form water, but then you're left with Mg+2 and HSO4- ions. It's just a clear liquid.
324126
The salt that is formed is Barium sulphate, which simply has low solubility in water (or acid or bases - you need a chelating agent for the Barium to dissolve it again). There is  no other significant reaction (like redox or altering pH).