For the pH question-pH is dependent on temperature. pH 7 is considered neutral at room temprature (25+273 K).- Nimish (age 17)Mumbai, India
The pH scale actually is based upon one more scale. We generally store track of the concentration of solutes in moles per liter (M). The pH is minus the log (base 10) of the H+ concentration in moles per liter. Because at room temperature in pure water, that concentration is exceptionally close to 10-7 M, pH 7 is neutral.Mike W.
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The over explacountries just define why water has a pH of 7, but not why this NEUTRAL.I think it is "neutral" bereason the concentration of hydroxide ions (OH-) is also 7 (pOH=7)and therefore balances out the concentration of hydrogen ions (pH=7).- Alan Bottomley (age 67)Hobart, Tasmania, Australia
That"s true. We implied that by describing the liquid as pure water, so that the formation of an H+ constantly goes along with the development of an OH-. In remedies through other ions (say Na+ or Cl-) there"s no such constraint, so the H+ and also OH- concentrations no longer equal. Hence NaOH creates a base, with several OH-, and HCl creates an acid, with lots of H+.Mike W.
Could you say that a solution via s pH = 7, neither contains H+ ions or OH– ions? Only H2O?- William (age 18)Norway
Nope. Several of the water molecules loss acomponent into ions. At concentrations of 10-7M H+ and also OH-, the rates of water falling apart and also ions recombining simply balance, so that"s the equilibrium concentration of those ions.Mike W.
OK, I think I follow all the answers so far... begin via H2O, one H+ for eextremely OH-, at room temperature that happens to be 10-7 for pH=7.But, what around various other temperatures? Does it follow that at 99C (or greater under pressure) that a "neutral" pH might not be 7 bereason the water might disassociate more at higher temperatures??Thanks for your answers.- Christopher (age 16)Greer, SC USA
Exactly. Here's a table of the neutral pH worths over a range of temperatures, obtained from the attach listed below. That site likewise has actually a nice discussion
My question has 2 parts:First, dissolving a strong base in water produce most OH-. I"m assuming that this does not change the hydrogen ion concentration. Why is the PH of a base bigger than 7?Second,At the equivalence suggest of a titration in between acetic acid (weak acid) and sodium hydroxide (strong base). The PH is roughly 9. This is because CH3COOH reacts with OH- created water and also CH3OO- which is a relatively solid conjugate base. CH3OO- react through water create some OH- for this reason increase the PH at the equivalence suggest. I wonder why can not the OH- produce in second reaction going back to be the reactant of the initially reaction? This method, fewer moles of NaOH than acetic acid will be necessary to include to the system to reach the endsuggest. Also, the endsuggest would still be organic. I know this hypothesis is wrong however please let me understand why.Thank you for taking the moment to answer this long question!- Alina Wang (age 17)Mechanicsburg, Pennsylmuzic-ivan.infoia, USA
The key point is that your presumption right here is wrong. "...create most OH-. I'm assuming that this does not adjust the hydrogen ion concentration." Some of the OH- combines via H+ to make ordinary H2O. At room temperature in equilibrium
I got a small lost in your second question, but probably the first answer will clarify it. For each reactivity there's an equlibrium reached, wbelow (approximately) the product of the concentrations of reactants on one side of the reactivity amounts to some constant time the product of the concentrations of reactants on the various other side. (In the products each reactant concentration is multiplied in the variety of times that the reactant appears in the reactivity formula.)
The reactions are maintained in dynamic equilibrium, wbelow both directions of reaction save happening, however in equilibrium the forward and also backward prices are equal.
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