describe the neutralization of an acid nad a base?
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An acid and a base react to form a salt and water.  For example:  NaOH + HCl ==> NaCl + H20.  The products will always include some sort of salt, as well as water, and the reation will always be exothermic, meaning energy is released.
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Technically with molar amounts being equal, an acid and a base react in what is called a "neutralization reaction"...\n\nie:\n\nHCl + NaOH ---> NaCl and water\n\nBasically you get a salt and a water.
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A salt is formed between the reaction of an acid and a base. Usually, a neutral salt is formed when a strong acid and a strong base is neutralized in the reaction: \n           H+ + OH- = H2O \nThe bystander ions in an acid-base reaction form a salt solution. Most neutral salts consist of\ncations: Na+,K+,Rb+,Cs+,Mg2+,Ca2+,Sr2+,Ba2+ \nanions:  Cl-,Br- ,I-,ClO4-,BrO4-,ClO3-,NO3-\nThese ions have little tendency to react with water. Thus, salts consisting of these ions are neutral salts. For example: NaCl, KNO3, CaBr2, CsClO4 are neutral salts.\n \nWhen weak acids and bases react, the relative strength of the conjugated acid-base pair in the salt determines the pH of its solutions. The salt, or its solution, so formed can be acidic, neutral or basic. A salt formed between a strong acid and a weak base is an acid salt, for example NH4Cl. A salt formed between a weak acid and a strong base is a basic salt, for example NaCH3COO. These salts are acidic or basic due to their acidic or basic ions.\nAcidic ions: NH4+,Al3+,Pb2+,Sn2+.\nTransition metal ions: HSO4-, H2PO4- \nBasic Ions: F-,C2H3O2-,NO2-,HCO3-,CN-,CO32-,S2-                 SO42-,HPO42-,PO43-
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When an acid reacts with an alkali (base), neutralisation occurs as the pH of the mixture becomes neutral, pH=7. (Acidic: pH < 7, Basic: pH > 7).\n\nSo an example would be to react sulphuric acid with sodium hydroxide to form sodium sulphate (salt) and water.\n2NaOH + H2SO4 ---> Na2SO4 + 2H20\n\nAn ELEMENT that would neutralise sulphuric acid (i.e. make its pH 7) could be any metal.\n\ne.g. Mg + H2SO4 ---> MgSO4 + H2\n\nBut this is not called a neutralisation reaction.
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There's two things you're being asked to recognize.\n(1) what kind of reaction is this\n(2) is it going to go forward?\n\nLets deal with them in order.\n\n(1)  What kind of reaction is it.  \n\nI find it very helpful personally to say the names of the molecules out loud.\n\nPhosphoric Acid reacts with Strontium Hydroxide to form what?\n\nWell, the first reactant is an acid, right? The second reactant is a metal hydroxide, like sodium hydroxide, so its a base.  That makes this an acid-base neutralization.  There's no redox chemistry going on here, so the bonds in the polyatomic anion, phosphate (PO4 (3-) ) are going to all remain intact.\n\nRemember, an acid + base neutralization will always form water and a salt.  In this case , your salt would be a combination of the non-hydrogen portions of the acid (PO4) and the metal.  \n\n\n(2)  Will this reaction go forward?\nStrontium hydroxide is moderately soluble in water.  The phosphate salt very nonsoluble.  That means that the product of the displacement will be taken "out" of the solution, driving the reaction towards formation of products.\n\n*********NOTE**********\nMany of your choices aren't charge-balanced molecules.  This may help you tremendously.  I think you may have a typo in your question.\n\n*********NOTE 2*********\nOnce you fixed the choice (d) your typo was taken care of.
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Carbon Dioxide-Acidic\n\nOxygen-Neutral
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na+2h2o=na(oh)2 + h2\n1.Note that na is a highly reactive metalk reacts even with cold water producing sodium hydroxide and liberating hydrogen.\n2h2so4+naoh = na(so4)2 +2h2o\nNote that h2so4 (sulphuric acid) reacts with naoh(sodium hydroxide),abase and the reaction b/w acid and base forming water and a salt is called neutralization reaction
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A Bronsted acid is a substance which releases H+ in water.\n\nHF + H2O --> F- + H3O+\n\nNH4+ + H2O --> NH3+ H3O+\n\nH2CO3 + H2O --> HCO3- + H3O+\n\nHNO2 + H2O --> NO2- + H3O+\n\nNote that the final result is always the hydronium ion \n(H3O+)
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NaOH ® Na+ + OH- is sodium hydroxide, a common base.\nWater has equal hydronium and hydroxide ion and is thus neutral as is C2H5OCOOH ® H+ + C2H5OCO O- which is in chemical equilibria and C2H5OH is ethanol that might have a slight alkalinity but is not considered a base.
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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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For any reaction between a strong base (potassium hydroxide) and a strong acid (nitric acid) the end result is the neutralization of the acid and base to produce water.  The net ionic reaction will always be the same and show the reaction of the acid (H+) with the base (OH-) to form water.  Therefore,\n\nH+  +  OH-  --->  H2O
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It's a salt - ammonium acetate. Ammonium is an acid, but the acetate ion is actually alkaline.
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A neutralization reaction occurred between the acetic acid in the vinegar and the baking soda (sodium bicarbonate) to produce sodium acetate and carbonic acid, which decomposed to form water and carbon dioxide.  Since the chemical species are different now than they were before the reaction started, a chemical change has occurred.
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Well first of all you have not given us all the information to be able to answer this buffer question.  We need to know the Ka (6.2x10-8)of the acid.  But the steps to perform the task.  Calculate how much of the acid is neutralized by the addition of the base.  Recalculate the equilibrium concentration of both the acid and base with the new acid value.  using Ka=[H+][Na2HPO4]/[NaH2PO4] solve for H+ and finally use pH=-log[H+].  Your final answer..pH=7.25
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to determine whether an acid or a base is soluble in say the universal polar solvent water, u should be knowing whether the substance is strong or weak\nnow bases like NaOH, CsOH, RbOH, Mg(OH)2 are strong bases and in solution they give us the cations and anions(mostly the hydroxyl grp)\nbases like Be(OH)2, Fe(OH)2 or 3, Cu(OH)2 or any of their oxides are weak and hence in solution they do not undergo complete dissociation and most of these are insoluble\nso in case ur not in a lab, the only way is to identify their degree of weakness
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a) neutral\nb) basic\nc) basic\nd) acidic\ne) acidic if in solution\nf) basic.\n\npH is a scale ranging from 0-14.  7 is the intermediate and a pH of 7 means that the solution is neutral.  If the pH is below 7, then there are more H+ than OH- in the solution.  Hence the solution becomes acidic.  If the pH however is greater than 7, then there is less H+ than OH- in the solution and the solution is basic.\n\nFor the acid H2SO4, when in solution, it will dissociate to form H+ and SO4-.  The H+ gives the acid its acidic property.  Similarly when Ca(OH)2 is dissolved, it dissociates into Ca2+ and OH-.  The OH- gives the compound its basic property.
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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!!