How will you tell if a solution is acid?
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acidity has three different definations.\nLewis Acids - a substance capable of accepting as=n unshared electron from a base to form a dative covalent bond.\nArrhenius Acid - a Hydrogen containing compound that ionises and releases protons, [H+] in an aquous solution,\nBronsted Acid - a substances consisting of molecules or ions which donates protons, [H+].\nif any substances adhere to any of the three conditions, it is an acid. \nthe common theory is the Bronsted theory. this is where the term pH is introduced, where pH means 'potential of H+'. a solution with more H+ ions then OH- ions is an acidic solution. the pH is generally <7. however, this standard varies with temperature, and the concentration of the solute(water). \na general apparatus to determined is the blue litmus paper. it'll turn red on contact with acidic solutions.
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NaHSO4 itself is acidic, so the solution's color should be yellow due to the bromcresol green being in the presence of acid
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theoretically yes 10m acid has a pH of -1, and 10 moles of base pH 15.\n\nBut , in fact, for very high concentrations, you must not take in account the concentration of ions H+ but the activity . The actvity takes in account the high concentration and is \n\nactivity = gamma * pH where gamma is lower than one for high concentrations
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In these sorts of problems, you just need to keep your eye on H+, the hydrogen ion. An acid is anything that can be a source of H+ and a base is anything that can accept  an H+. \n\nBut once a base has gotten that H+, what do you call it then? It could possibly give that H+ back - so it is sort of like an acid at that point, since things that can give up an H+ are acids.  Well, chemists don't like saying "sort-of like", so it's called a "conjugate acid". Likewise, the molecule that gave up that H+ originally (the acid), could possibly take one back. So it's sort-of like a base after it has lost the H+, again, invoking the "sort-of like" naming rule again, it's called a "conjugate base."\n\nYou end up with what are called conjugate acid - base pairs. Say you put an acid in solution. If it gives up it's H+ it is now a conjugate base. So the acid and its conjugate base are called a pair.
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the rule of thumb is "like dissolves like" \nWater is polar so if it dissolves a substance, that substance is also polar.
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the only way to determine the rate of a reaction is to do the experiment yourself.\n\nUse starch as the indicator and plenty of acid.
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HNO3\n\nIf you couldn't answer this question, you must be a real noob in chemistry!!  Well, for other times, here's the way to differentiate betwee acids and bases.\n\nAcids:   acids can be easily identified by the hydrogens they contain.  Most acids have their hydrogen in the beginning of their formula.  HNO3 can be easily identified as an acid: it is commonly called nitric acid.\n\nBases:  most bases can be identified by the (OH) group at the end of their formula... therefore, we can immediately label b) and d) as bases.   \n\nNow here, NH3 is kind of tough to define with the definitions given above.   I believe that the proper explanation is out of your scope for know (from what I can deduce).   So, you'll learn that later on.  But for your info, NH3 is ammonia, the stuff they use in cleaning fluids, and it is basic.\n\nHope this helps.
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TSP is a solid.  You have to dissolve it to get a pH reading.   The pH will necessarily be dependent upon concentration and the pH of the solvent used.
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an acid is a proton donor while a base is a proton acceptor or an electron donor\n Hope i'm right
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Make a solution saturated with calcium hydroxide.  If there is precipitate calcium hydroxide then that means there is as much dissolved calcium hydroxide as possible.  Filter the solution to get rid of the solid.  Now you have a saturated solution, and your objective is to determine the molarity of this solution.  Measure the volume and keep track of this measurement.  To determine the number of moles of Ca(OH)2, titrate it with strong acid like HCl, and see when the pH reaches 7.  When you titrate, keep track of the amound of acid you are adding, and the current pH of the solution.  At pH=7, the number of moles of HCl you added is equal to the 1/2 the number of moles of Ca(OH)2 (because the molarity of H+ and OH- are equal).  Take this number of moles and divide it by the original volume.  This value is the concentration of hydroxide [OH-].  Half of this value is the concentration of calcium [Ca++].  Ksp = [Ca++]·[OH-]²
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Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+
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Sulfuric acid has a higher dissociation constant than acetic acid.  This means that more of it will dissociate in solution.\nAlso, sulfuric acid has 2 hydrogen atoms  that it can give up to solution vs. 1 from acetic acid.
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Acid + base = salt + water.\n\nUnbalanced eqn is: Al(OH)3 + H2CO3 --> Al2(CO3)3 + H2O
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acid has a ph value below 7\nand alkali has a value above 7\n\nAn acid (often represented by the generic formula HA) is traditionally considered any chemical compound that when dissolved in water, gives a solution with a pH of less than 7. That approximates the modern definition of Brønsted and Lowry, who defined an acid as a compound which donates a hydrogen ion (H+) to another compound (called a base). Common examples include acetic acid (in vinegar) and sulfuric acid (used in car batteries). Acids generally taste sour;\n\nIn chemistry, an alkali (from Arabic: al-qaly القالي) is a specific type of base, formed as a carbonate, hydroxide or other basic (pH greater than 7) ionic salt of an alkali metal or alkali earth metal element. The word alkali or the adjective alkaline are frequently used to refer to all bases, since most common bases are alkalis, although strictly speaking this is inaccurate.
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Depends on the manufacturer and the initiators they use. Usually, if its "acid free", it will say so on the box that you bought them in.
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a. by the proccess of titration.  few drops of universal indicator are poured onto the base. acid is poured  slowly with the help of the burette. when the base is decolourised this indicates that it has been neutralised.\n\nb. vinegar\nc. all of the above\nd. 7
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A standard solution is one that has been very carefully analyzed and characterized, usually by means traceable to a central standards bureau, such as NIST, so that the value is well known and can be trusted for instrument calibrations and methods development.\n\nA control sample uses known quantities of an analyte (it may be a standard, but does not have to be) so that analytical chemists can confirm that their processes are accurate and precise.\n\nFor example, I might have a standard buffer solution that I use to calibrate a pH meter on a regular basis, say daily.  Then, during each day, as I run dozens or hundreds of pH readings, I will periodically (say, once ever 20 tests), run a control sample through to make sure my readings are still in line with what I'd expect.  This gives the customer more confidence that the readings really match the real world situation.\n\nHope that helps.